This document is a chemistry exam question paper focusing on electricity and chemistry. It contains 44 multiple choice questions testing understanding of key concepts such as:
- Substances used in electrical cables and why
- Products of electrolysis of various solutions and molten salts
- Electroplating and electrorefining processes
- Use of electrolysis in industrial processes like metal extraction
The document discusses the properties and extraction of sodium and its compounds. It describes that sodium is extracted through electrolysis of molten sodium chloride using the Downs process. Sodium reacts violently with water and acids, forming sodium hydroxide and hydrogen gas. Sodium hydroxide and sodium carbonate are important industrial compounds used to make paper, soap and glass.
Electroplating is a process where the surface of one metal is coated with a layer of a different metal. The metal being used to coat is less reactive than the one being coated. The anode is made from the pure metal used to coat, while the cathode is the object being electroplated. The electrolyte is an aqueous solution of a soluble salt of the pure metal at the anode. Electroplating is done to make metals more resistant to corrosion or damage and also to improve their appearance, such as chromium and nickel plating for resistance and silver plating cutlery for appearance.
Electrolytes are substances that can conduct electricity in the molten or liquid state and undergo chemical changes. Electrolysis is a process where electrolytes are broken down into their constituent elements by passing electricity through them. During electrolysis, ions migrate to the oppositely charged electrodes. At the anode, ions lose electrons and form gases or dissolve. At the cathode, ions gain electrons and form solid elements. Examples of electrolysis of molten lead(II) bromide and lead(II) oxide are described through their half reactions at the anode and cathode and overall reactions.
This document discusses electrolysis, which is the process of using direct current to cause non-spontaneous chemical reactions. Electrolysis requires an electrolyte containing free ions, a direct current power supply, and two electrodes. During electrolysis, ions are oxidized or reduced at the electrodes through electron transfer. As an example, electrolysis can be used to purify copper by dissolving impure copper and conducting electrolysis, depositing pure copper at the cathode. Electrolysis equations describe the half-reactions that occur at each electrode. The document also provides an example of electrolyzing brine to produce chlorine gas, hydrogen gas, and sodium hydroxide.
Checkpoint Lower Secondary Past Papers-P1 October-2017-sciencesmartexamresources
This document consists of a 16 page science exam for 11-12 year olds. It contains 12 multiple choice and short answer questions testing knowledge of topics like plant and animal cell structures, materials used in cars, light and color, food webs, chemical reactions, heat transfer, atoms, plant mineral absorption, soil properties, density, rabbit adaptations, and electrical circuits. Students are to write their answers directly in the exam paper.
The document discusses the chemical properties of alkali metals. It explains that alkali metals react vigorously with oxygen and water. The reactivity increases down the group as the atoms get larger, shielding the outer electrons from the nucleus and making them easier to lose. Equations for reactions of lithium, sodium, and potassium with oxygen, water, and other substances are provided. Flame tests for group 2 metals are also discussed.
This document provides information on tests for ions and gases from a chemistry course. It describes flame tests to identify Li+, Na+, K+, and Ca2+ cations, and tests using sodium hydroxide solution to detect NH4+ or produce precipitates of metal hydroxides to identify Cu2+, Fe2+, and Fe3+ cations. Anions can be identified by precipitates formed with silver nitrate and nitric acid for Cl-, Br-, or I-, barium chloride for SO42-, or by detecting carbon dioxide gas evolved from reaction with hydrochloric acid for CO32-. Common cations and anions are also listed.
1. The document is a chemistry exam paper focusing on molecules and covalent bonds. It contains 23 multiple choice questions testing understanding of covalent bonding, molecular structures, and properties of covalent and ionic compounds.
2. Key topics covered include electron dot diagrams of atoms, formation of covalent bonds via electron sharing, molecular geometry, and distinguishing between covalent and ionic bonding.
3. Questions require identifying bonding patterns in molecules like methane and water, writing molecular formulas, and understanding how atoms combine via electron transfers or sharing to form different types of chemical bonds and compounds.
The document discusses the properties and extraction of sodium and its compounds. It describes that sodium is extracted through electrolysis of molten sodium chloride using the Downs process. Sodium reacts violently with water and acids, forming sodium hydroxide and hydrogen gas. Sodium hydroxide and sodium carbonate are important industrial compounds used to make paper, soap and glass.
Electroplating is a process where the surface of one metal is coated with a layer of a different metal. The metal being used to coat is less reactive than the one being coated. The anode is made from the pure metal used to coat, while the cathode is the object being electroplated. The electrolyte is an aqueous solution of a soluble salt of the pure metal at the anode. Electroplating is done to make metals more resistant to corrosion or damage and also to improve their appearance, such as chromium and nickel plating for resistance and silver plating cutlery for appearance.
Electrolytes are substances that can conduct electricity in the molten or liquid state and undergo chemical changes. Electrolysis is a process where electrolytes are broken down into their constituent elements by passing electricity through them. During electrolysis, ions migrate to the oppositely charged electrodes. At the anode, ions lose electrons and form gases or dissolve. At the cathode, ions gain electrons and form solid elements. Examples of electrolysis of molten lead(II) bromide and lead(II) oxide are described through their half reactions at the anode and cathode and overall reactions.
This document discusses electrolysis, which is the process of using direct current to cause non-spontaneous chemical reactions. Electrolysis requires an electrolyte containing free ions, a direct current power supply, and two electrodes. During electrolysis, ions are oxidized or reduced at the electrodes through electron transfer. As an example, electrolysis can be used to purify copper by dissolving impure copper and conducting electrolysis, depositing pure copper at the cathode. Electrolysis equations describe the half-reactions that occur at each electrode. The document also provides an example of electrolyzing brine to produce chlorine gas, hydrogen gas, and sodium hydroxide.
Checkpoint Lower Secondary Past Papers-P1 October-2017-sciencesmartexamresources
This document consists of a 16 page science exam for 11-12 year olds. It contains 12 multiple choice and short answer questions testing knowledge of topics like plant and animal cell structures, materials used in cars, light and color, food webs, chemical reactions, heat transfer, atoms, plant mineral absorption, soil properties, density, rabbit adaptations, and electrical circuits. Students are to write their answers directly in the exam paper.
The document discusses the chemical properties of alkali metals. It explains that alkali metals react vigorously with oxygen and water. The reactivity increases down the group as the atoms get larger, shielding the outer electrons from the nucleus and making them easier to lose. Equations for reactions of lithium, sodium, and potassium with oxygen, water, and other substances are provided. Flame tests for group 2 metals are also discussed.
This document provides information on tests for ions and gases from a chemistry course. It describes flame tests to identify Li+, Na+, K+, and Ca2+ cations, and tests using sodium hydroxide solution to detect NH4+ or produce precipitates of metal hydroxides to identify Cu2+, Fe2+, and Fe3+ cations. Anions can be identified by precipitates formed with silver nitrate and nitric acid for Cl-, Br-, or I-, barium chloride for SO42-, or by detecting carbon dioxide gas evolved from reaction with hydrochloric acid for CO32-. Common cations and anions are also listed.
