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1) The document provides a chemistry exam for Class XII students with three sections - multiple choice questions, short answer questions, and descriptive answer questions.
2) The multiple choice section contains 16 questions testing concepts across the chemistry curriculum.
3) The short answer section contains 8 questions requiring students to provide explanations, equations, or names for various chemistry concepts.
4) The descriptive answer section provides 3 essay questions where students must explain processes, properties, or reactions in fuller detail. The exam aims to comprehensively test students' understanding of chemistry.
This document contains 8 stems with multiple chemistry questions below each stem. The stems provide chemical equations, molecular structures, names of compounds or lists of elements/compounds. Learners are asked questions testing their understanding of concepts like oxidation numbers, positions in the periodic table, bond formation, types of chemical reactions, and more. The questions require analyzing the information given in each stem and applying chemistry knowledge to explain, calculate, relate or derive requested information.
Here are the answers to the practice questions:
1. Displacement reaction
2. (g) indicates the substance is in gaseous state
3. By storing in air tight containers to prevent reaction with oxygen
4. CO2 dissolves in water to form carbonic acid which reacts with calcium hydroxide to form calcium carbonate, making the solution milky
5. Nitrogen
6. By the direction of the gas bubbles - oxygen bubbles up and hydrogen bubbles down
7. Photodecomposition of hydrogen chloride to form hydrogen and chlorine
8. In the displacement reaction, iron displaces copper from its solution. The iron nail becomes coated with copper and the blue
F.sc.2.Chemistry.Ch.05 Solved Test (Malik Xufyan)Malik Xufyan
1. The document contains questions from a chemistry test on Chapter 5 covering topics like halogens, noble gases, oxides and compounds.
2. Short answers are provided for questions asking about bleaching powder preparation, disproportionation reactions, iodized salt, uses of halogens, noble gas properties and more.
3. Longer answers discuss similarities and differences of fluorine, oxidizing properties of halogens, reactions of chlorine with sodium hydroxide, and industrial bleaching powder manufacture.
I. This document introduces chemical reactions and their key components:
II. A chemical reaction involves the rearrangement of atoms and conserves mass. Signs of a reaction include heat, gas, precipitate, or color changes.
III. Chemical equations are used to represent reactions, balancing the reactants and products. They use symbols to show quantities, identities, and states of substances involved.
FellowBuddy.com is a platform which has been setup with a simple vision, keeping in mind the dynamic requirements of students.
Our Vision & Mission - Simplifying Students Life
Our Belief - “The great breakthrough in your life comes when you realize it, that you can learn anything you need to learn; to accomplish any goal that you have set for yourself. This means there are no limits on what you can be, have or do.”
Like Us - https://www.facebook.com/FellowBuddycom-446240585585480
1) The document provides a chemistry exam for Class XII students with three sections - multiple choice questions, short answer questions, and descriptive answer questions.
2) The multiple choice section contains 16 questions testing concepts across the chemistry curriculum.
3) The short answer section contains 8 questions requiring students to provide explanations, equations, or names for various chemistry concepts.
4) The descriptive answer section provides 3 essay questions where students must explain processes, properties, or reactions in fuller detail. The exam aims to comprehensively test students' understanding of chemistry.
This document contains 8 stems with multiple chemistry questions below each stem. The stems provide chemical equations, molecular structures, names of compounds or lists of elements/compounds. Learners are asked questions testing their understanding of concepts like oxidation numbers, positions in the periodic table, bond formation, types of chemical reactions, and more. The questions require analyzing the information given in each stem and applying chemistry knowledge to explain, calculate, relate or derive requested information.
Here are the answers to the practice questions:
1. Displacement reaction
2. (g) indicates the substance is in gaseous state
3. By storing in air tight containers to prevent reaction with oxygen
4. CO2 dissolves in water to form carbonic acid which reacts with calcium hydroxide to form calcium carbonate, making the solution milky
5. Nitrogen
6. By the direction of the gas bubbles - oxygen bubbles up and hydrogen bubbles down
7. Photodecomposition of hydrogen chloride to form hydrogen and chlorine
8. In the displacement reaction, iron displaces copper from its solution. The iron nail becomes coated with copper and the blue
F.sc.2.Chemistry.Ch.05 Solved Test (Malik Xufyan)Malik Xufyan
1. The document contains questions from a chemistry test on Chapter 5 covering topics like halogens, noble gases, oxides and compounds.