1. The document is a chemistry exam paper focusing on molecules and covalent bonds. It contains 23 multiple choice questions testing understanding of covalent bonding, molecular structures, and properties of covalent and ionic compounds.
2. Key topics covered include electron dot diagrams of atoms, formation of covalent bonds via electron sharing, molecular geometry, and distinguishing between covalent and ionic bonding.
3. Questions require identifying bonding patterns in molecules like methane and water, writing molecular formulas, and understanding how atoms combine via electron transfers or sharing to form different types of chemical bonds and compounds.
GIANT IONIC AND COVALENT STRUCTURES-GCSE.pdfFarhadAlsaeid
Giant covalent and ionic structures form when many atoms are bonded together in repeating patterns. Giant covalent structures include carbon materials like diamond and graphite, which have carbon atoms bonded together in tetrahedral or planar arrangements. Silicon dioxide also has a giant covalent structure where silicon atoms are bonded to four oxygen atoms in a repeating pattern. Giant ionic structures form crystalline ionic compounds where ions are bonded via electrostatic forces, such as sodium chloride which contains sodium and chloride ions. These giant structures have high melting points due to the large amount of energy required to overcome the numerous bonds between constituent atoms.
When sodium chloride dissolves in water, the ions separate from each other into positive sodium ions and negative chloride ions. This dissolving process can be represented by the equation NaCl(s) → Na+(aq) + Cl-(aq). The solubility of compounds is based on rules regarding which ions combine to form soluble or insoluble compounds. Compounds that do not dissolve in water and remain as a solid are considered precipitates, and chemical reactions where precipitates form are called precipitation reactions.
Electrochemistry class 12 ( a continuation of redox reaction of grade 11)ritik
Electrochemistry involves the study of chemical reactions that produce electricity and chemical reactions produced by electricity. A galvanic (voltaic) cell converts the chemical energy of a spontaneous redox reaction into electrical energy. Daniell's cell uses the redox reaction of zinc oxidizing copper ions to produce a cell potential of 1.1 V. An electrolytic cell uses an applied voltage to drive a nonspontaneous redox reaction in the opposite direction of the natural reaction in a galvanic cell. Standard reduction potentials allow prediction of the tendency of half-reactions to occur and their oxidizing or reducing power.
The document discusses the reactivity series of metals and how it is determined. The reactivity of a metal is based on its tendency to lose electrons and form positive ions. Experiments are conducted to see which metals react with water, acids, carbon, other metals, and metal ion solutions. These experiments allow metals to be ranked in a reactivity series from most reactive to least reactive. The reactivity series can then be used to predict and understand redox reactions between metals.
Biomolecules include carbohydrates, lipids, proteins, nucleic acids, and vitamins. Carbohydrates can be monosaccharides (such as glucose), oligosaccharides, or polysaccharides (such as starch and cellulose). Proteins are made of amino acids linked through peptide bonds. Important proteins include enzymes, antibodies, and hemoglobin. Nucleic acids such as DNA and RNA contain nucleotides and carry genetic information. Vitamins are organic compounds essential in small amounts for normal growth and activity.
1. The document is a 19-page syllabus approved for use in teaching physics in several countries.
2. It includes sample multiple choice exam questions covering topics in physics like motion, energy, electricity, waves and nuclear physics.
3. The questions are meant to test understanding of core physics concepts and include diagrams, graphs and calculations.
Memorize and Remember The Reactivity Series Using MnemonicsSancy See
Memorize and remember the reactivity series in order using mnemonics.
Easiest ways to remember reactivity series.
Reactivity series mnemonic funny.
Reactivity series of metals trick.
Mnemonics for reactivity series of metal.
This document provides information about alkali metals and describes the extraction and uses of sodium and sodium compounds. It discusses the periodic table classification of alkali metals. Key points include:
- Alkali metals are soft, silvery-white reactive metals found in Group 1 of the periodic table.
- Sodium is extracted commercially via the Downs process, which involves electrolysis of molten sodium chloride.
- Sodium reacts violently with water and is used to produce sodium hydroxide and other sodium compounds.
- Sodium hydroxide and sodium carbonate are manufactured via electrolysis or other chemical processes and have various industrial and household applications.
Electrolysis is a process where an electric current is passed through an electrolyte solution or molten salt, causing ions to migrate to the electrodes and undergo chemical reactions. During electrolysis, ions react at the electrodes by either gaining or losing electrons. Michael Faraday discovered that the mass of substance produced at the electrodes is directly proportional to the quantity of electricity passed through the electrolyte. His two laws of electrolysis state that the mass of substance liberated is directly proportional to the current over time, and that for the same quantity of electricity, the masses produced are proportional to the substances' equivalent masses. Electrolysis has many applications including metal extraction and coating materials with thin metal layers.
The document outlines key concepts and objectives for students to understand about electrolysis. It discusses how molten ionic compounds conduct electricity but solid ionic compounds do not due to mobile ions in liquids. Students should be able to state the direction of ion and electron movement during electrolysis, name products and write electrode reactions. They should also be able to predict and describe electrolysis products and processes like electroplating, copper refining and aluminum extraction. Worksheets are provided to reinforce these concepts through exercises on specific electrolysis reactions.
This document is from a KS3 Physics textbook. It provides information on electrical circuits, including introducing series and parallel circuits. Key points covered include:
- Series circuits have components connected in a single loop so the current is the same throughout. The voltage splits between components.
- Parallel circuits have multiple paths so the current can split and join at junctions. The voltage is the same across each part.
- Energy from batteries is transferred through electrical circuits and converted to other forms like light and heat in bulbs. The total energy transferred equals the chemical energy lost from the battery.
This chapter discusses ionic bonding. It begins by explaining that noble gases have a stable electronic configuration with a full outer shell. Most other elements form ions by gaining or losing electrons to achieve a noble gas configuration. Ionic bonds form when metals transfer electrons to non-metals to form positively charged cations and negatively charged anions. Ionic compounds have a crystalline structure where the ions are arranged in a repeating pattern with strong electrostatic forces between them. This results in ionic compounds having high melting points, being insoluble in organic solvents, and capable of conducting electricity when molten or dissolved in water.
The document describes various properties of metals. It discusses the physical properties of metals, including their high melting and boiling points, malleability, ductility, and ability to conduct heat and electricity well. It also describes alloys as mixtures of metals that are stronger than pure metals. Additionally, the document outlines some chemical properties of metals, such as their reactivity patterns and reactions with water, steam, and acids according to the reactivity series. It provides examples of equations to represent these reactions.
- Water is a polar solvent due to its molecular structure, with oxygen having a partial negative charge and hydrogen having partial positive charges. This allows it to dissolve ionic compounds by interacting with and separating the ions.
- Ionic compounds dissolve to varying degrees in water depending on how strongly the ions are attracted to each other versus water molecules. Solubility can be measured in g/L.
- Acids donate H+ ions in water and are classified as strong or weak based on how completely they ionize. Their strength affects pH calculations. Bases accept H+ and similarly ionize more or less completely.
Properties and Formation of Ionic Compounds PowerpointNeQuelle DeFord
Ionic compounds form when ions bond through electrostatic attraction. Metals form cations by losing electrons to achieve a full outer shell, while nonmetals form anions by gaining electrons. Cations and anions are attracted due to their opposite charges. Ionic compounds have high melting points, are crystalline solids, and dissolve in water due to the separation of ions. They do not conduct electricity as solids but do so as liquids or dissolved solutions.
Cambridge Lower Secondary Checkpoint Past Paper P2 October-2017-scienceSmart Exam Resources
This document consists of a 20 page science exam for students taking the Cambridge Secondary 1 Checkpoint exam. The exam contains 17 multiple choice and short answer questions testing knowledge of various science topics including the human body, states of matter, sound waves, biology, chemistry, physics, and ecology. Students are asked to interpret diagrams, graphs, tables of data and describe scientific processes and concepts.
This document discusses naming ionic compounds by first naming the cation and anion components. It provides rules for naming main group and transition metal cations, such as naming sodium as the "sodium cation" and copper as the "copper (II) cation". It also provides rules for naming anions by taking the root of the element name and adding "-ide", such as naming chloride and bromide anions. Examples and practice problems are given to demonstrate applying these rules to name common cations and anions.
This document contains a chemistry exam paper with questions about electrolysis and electricity. There are 30 multiple choice questions testing understanding of key concepts such as: products formed during the electrolysis of different substances like acids, salts and molten compounds; which electrodes specific elements are formed at; and why certain materials like copper, plastic and steel are used in electrical cables and circuits. The questions cover topics including electroplating, electrolysis of aqueous and molten solutions, and electrical safety.
This document discusses the electrolysis of brine solution (concentrated NaCl) to produce sodium hydroxide and chlorine gas. During electrolysis, sodium and hydrogen ions move to the cathode while chlorine and hydroxide ions move to the anode. At the cathode, only hydrogen ions are discharged to form hydrogen gas. At the anode, chlorine ions are discharged to form chlorine gas, leaving behind a solution of sodium hydroxide. A diaphragm cell is used to separately collect the chlorine gas and sodium hydroxide solution produced. Sodium hydroxide has uses including in soap production and paper making. Chlorine gas has uses as a bleaching agent and to produce hydrochlor
GIANT IONIC AND COVALENT STRUCTURES-GCSE.pdfFarhadAlsaeid
Giant covalent and ionic structures form when many atoms are bonded together in repeating patterns. Giant covalent structures include carbon materials like diamond and graphite, which have carbon atoms bonded together in tetrahedral or planar arrangements. Silicon dioxide also has a giant covalent structure where silicon atoms are bonded to four oxygen atoms in a repeating pattern. Giant ionic structures form crystalline ionic compounds where ions are bonded via electrostatic forces, such as sodium chloride which contains sodium and chloride ions. These giant structures have high melting points due to the large amount of energy required to overcome the numerous bonds between constituent atoms.
When sodium chloride dissolves in water, the ions separate from each other into positive sodium ions and negative chloride ions. This dissolving process can be represented by the equation NaCl(s) → Na+(aq) + Cl-(aq). The solubility of compounds is based on rules regarding which ions combine to form soluble or insoluble compounds. Compounds that do not dissolve in water and remain as a solid are considered precipitates, and chemical reactions where precipitates form are called precipitation reactions.
Electrochemistry class 12 ( a continuation of redox reaction of grade 11)ritik
Electrochemistry involves the study of chemical reactions that produce electricity and chemical reactions produced by electricity. A galvanic (voltaic) cell converts the chemical energy of a spontaneous redox reaction into electrical energy. Daniell's cell uses the redox reaction of zinc oxidizing copper ions to produce a cell potential of 1.1 V. An electrolytic cell uses an applied voltage to drive a nonspontaneous redox reaction in the opposite direction of the natural reaction in a galvanic cell. Standard reduction potentials allow prediction of the tendency of half-reactions to occur and their oxidizing or reducing power.
The document discusses the reactivity series of metals and how it is determined. The reactivity of a metal is based on its tendency to lose electrons and form positive ions. Experiments are conducted to see which metals react with water, acids, carbon, other metals, and metal ion solutions. These experiments allow metals to be ranked in a reactivity series from most reactive to least reactive. The reactivity series can then be used to predict and understand redox reactions between metals.
Biomolecules include carbohydrates, lipids, proteins, nucleic acids, and vitamins. Carbohydrates can be monosaccharides (such as glucose), oligosaccharides, or polysaccharides (such as starch and cellulose). Proteins are made of amino acids linked through peptide bonds. Important proteins include enzymes, antibodies, and hemoglobin. Nucleic acids such as DNA and RNA contain nucleotides and carry genetic information. Vitamins are organic compounds essential in small amounts for normal growth and activity.
1. The document is a 19-page syllabus approved for use in teaching physics in several countries.
2. It includes sample multiple choice exam questions covering topics in physics like motion, energy, electricity, waves and nuclear physics.
3. The questions are meant to test understanding of core physics concepts and include diagrams, graphs and calculations.
Memorize and Remember The Reactivity Series Using MnemonicsSancy See
Memorize and remember the reactivity series in order using mnemonics.
Easiest ways to remember reactivity series.
Reactivity series mnemonic funny.
Reactivity series of metals trick.
Mnemonics for reactivity series of metal.
This document provides information about alkali metals and describes the extraction and uses of sodium and sodium compounds. It discusses the periodic table classification of alkali metals. Key points include:
- Alkali metals are soft, silvery-white reactive metals found in Group 1 of the periodic table.
- Sodium is extracted commercially via the Downs process, which involves electrolysis of molten sodium chloride.
- Sodium reacts violently with water and is used to produce sodium hydroxide and other sodium compounds.
- Sodium hydroxide and sodium carbonate are manufactured via electrolysis or other chemical processes and have various industrial and household applications.
Electrolysis is a process where an electric current is passed through an electrolyte solution or molten salt, causing ions to migrate to the electrodes and undergo chemical reactions. During electrolysis, ions react at the electrodes by either gaining or losing electrons. Michael Faraday discovered that the mass of substance produced at the electrodes is directly proportional to the quantity of electricity passed through the electrolyte. His two laws of electrolysis state that the mass of substance liberated is directly proportional to the current over time, and that for the same quantity of electricity, the masses produced are proportional to the substances' equivalent masses. Electrolysis has many applications including metal extraction and coating materials with thin metal layers.
The document outlines key concepts and objectives for students to understand about electrolysis. It discusses how molten ionic compounds conduct electricity but solid ionic compounds do not due to mobile ions in liquids. Students should be able to state the direction of ion and electron movement during electrolysis, name products and write electrode reactions. They should also be able to predict and describe electrolysis products and processes like electroplating, copper refining and aluminum extraction. Worksheets are provided to reinforce these concepts through exercises on specific electrolysis reactions.
This document is from a KS3 Physics textbook. It provides information on electrical circuits, including introducing series and parallel circuits. Key points covered include:
- Series circuits have components connected in a single loop so the current is the same throughout. The voltage splits between components.
- Parallel circuits have multiple paths so the current can split and join at junctions. The voltage is the same across each part.