2. Short answers are provided for questions asking about bleaching powder preparation, disproportionation reactions, iodized salt, uses of halogens, noble gas properties and more.
3. Longer answers discuss similarities and differences of fluorine, oxidizing properties of halogens, reactions of chlorine with sodium hydroxide, and industrial bleaching powder manufacture.
I. This document introduces chemical reactions and their key components:
II. A chemical reaction involves the rearrangement of atoms and conserves mass. Signs of a reaction include heat, gas, precipitate, or color changes.
III. Chemical equations are used to represent reactions, balancing the reactants and products. They use symbols to show quantities, identities, and states of substances involved.
This document provides instructions and questions for a chemistry exam for Class XII. It includes:
1. General instructions for the exam, such as it being compulsory, question types and marks.
2. 26 total questions ranging from very short answer to long answer questions covering topics in chemistry.
3. Contact information at the end for additional chemistry exam preparation assistance.
This document contains summaries of 4 class tests covering various chemistry topics:
1. A 10-mark chemical equilibrium test covering definitions of key terms like exothermic/endothermic reactions, degree of dissociation, and buffers. It also covers concepts like the dynamic nature of chemical equilibrium and Le Chatelier's principle.
2. A 10-mark test on chemical bonds covering definitions of ionic and covalent bonds, hybridization, the octet rule, and valence bond theory.
3. A 10-mark test on hydrogen covering its position in the periodic table, methods of production, isotopes, and physical properties.
4. A 10-mark test on organic chemistry basics covering industries
The document discusses different types of chemical reactions including precipitation, corrosion, metal displacement, combustion, decomposition, combination, and redox reactions. It provides examples of each type and asks 13 multiple choice and written response questions to test understanding of reaction types, equations, and products. Students are assessed on completing the questions with a grade scale of A for 12-13 correct, B for 8-11, C for 6-7, and D for less than 5.
1. Carbon exists in three allotropic forms: diamond, graphite, and fullerenes.
2. Diamond is extremely hard due to its rigid, three-dimensional covalent network structure where each carbon atom is bonded to four others in a tetrahedral shape. It is formed under high temperature and pressure deep in the Earth.
3. Diamond has many uses such as cutting, grinding, drilling, and jewelry due to its properties including hardness, high melting point, thermal conductivity, and brilliance when cut and polished. Synthetic diamonds are also produced for industrial applications.
This document provides an overview of basic chemistry concepts related to naming and writing formulas for ionic compounds. It discusses:
1) How to name ionic compounds by writing the cation first followed by the anion with "-ide" ending, except for polyatomic ions.
2) How to write formulas for ionic compounds by ensuring charges are balanced between cations and anions using subscripts.
3) Special rules for writing formulas involving polyatomic ions and d-block metal cations, which can have multiple oxidation states requiring specifying the oxidation number.
4) How to calculate formula masses of compounds by multiplying the number of atoms of each element by the atomic mass and summing the products.
The document discusses the Diels-Alder reaction, a [2+4] cycloaddition reaction discovered in 1928 by Otto Diels and Kurt Alder. It involves the addition of a conjugated diene and an alkene to form a six-membered ring. The reaction proceeds through a transition state with aromatic character involving the overlap of 6π electrons.
There are 5 general types of chemical reactions:
1. Synthesis reactions combine two or more substances to form one new substance.
2. Decomposition reactions break down a single substance into two or more new substances.
3. Combustion reactions involve burning and produce carbon dioxide, water, and other products.
4. Single displacement reactions involve one element replacing another in a compound.
5. Double displacement reactions involve the switching of cations and anions between two compounds.
This document discusses:
1) Transforming worded chemical equations into balanced chemical equations. Examples include iron reacting with bromine to form iron bromide and hydrogen chloride splitting into hydrogen and chlorine.
2) Classifying chemical equations as synthesis, analysis, single replacement, or double replacement reactions. Examples classified include ammonia forming from nitrogen and hydrogen (analysis) and calcium oxide reacting with carbon dioxide to form calcium carbonate (synthesis).