- Energy from batteries is transferred through electrical circuits and converted to other forms like light and heat in bulbs. The total energy transferred equals the chemical energy lost from the battery.
This chapter discusses ionic bonding. It begins by explaining that noble gases have a stable electronic configuration with a full outer shell. Most other elements form ions by gaining or losing electrons to achieve a noble gas configuration. Ionic bonds form when metals transfer electrons to non-metals to form positively charged cations and negatively charged anions. Ionic compounds have a crystalline structure where the ions are arranged in a repeating pattern with strong electrostatic forces between them. This results in ionic compounds having high melting points, being insoluble in organic solvents, and capable of conducting electricity when molten or dissolved in water.
The document describes various properties of metals. It discusses the physical properties of metals, including their high melting and boiling points, malleability, ductility, and ability to conduct heat and electricity well. It also describes alloys as mixtures of metals that are stronger than pure metals. Additionally, the document outlines some chemical properties of metals, such as their reactivity patterns and reactions with water, steam, and acids according to the reactivity series. It provides examples of equations to represent these reactions.
- Water is a polar solvent due to its molecular structure, with oxygen having a partial negative charge and hydrogen having partial positive charges. This allows it to dissolve ionic compounds by interacting with and separating the ions.
- Ionic compounds dissolve to varying degrees in water depending on how strongly the ions are attracted to each other versus water molecules. Solubility can be measured in g/L.
- Acids donate H+ ions in water and are classified as strong or weak based on how completely they ionize. Their strength affects pH calculations. Bases accept H+ and similarly ionize more or less completely.
Properties and Formation of Ionic Compounds PowerpointNeQuelle DeFord
Ionic compounds form when ions bond through electrostatic attraction. Metals form cations by losing electrons to achieve a full outer shell, while nonmetals form anions by gaining electrons. Cations and anions are attracted due to their opposite charges. Ionic compounds have high melting points, are crystalline solids, and dissolve in water due to the separation of ions. They do not conduct electricity as solids but do so as liquids or dissolved solutions.
Cambridge Lower Secondary Checkpoint Past Paper P2 October-2017-scienceSmart Exam Resources
This document consists of a 20 page science exam for students taking the Cambridge Secondary 1 Checkpoint exam. The exam contains 17 multiple choice and short answer questions testing knowledge of various science topics including the human body, states of matter, sound waves, biology, chemistry, physics, and ecology. Students are asked to interpret diagrams, graphs, tables of data and describe scientific processes and concepts.
This document discusses naming ionic compounds by first naming the cation and anion components. It provides rules for naming main group and transition metal cations, such as naming sodium as the "sodium cation" and copper as the "copper (II) cation". It also provides rules for naming anions by taking the root of the element name and adding "-ide", such as naming chloride and bromide anions. Examples and practice problems are given to demonstrate applying these rules to name common cations and anions.
This document contains a chemistry exam paper with questions about electrolysis and electricity. There are 30 multiple choice questions testing understanding of key concepts such as: products formed during the electrolysis of different substances like acids, salts and molten compounds; which electrodes specific elements are formed at; and why certain materials like copper, plastic and steel are used in electrical cables and circuits. The questions cover topics including electroplating, electrolysis of aqueous and molten solutions, and electrical safety.
This document discusses the electrolysis of brine solution (concentrated NaCl) to produce sodium hydroxide and chlorine gas. During electrolysis, sodium and hydrogen ions move to the cathode while chlorine and hydroxide ions move to the anode. At the cathode, only hydrogen ions are discharged to form hydrogen gas. At the anode, chlorine ions are discharged to form chlorine gas, leaving behind a solution of sodium hydroxide. A diaphragm cell is used to separately collect the chlorine gas and sodium hydroxide solution produced. Sodium hydroxide has uses including in soap production and paper making. Chlorine gas has uses as a bleaching agent and to produce hydrochlor
This document contains a chemistry exam paper focusing on air and water topics. It includes 38 multiple choice questions testing understanding of air composition, air pollution, and rusting processes. The questions cover causes of acid rain, the purpose of catalytic converters, formation of oxides of nitrogen in car engines, and methods of rust prevention like painting and galvanization.
This document provides the marking scheme for an electrochemistry exam consisting of multiple choice and structured questions.
Question 8 asks students to write the formula of ions present in different electrolytes, identify which ions are attracted to the anode and cathode, which ion is selectively discharged and why, and write the half reactions and observe the products at the electrodes.
Question 9 is similar to question 8 but provides a different electrolyte composition.
Question 10 asks about an electrolyte containing copper ions, the process occurring at the electrodes, and what would be observed to the electrolyte.
Question 11 provides an electrolyte and asks students to identify the positive and negative terminals, write reactions at each terminal, and observations made
This document provides an overview of electrochemistry concepts including:
- The differences between electrolytic and galvanic cells and how they convert between chemical and electrical energy.
- How standard electrode potentials are measured and used to determine the electrode potential of other electrodes relative to the standard hydrogen electrode.
- How galvanic cells work and the relationship between electrode potentials and the overall cell potential.
- The electrochemical series and how it arranges electrodes by their reduction potentials.
- How corrosion occurs via electrochemical reactions and how the presence of more or less reactive metals affects the corrosion of iron.
- Examples of primary batteries like dry cells and secondary batteries like lead-acid batteries, including their cell reactions.
This document outlines the key topics and concepts covered in a syllabus for a C5 Electricity & Chemistry course. It includes 9 points that describe electrolysis processes, products, and principles. Specifically, it covers how electrolysis breaks ionic compounds into simpler substances through the chemical effects of electricity. It also describes the use of electrodes, electrolytes, anodes and cathodes and how they relate to the reactions and products in different electrolysis examples, including molten salts, aqueous solutions, and metal refining. Finally, it mentions electroplating of metals and the industrial production of aluminum, chlorine, hydrogen and sodium hydroxide.
1. Electricity can affect substances in different ways depending on whether they are conductors, insulators, electrolytes or non-electrolytes. Conductors allow electric current to pass through due to mobile electrons, while insulators do not due to electrons locked in bonds.
2. Electrolysis is the decomposition of an electrolyte solution or melt by passing an electric current through it. At the anode, oxidation occurs as ions lose electrons. At the cathode, reduction occurs as ions gain electrons. Common electrolytes decomposed include NaCl, CuSO4 and acidified water.
3. During the electrolysis of molten lead(II) bromide, lead metal deposits at the cathode while bromine
7th Lecture on Electrochemistry | Chemistry Part I | 12th StdAnsari Usama
The document summarizes three types of rechargeable batteries: lead-acid, nickel-cadmium, and mercury batteries. It describes the electrode reactions, electrolytes, and applications of each battery type. Lead-acid batteries use lead and lead dioxide electrodes with sulfuric acid electrolyte and are used in cars and inverters. Nickel-cadmium batteries have cadmium and nickel oxide electrodes with an alkaline electrolyte and are used in small electronics. Mercury batteries contain zinc, mercury, and carbon electrodes with a paste electrolyte and provide a constant voltage for hearing aids and watches.
The document discusses different types of batteries, including nickel-cadmium, alkaline, lithium-iodine, mercury, and lead-acid batteries. It provides the chemical reactions, components, and properties of each battery type. In particular, it notes that nickel-cadmium and lead-acid batteries are rechargeable because their reaction products cling to the electrodes, allowing the reactions to be run in reverse when an external voltage is applied. Alkaline batteries are not rechargeable because their reaction products do not remain attached to the electrodes.
F.Sc. Part 1 Chemistry.Ch.10.Test (Malik Xufyan)Malik Xufyan
The document contains information about chemistry test series books published by Malik Xufyan of JIAS Academy, Jhang Institute for Advanced Studies. It lists the titles of 9 books covering chemistry courses from 9th class to F.Sc. Part II, which are available in both chapter-wise and board paper-wise test series formats. It also provides the contact information of the publisher.
New chm-152-unit-9-power-points-sp13-140227172048-phpapp02Cleophas Rwemera
This document discusses electrolysis and Faraday's law of electrolysis. It begins by introducing electrolytic cells and predicting the products of electrolysis. It then explains that according to Faraday's law, the amount of substance produced at each electrode is directly proportional to the quantity of electricity passing through the cell. The document provides an example calculation applying Faraday's law to determine the current needed in an electrolysis process. It also discusses some key aspects of Faraday's law, such as defining the faraday as one mole of electrons.
This document discusses electrochemistry and voltaic cells. It begins by defining electrochemistry as the interconversion of chemical and electrical energy. It then discusses electrolysis and voltaic cells. Electrolysis involves using electricity to break down substances, while voltaic cells convert chemical energy to electrical energy. The document goes on to describe the components and reactions of voltaic cells, including simple voltaic cells and Daniell cells. It also discusses applications of electrolysis in industries such as metal extraction and electroplating.
The document discusses corrosion and rusting of metals such as iron. It explains that rusting is the corrosion of iron caused by a redox reaction with oxygen and water to form iron(III) oxide. Rusting occurs faster in the presence of salts or acids as they provide electrolytes that allow electrons to transfer between reactants. Various methods are described to prevent corrosion through physical barriers or sacrificial protection of more reactive metals.
A student conducted an experiment using aluminium, iron, and copper metals and their sulfate salt solutions. Aluminium was found to be the most reactive metal as it displaced both iron and copper from their aqueous solutions. When barium chloride and sodium sulfate solutions were mixed, a white precipitate formed through a double displacement reaction. Heating lead nitrate produces yellow-brown lead oxide and brown nitrogen dioxide gas. Heating ferrous sulfate turns it from light green to brown and produces sulfurous oxide gas.
Electrolysis is the process of using electric current to cause non-spontaneous chemical changes. During electrolysis, ions are discharged at the electrodes. The key factors that determine which ions are discharged include the position of ions in the electrochemical series, concentration of ions, and type of electrode. Electrolysis has various industrial applications including electroplating, metal purification, and metal extraction.
Electrolysis is the process of using electric current to cause non-spontaneous chemical changes. During electrolysis, ions are discharged at the electrodes. The key factors that determine which ions are discharged include the position of ions in the electrochemical series, concentration of ions, and type of electrode. Electrolysis has important industrial applications such as electroplating, metal purification, and metal extraction.
Maths and sciience class 8 questions cbseTanvy Sharma
This document contains math and science questions for students. For math, it includes questions on expressing expressions as trinomials, finding identities, products, and simplifying expressions. For science, it discusses topics like strong vs. weak electrolytes, electroplating, identifying battery terminals using a potato, and explaining why a compass needle deflects more in sea water than drinking water due to conductivity. It also addresses safety concerns with electrical repairs during rain due to water conducting electricity.
This document provides an overview of redox reactions and electrochemistry applications. It discusses oxidation-reduction concepts like oxidation states and the OIL RIG mnemonic. Examples of redox reactions and electrochemistry applications are given, including galvanic cells, corrosion, electrolysis, and batteries. Key concepts covered include cell potential, the Nernst equation, and how concentration affects cell potential. Diagrams illustrate galvanic cells and how they function.
This document contains information about four experiments conducted to investigate the rate of reaction between solutions J and K and sulfuric acid at different temperatures. The key details are:
- Experiment 1 was conducted at room temperature and used as the baseline. Experiments 2-4 heated the mixture to increasing temperatures before adding solution K.
- The time taken for the mixtures to turn pale yellow was recorded.
- A line graph of time vs average temperature showed the rate of reaction increased with increasing temperature.
- Extrapolating the graph indicated a temperature of 60°C would yield a reaction time of around 15 seconds.
The document is a chemistry exam paper testing students' ability to identify ions and gases through laboratory tests. It describes tests carried out on various solid and liquid samples and asks students to identify the substances, describe observations, and draw conclusions. The paper tests knowledge of common chemical tests including flame tests, reactions of salts with acids and bases, and precipitation reactions to identify anion groups present. Students must analyze the provided data and apply their understanding of chemical reactions and properties to deduce the identities and nature of the unknown samples.
This document is a chemistry exam question paper that tests students' knowledge of types of oxides. It contains 16 multiple choice questions about classifying elements based on whether their oxides are acidic or basic, identifying properties of acidic and basic oxides, and predicting reactions of oxides with acids and bases. The questions cover topics like the positions of elements in the periodic table that relate to the acidity or basicity of their oxides, and common reactions of oxides like neutralization. The document also provides the grade boundaries for scoring the exam.
This document is a chemistry exam paper assessing knowledge of acids, bases and salts. It contains multiple choice and written response questions testing understanding of:
- Preparing soluble salts from insoluble bases and acids
- Properties of strong and weak acids
- Reactions of acids with metals, bases, carbonates and other salts
- Acid-base theories including proton transfer and pH
- Methods of salt preparation and properties of common oxides
This document contains information about acids, bases and salts. It includes questions about determining the reactivity series of metals through displacement reactions and measuring cell voltages. It also discusses properties of specific acids like malonic acid and sulfuric acid, and preparation of salts through various methods like precipitation, neutralization and titration. Example reactions provided include the reaction of magnesium with acids, and the reaction of ethylamine with iron(III) chloride that forms a brown precipitate.
This document provides a chemistry exam on acids, bases and salts from the Cambridge International Examinations board. It contains 21 multiple choice questions testing understanding of concepts such as the preparation of salts from reactions between acids and bases or metal oxides. Students are asked about the purpose of steps in salt preparation procedures, the products and reagents of different salt forming reactions, and the equipment used. The document also provides the grade boundaries for the exam.
1. The document is a biology exam paper covering the topic of coordination and response. It contains 50 multiple choice questions testing students' understanding of topics like reflex arcs, hormones, homeostasis, and plant tropisms.
2. The questions cover a range of concepts in human physiology and plant biology including the eye, skin, circulatory and nervous systems, temperature regulation, tropic responses, and hormonal coordination.
3. Additional resources for students can be found at the website savemyexams.co.uk which provides GCSE and A level materials across multiple subjects.
1. The document is an exam paper on acids and bases for IGCSE Chemistry. It contains 31 multiple choice questions testing knowledge of acid-base reactions and properties.