3) Calculating the molar mass of various compounds from their chemical formulas. Examples given are the molar mass of copper(II) sulfate, tin(III) chloride, magnesium oxide, sulfuric acid, and aluminum sulfide.
F.Sc.2.Chemistry.Ch.6.Test Solved - Malik XufyanMalik Xufyan
This document contains the solved test questions from Class 12 Chemistry Chapter 5 on transition elements and coordination compounds. It includes short answer questions covering topics such as the properties of transition elements, oxidation states, corrosion prevention methods, and the nomenclature and preparation of coordination compounds. The test also has longer answer questions on the manufacturing of steel via open hearth and Bessemer processes, electrochemical theory of corrosion, and properties of transition elements such as binding energies and atomic radii.
This document provides answers to summary questions about chemical reactions and kinetics experiments.
1) It describes two experiments where the rate of reaction between nitric acid and marble chips was measured using different concentrations of nitric acid. The rate was faster for the higher concentration as there were more collisions between reactants.
2) It also describes an experiment where the surface area of zinc reacting with hydrochloric acid was varied. Doubling the surface area doubled the rate of reaction through more frequent collisions.
3) Catalyst experiments are discussed where manganese dioxide increased the rate of hydrogen peroxide decomposition but was not used up in the reaction.
This document contains review questions about matter and changes in chemistry. It covers topics like physical and chemical properties, physical and chemical changes, states of matter, mixtures and compounds. Some key points addressed are:
- The difference between mixtures and compounds
- Properties of substances, mixtures and compounds
- Physical and chemical changes and what distinguishes them
- The three common states of matter
- Chemical symbols and formulas
1. The document provides a topical test with 6 questions about chemical equations and stoichiometric calculations. It asks the student to write chemical equations for reactions involving sodium, magnesium carbonate, aluminum, copper nitrate, and iron. It also asks the student to calculate relative molecular mass, mass of atoms, relative molecular mass of a gas, a combustion reaction of magnesium, and the volume and number of oxygen molecules from the decomposition of hydrogen peroxide.
The document provides a lesson plan on chemistry topics including:
1. Diagnostic questions, answering techniques, and the particulate nature of matter will be covered.
2. Answering techniques include short answers, active sentences, keywords, and relating topics like acids/bases.
3. The particulate nature of matter is explained using kinetic particle theory including the properties of solids, liquids, and gases. Particle movement and intermolecular forces are related to physical properties.
London dispersion forces are the attractive force between two molecules with hydrogen bonded to the oxygen atom. CH4 has dispersion forces as its only intermolecular force. Adsorption is the process of a substance sticking to the surface of another. Surface tension is the energy required to expand the surface area of a liquid by a unit amount of area. The vapor pressure of any substance at its normal boiling point is 1 atm. The concentration of nitrate ion in a solution containing 0.900 M aluminum nitrate is 2.70 M. Sublimination is the direct conversion of a solid to a gas.
Student Study Guide Physical Science 416/436Neil MacIntosh
This student study guide was prepared to help English students in the province prepare for their Physical Sciences 416/436 MEQ written examination. The guide was first prepared in 1996 and has undergone revisions in 1997, 1998, and 1999. It provides references to course materials and includes sample exam questions to help students study. The authors request that teachers provide feedback to help improve the guide. Special thanks are given to those involved in creating and revising the guide over the years.
6th Lecture on Elements of groups 16, 17 & 18 | Chemistry Part I | 12th StdAnsari Usama
This document discusses interhalogen compounds and xenon compounds. It provides an overview of interhalogen compounds, including their classification, general characteristics, states at 25°C, methods of preparation, properties, uses, and structures. It then discusses compounds of xenon, including preparation of xenon fluorides, reactions of XeF2, xenon trioxide, oxyfluorides of xenon, and the structures of xenon compounds.
This document outlines key concepts about molecules and compounds including:
1) Compounds have constant compositions with the same proportions of elements. Formulas represent atoms in molecules with subscripts.
2) Elements exist as single atoms or diatomic/polyatomic molecules. Molecular compounds form between nonmetals, while ionic compounds form between metals and nonmetals.
3) Formulas for ionic compounds contain positive and negative ions to be electrically neutral. Naming involves the cation name and anion name or polyatomic ion name.