2. The questions cover topics like the characteristic properties of acids and bases, pH scales, acid-base indicators, and reactions like neutralization and those that produce carbon dioxide or ammonia gas.
3. Sample questions identify acids and bases, interpret acid-base titration curves, and write balanced equations for acid-base reactions.
This document contains a 25 question biology exam on coordination and response. It tests students' understanding of topics like reflexes, homeostasis, the nervous and endocrine systems, plant tropisms, and human physiology. Diagrams of biological structures like the eye, neurons, and plant shoots accompany several questions. The exam is scored out of 25 marks and is designed to take 30 minutes to complete.
This document contains an excerpt from a biology exam on coordination and response. It includes several multiple choice and short answer questions testing understanding of topics like the nervous system, reflexes, plant tropisms, homeostasis, and glucose regulation. Diagrams are provided of biological systems like the mammalian nervous system, a reflex arc, seedling growth responses, human skin response to cold, the liver and associated blood vessels, and control of blood glucose concentration. Students are asked to label parts, describe processes, explain concepts, and perform basic calculations.
This document contains a biology exam paper on coordination and response. It includes multiple choice and short answer questions testing understanding of topics like sensitivity, voluntary vs involuntary actions, reflex arcs, hormones, and how the nervous and endocrine systems coordinate organs and responses in the body. The exam is for IGCSE level and contains 58 minutes worth of content divided into 4 sections with a total possible score of 48 marks.
The students use a starting pistol, stopwatch, and measuring tape to measure the speed of sound. One student fires the starting pistol while the other times how long it takes the sound to travel a known distance measured with the tape. They calculate the speed of sound by dividing the distance traveled by the time taken.
The document contains multiple choice questions about sound waves and ultrasound. It covers topics like the range of human hearing, properties that determine the loudness and pitch of sounds, how echoes are produced, and using the speed of sound to calculate distances.
Ultrasound cannot be heard by humans because its frequency is too high. The range of audible sound frequencies for humans is typically 20 Hz to 20 kHz. A louder or higher pitched sound will have a greater amplitude and higher frequency respectively. Sound is a longitudinal wave that requires a medium, such as air or water, to travel through and be heard.
This document provides the mark scheme for an International General Certificate of Secondary Education (IGCSE) chemistry exam from May/June 2010. It shows teachers how to award marks to exam answers and serves as guidance, though alternative answers may be acceptable. The mark scheme details the requirements for each question on the exam paper and provides sample answers with marks allocated. CIE will not discuss or justify the mark scheme further.
This document is the mark scheme for the May/June 2010 International General Certificate of Secondary Education (IGCSE) Chemistry exam. It provides guidance to teachers on how to award marks for exam questions. The mark scheme indicates the requirements to receive marks and shows the basis on which examiners were instructed to award marks. It does not discuss the examiners' meetings before marking began. CIE will not enter into discussions about the mark schemes. CIE is publishing mark schemes for most IGCSE, GCE Advanced Level, and Advanced Subsidiary Level exams from May/June 2010.
This document consists of 16 pages related to a chemistry exam, including:
1. 15 multiple choice questions on chemistry topics
2. 1 blank page
3. Instructions for exam takers on how to fill out the multiple choice answer sheet.
This document provides instructions for a chemistry exam. It consists of 16 printed pages and covers topics like gases, hydrogen compounds, cobalt chloride, seawater compounds, fertilizers, metals and extraction, petroleum, and conductivity. Students are instructed to write their identification details on the paper and answer all questions in dark blue or black pen, using a pencil for diagrams. They should not use staples or correction fluid. The exam is 1 hour and 15 minutes long.
This document provides instructions for a chemistry exam. It tells students to write their identification information at the top, use dark ink or pencil for diagrams, and do not use staples or correction fluid. It lists the number of marks for each question. The exam contains 15 printed pages and 1 blank page. A periodic table is provided on page 16. Students should answer all questions and fasten their work together at the end.
This document provides the mark scheme for the May/June 2011 International General Certificate of Secondary Education (IGCSE) Chemistry exam. It lists the correct answers for the 40 multiple choice questions on the exam paper and is intended to guide teachers in marking the exam. The document also notes that Cambridge will not enter into discussions about the mark schemes and that they are publishing mark schemes for most IGCSE and other exam papers from May/June 2011.
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Walmart Business+ and Spark Good for Nonprofits.pdfTechSoup
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Beyond Degrees - Empowering the Workforce in the Context of Skills-First.pptxEduSkills OECD
Iván Bornacelly, Policy Analyst at the OECD Centre for Skills, OECD, presents at the webinar 'Tackling job market gaps with a skills-first approach' on 12 June 2024
A workshop hosted by the South African Journal of Science aimed at postgraduate students and early career researchers with little or no experience in writing and publishing journal articles.
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বাংলাদেশের অর্থনৈতিক সমীক্ষা ২০২৪ [Bangladesh Economic Review 2024 Bangla.pdf] কম্পিউটার , ট্যাব ও স্মার্ট ফোন ভার্সন সহ সম্পূর্ণ বাংলা ই-বুক বা pdf বই " সুচিপত্র ...বুকমার্ক মেনু 🔖 ও হাইপার লিংক মেনু 📝👆 যুক্ত ..
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LAND USE LAND COVER AND NDVI OF MIRZAPUR DISTRICT, UPRAHUL
This Dissertation explores the particular circumstances of Mirzapur, a region located in the
core of India. Mirzapur, with its varied terrains and abundant biodiversity, offers an optimal
environment for investigating the changes in vegetation cover dynamics. Our study utilizes
advanced technologies such as GIS (Geographic Information Systems) and Remote sensing to
analyze the transformations that have taken place over the course of a decade.
The complex relationship between human activities and the environment has been the focus
of extensive research and worry. As the global community grapples with swift urbanization,
population expansion, and economic progress, the effects on natural ecosystems are becoming
more evident. A crucial element of this impact is the alteration of vegetation cover, which plays a
significant role in maintaining the ecological equilibrium of our planet.Land serves as the foundation for all human activities and provides the necessary materials for
these activities. As the most crucial natural resource, its utilization by humans results in different
'Land uses,' which are determined by both human activities and the physical characteristics of the
land.
The utilization of land is impacted by human needs and environmental factors. In countries
like India, rapid population growth and the emphasis on extensive resource exploitation can lead
to significant land degradation, adversely affecting the region's land cover.
Therefore, human intervention has significantly influenced land use patterns over many
centuries, evolving its structure over time and space. In the present era, these changes have
accelerated due to factors such as agriculture and urbanization. Information regarding land use and
cover is essential for various planning and management tasks related to the Earth's surface,
providing crucial environmental data for scientific, resource management, policy purposes, and
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Accurate understanding of land use and cover is imperative for the development planning
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changes, conversion trends, and other related patterns. The spatial dimensions of land use and
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these patterns indicate shifts in economic and social conditions. Monitoring such changes with the
help of Advanced technologies like Remote Sensing and Geographic Information Systems is
crucial for coordinated efforts across different administrative levels. Advanced technologies like
Remote Sensing and Geographic Information Systems
9
Changes in vegetation cover refer to variations in the distribution, composition, and overall
structure of plant communities across different temporal and spatial scales. These changes can
occur natural.
it describes the bony anatomy including the femoral head , acetabulum, labrum . also discusses the capsule , ligaments . muscle that act on the hip joint and the range of motion are outlined. factors affecting hip joint stability and weight transmission through the joint are summarized.
How to Fix the Import Error in the Odoo 17Celine George
An import error occurs when a program fails to import a module or library, disrupting its execution. In languages like Python, this issue arises when the specified module cannot be found or accessed, hindering the program's functionality. Resolving import errors is crucial for maintaining smooth software operation and uninterrupted development processes.
1. 5.0 Electricity and Chemistry
Question Paper
Level IGCSE
Subject Chemistry(0620)
ExamBoard CambridgeInternationalExaminations(CIE)
Topic ElectricityandChemistry
Sub-Topic 5.0ElectricityandChemistry
Booklet QuestionPaper
Time Allowed: 60 minutes
Score: /51
Percentage: /100
Grade Boundaries:
A* A B C D E U
>85% 75% 60% 45% 35% 25% <25%
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2. 1 The diagram shows an electrical cable.
metal core
plastic coating
Which statement about the substances used is correct?
A The coating is plastic because it conducts electricity well.
B The core is copper because it conducts electricity well.
C The core is copper because it is cheap and strong.
D The core is iron because it is cheap and strong.
2 When substance X is electrolysed, the amount of gases P and Q formed is shown.
P Q
+–
substance X
What is substance X?
A concentrated aqueous sodium chloride
B concentrated hydrochloric acid
C dilute sulfuric acid
D molten lead(II) bromide
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3. 3 What are the products at the electrodes when dilute sulfuric acid is electrolysed using inert
electrodes?
4 Electricity is passed separately through concentrated hydrochloric acid, concentrated aqueous
sodium chloride and dilute sulfuric acid.
In which rows are the electrolysis products correctly named?
cathode product anode product
1 hydrogen chlorine
2 sodium chlorine
3
concentrated
hydrochloric acid
concentrated
aqueous sodium chloride
dilute sulfuric acid hydrogen oxygen
A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only
5 Which row describes the electrolysis of molten potassium bromide?
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4. 6 The diagram shows a section of an overhead power cable.
aluminium
steel
ceramic
Which statement explains why a particular substance is used?
A Aluminium has a low density and is a good conductor of electricity.
B Ceramic is a good conductor of electricity.
C Steel can rust in damp air.
D Steel is more dense than aluminium.
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5. 7 The diagram shows the electrolysis of concentrated hydrochloric acid and concentrated aqueous
sodium chloride using carbon electrodes.
–+ + –
electrode 2electrode 1
concentrated
hydrochloric acid
electrode 4electrode 3
concentrated aqueous
sodium chloride
At which electrode(s) is hydrogen produced?
A electrode 1 only
B electrodes 1 and 3
C electrode 2 only
D electrodes 2 and 4
8 What are the electrode products when molten silver iodide is electrolysed between inert
electrodes?
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6. 9 Copper and hydrogen can each be formed by electrolysis.
At which electrodes are these elements formed?
10 The diagram shows a failed attempt to copper-plate a pan.
pan
copper sulfate
solution
copper cathode
3V
+–
Which action will plate the pan with copper?
A cooling the copper sulfate solution in an ice bath
B heating the copper sulfate solution to boiling point
C increasing the voltage from 3V to 6V
D making the pan the cathode and the copper the anode
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7. 11 The diagram shows the electroplating of a steel object.
copper steel object
copper(II) sulfate solution
+ –
A student made the following statements.
1
2
3
The object turns a reddish-brown colour.
The copper sulfate solution changes to a paler blue colour.
The copper electrode becomes smaller.
Which statements are correct?
A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only
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8. 12 The diagram shows an electrolysis experiment.
electrode P
X
electrode Q
During the electrolysis, sodium was formed at electrode P and chlorine at electrode Q.
Which row correctly identifies P, Q and X?
P Q X
A anode cathode
B anode cathode
C cathode anode
D cathode anode
concentrated solution of
sodium chloride in water
molten sodium chloride
concentrated solution of
sodium chloride in water
molten sodium chloride
13 The diagram shows apparatus for plating a spoon with silver.
spoon metal electrode
electrolyte
Which statement is not correct?
A Silver would stick to the spoon because it is a very reactive metal.
B The electrolyte would be a silver salt dissolved in water.
C The metal electrode would be made from silver.
D The spoon would be connected to the negative terminal of the power supply.
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9. 14 Which metal could not be used for electroplating by using an aqueous solution?
A chromium
B copper
C silver
D sodium
15 Which products are formed at the electrodes when a concentrated solution of sodium chloride is
electrolysed?
16 A student wishes to electroplate an object with copper.
Which row is correct?
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10. 17 In the electrolysis shown, chlorine is produced at W and sodium at X.
+ –
XW
Y
Which labels are correct?
18 Which substance will not conduct electricity?
A aluminium
B copper
C plastic
D steel
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11. 19 Which products are formed at the anode and cathode when electricity is passed through molten
lead(II) bromide?
anode (+) cathode (–)
A
B
C
D
bromide ions
bromine molecules
lead atoms
lead ions
lead ions
lead atoms
bromine molecules
bromide ions
20 Electrical cables are made from either ……1……, because it is a very good conductor of
electricity, or from……2……, because it has a low density.
Overhead cables have a ……3…… core in order to give the cable strength.
Which words correctly complete gaps 1, 2 and 3?
21 What will be produced at the anode and at the cathode, if molten potassium chloride is
electrolysed?
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12. 22 The diagram shows the circuit for electrolysing lead(II) bromide and sodium chloride to liberate
the metal.
A
container for
lead(II) bromide
container for
sodium chloride
In what form are these salts electrolysed for liberating the metal?
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13. 23 The diagram shows the electrolysis of concentrated aqueous sodium chloride.
+
anode
–
cathode
concentrated
aqueous sodium
chloride and litmus
carbon
rods
What is the colour of the litmus at each electrode after five minutes?
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14. 24 Two electrolysis experiments were carried out as shown in the diagram below.
The graphite electrodes are labelled 1-4.
molten
sodium chloride
21 3 4
concentrated aqueous
sodium chloride
– ++ –
Which row describes the products at the electrodes in these experiments?
25 One molten compound and two aqueous solutions were electrolysed.
The table gives the compounds electrolysed and the electrodes used.
substance electrolysed electrodes
1 carbon
2 platinum
3
concentrated hydrochloric acid
concentrated sodium chloride
molten lead bromide platinum
In which experiments is a gas evolved at the cathode?
A 1, 2 and 3 B 1 and 2 only C 1 only D 3 only
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15. 26 The diagram shows an incomplete circuit.
glass tube
lamp
Which substance causes the lamp to light when added to the glass tube?
A aqueous sodium chloride
B aqueous sugar
C solid sodium chloride
D solid sugar
27 The diagram shows an electrical cable.
metal core
plastic coating
Which statement about the substances used is correct?
A The coating is plastic because it conducts electricity well.
B The core is copper because it conducts electricity well.
C The core is copper because it is cheap and strong.
D The core is iron because it is cheap and strong.
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16. 28 The diagram shows an electrolysis circuit.
At which electrode is hydrogen formed?
+ – + –
A B C D
aqueous
sodium
chloride
molten
sodium
chloride
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17. 29 Concentrated aqueous sodium chloride, concentrated hydrochloric acid and molten lead bromide
were separately electrolysed in experiments 1, 2 and 3.
platinum
electrodes
concentrated
aqueous
sodium
chloride
experiment 1
platinum
electrodes
concentrated
hydrochloric
acid
experiment 2
experiment 3
d.c. power supply
lamp
LEAD
BROMIDE
TOXIC
heat
Which statement about the electrode products is correct?
A Gases were given off at the anode in experiments 2 and 3 only.
B Gases were given off at the cathode in experiments 1 and 2 only.
C Metals were formed at the anode in experiments 1 and 3 only.
D Metals were formed at the cathode in experiments 1 and 3 only.
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18. 30 The diagram shows the electrolysis of concentrated aqueous sodium chloride.
–+
positive
electrode
negative
electrode
concentrated
aqueous sodium
chloride
carbon
rods
What is produced at each of the electrodes?
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19. 31 The diagram shows an electrolysis experiment using metals X and Y as electrodes.
aqueous solution
X Y
+ –
One of the metals becomes coated with copper.
Which metal becomes coated and which aqueous solution is used?
metal
aqueous
solution
A X Cr l3
B X Cu l2
C Y Cr l3
D Y Cu l2
32 In separate experiments, electricity was passed through concentrated aqueous sodium chloride
and molten lead bromide.
What would happen in both experiments?
A
B
C
D
A halogen would be formed at the anode.
A metal would be formed at the cathode.
Hydrogen would be formed at the anode.
Hydrogen would be formed at the cathode.
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20. 33 Winston Churchill, a British Prime Minister, had his false teeth electroplated with gold.
The teeth were coated with a thin layer of carbon and were then placed in the apparatus shown.
false teeth
switch
gold
aqueous solution
of a gold salt
X Y
Which row is correct?
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21. 34 The diagram shows that two gases are formed when concentrated hydrochloric acid is
electrolysed using inert electrodes.
+ve –ve
concentrated
hydrochloric acid
Which row correctly describes the colours of the gases at the electrodes?
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22. 35
aluminium
The diagram shows a section of an overhead power cable.
steel
glazed porcelain
Which statement explains why a particular substance is used?
A Aluminium has a low density and is a good conductor of electricity.
B Porcelain is a good conductor of electricity.
C Steel can rust in damp air.
D Steel is more dense than aluminium.
36 Metals could be extracted from their molten chlorides using electrolysis.
Which substances are formed at each electrode?
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23. 37 Concentrated aqueous potassium bromide solution is electrolysed using inert electrodes.
The ions present in the solution are K+
, Br–
, H+
and OH–
.
To which electrodes are the ions attracted during this electrolysis?
attracted to anode attracted to cathode
A H+
and OH–
B
Br–
and K+
Br–
and OH–
H+
and K+
C +
H and K+
D +
H and OH–
Br–
and OH–
Br–
and K+
38 Electricity from a power station passes through overhead cables to a substation and then to a
school where it is used to electrolyse concentrated hydrochloric acid using inert electrodes.
Which substances are used for the overhead cables and for the electrodes?
39 Which statement about the electrolysis of molten lead(II) bromide is correct?
A A colourless gas is seen at the cathode.
B A grey metal is seen at the anode.
C A red/brown gas is seen at the anode.
D A red/brown metal is seen at the cathode.
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24. 40 Electricity is passed through concentrated aqueous sodium chloride, as shown.
+ –
positive
electrode
negative
electrode
concentrated
aqueous sodium
chloride
carbon
rods
What is the test for the gas formed at the positive electrode?
A bleaches damp litmus paper
B ‘pops’ with a lighted splint
C relights a glowing splint
D turns damp red litmus paper blue
41 The diagram shows apparatus used in an attempt to electroplate a metal ring with copper.
+ –
copper electrode
aqueous copper(II)
sulfate (electrolyte)
metal ring
bulb
The experiment did not work.
What change is needed in the experiment to make it work?
A Add solid copper(II) sulfate to the electrolyte.
B Increase the temperature of the electrolyte.
C Replace the copper electrode by a carbon electrode.
D Reverse the connections to the battery.
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25. 42 When concentrated sodium chloride solution is electrolysed, elements X and Y are formed.
X
+–
Y
concentrated
sodium chloride
solution
What are X and Y?
43 Substance X was electrolysed in an electrolytic cell.
A coloured gas was formed at the anode and a metal was formed at the cathode.
cathode
substance X
anode
power supply
What is substance X?
A aqueous sodium chloride
B molten lead bromide
C molten zinc oxide
D solid sodium chloride
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26. 44 Aqueous copper(II) sulfate solution is electrolysed using inert electrodes.
2−
4SO ) areCopper(II) ions (Cu2+
), hydrogen ions (H+
), hydroxide ions (OH–
) and sulfate ions (
present in the solution.
To which electrodes are the ions attracted during this electrolysis?
attracted to anode attracted to cathode
A Cu2+
and H+
OH–
and 2−
4SO
B Cu2+
and 2−
4SO +
H and OH–
C +
H and OH–
Cu2+
and 2−
4SO
D OH–
and 2−
4SO Cu2+
and H+
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27. 45 Three electrolysis cells are set up. Each cell has inert electrodes.
The electrolytes are listed below.
cell 1
cell 2
cell 3
aqueous sodium chloride
concentrated hydrochloric acid
molten lead(II) bromide
In which cells is a gas formed at both electrodes?
A 1 and 2 B 1 and 3 C 2 only D 3 only
46 The diagram shows how aluminium is manufactured by electrolysis.
cathode (–ve)
molten aluminium
aluminium
oxide
dissolved in
cryolite
anode (+ve)
What are the anode and cathode made of?
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28. 47 The diagram shows the electrolysis of concentrated aqueous sodium chloride.
–+
positive
electrode
negative
electrode
concentrated
aqueous sodium
chloride and
Universal Indicator
carbon
rods
What is the colour of the Universal Indicator at each electrode after five minutes?
48 The diagram shows an electrical cable.
metal core
plastic coating
Which statement about the substances used is correct?
A The coating is plastic because it conducts electricity well.
B The core is copper because it conducts electricity well.
C The core is copper because it is cheap and strong.
D The core is iron because it is cheap and strong.
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29. 49 Aluminium is extracted from its oxide by electrolysis.
The oxide is dissolved in ……1…… cryolite and aluminium is deposited at the ……2……
Which words correctly complete gaps 1 and 2?
50 Molten lead(II) bromide is electrolysed as shown.
A
+ –
molten lead(II) bromide
Which ions are discharged at each electrode?
positive electrode negative electrode
A Pb+
Br2–
B Pb2+
Br–
C Br2–
Pb+
D Br–
Pb2+
51 Which of these elements could be formed at the anode when a molten salt is electrolysed?
A copper
B iodine
C lithium
D strontium
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