The document contains a short quiz asking students to:
1. Write the chemical formulas for potassium nitrate, sodium sulphate, and copper(II) sulphate.
2. Write the chemical equation for the reaction between magnesium carbonate and hydrochloric acid, which forms magnesium chloride, water, and carbon dioxide.
3. Identify the anion in phosphide ion and the cation in magnesium ion from multiple choice options.
HAZARDOUS MATERIALSQuestion 1Polar substances are de.docxjosephineboon366
HAZARDOUS MATERIALS
Question 1
Polar substances are described as:
[removed]
a congregation of positive and negative charges on opposite ends of the molecules.
[removed]
molecules that are diatomic.
[removed]
molecules that possess only single atoms, also known as monatomic.
[removed]
molecules that only have positively charged ions.
5 points
Question 2
Decide why the heat from a candle flame is barely tolerable when a person places his or her hand above the candle compared to when the hand is placed next to the candle.
[removed]
The highest temperature is at the tip of the candle flame.
[removed]
Hot air rises upward, not sideways, by the mechanism of convection.
[removed]
Hot air rises upward, not sideways by the mechanism of conduction.
[removed]
The highest temperature is at the base of the candle flame.
5 points
Question 3
The fuel used in some racing cars contains isoamyl nitrite. Select which one of the characteristics below is classified as a chemical change/property?
[removed]
Isoamyl nitrite is a yellowish liquid having an ethereal odor.
[removed]
At 77
�
F (25
�
C) isoamyl nitrite has a specific gravity in the range 0.865-0.875
.
[removed]
Isoamyl nitrite is nearly insoluble in water.
[removed]
Isoamyl nitrite decomposes when exposed to light.
5 points
Question 4
The lead (Pb) concentration detected from a water-supply well is 0.15 mg/l (assume specific gravity of the well water is 1.0 at 25 deg C). If the drinking water standard is 15 ppb, what is your evaluation of this data?
[removed]
The Pb concentration is equivalent to 0.015 ppb and therefore meets the drinking water standard.
[removed]
The Pb concentration is equivalent to 15 ppb and therefore meets the drinking water standard.
[removed]
The Pb concentration is equivalent to 150 ppb and therefore does not meet the drinking water standard.
[removed]
The Pb concentration is equivalent to 1,500 ppb and therefore does not meet the drinking water standard.
5 points
Question 5
An area measuring 400 ft
�
120 ft is engulfed in a raging forest fire. During a single pass over the fire, a water-bearing helicopter drops sufficient water to extinguish a burning area measuring 20 m
�
20 m. Assuming the fire remains confined within the original area, how many passes must four helicopters make to extinguish the fire?
[removed]
3
[removed]
2
[removed]
4
[removed]
5
5 points
Question 6
The vaporization of the liquid elements of gasoline constitutes a __________ change.
Words:0
5 points
Question 7
Radon, which is a radioactive gas, is a member of the __________ gas family. Name one other element in this group or family: __________.
5 points
Question 8
Carbon disulfide is immiscible with water and sinks below the water because its specific gravity is __________ than 1.0.
5 points
Question .
This document provides instructions and questions for a chemistry exam for Class XII. It includes:
1. General instructions for the exam, such as it being compulsory, question types and marks.
2. 26 total questions ranging from very short answer to long answer questions covering topics in chemistry.
3. Contact information at the end for additional chemistry exam preparation assistance.
This document contains summaries of 4 class tests covering various chemistry topics:
1. A 10-mark chemical equilibrium test covering definitions of key terms like exothermic/endothermic reactions, degree of dissociation, and buffers. It also covers concepts like the dynamic nature of chemical equilibrium and Le Chatelier's principle.
2. A 10-mark test on chemical bonds covering definitions of ionic and covalent bonds, hybridization, the octet rule, and valence bond theory.
3. A 10-mark test on hydrogen covering its position in the periodic table, methods of production, isotopes, and physical properties.
4. A 10-mark test on organic chemistry basics covering industries
The document discusses different types of chemical reactions including precipitation, corrosion, metal displacement, combustion, decomposition, combination, and redox reactions. It provides examples of each type and asks 13 multiple choice and written response questions to test understanding of reaction types, equations, and products. Students are assessed on completing the questions with a grade scale of A for 12-13 correct, B for 8-11, C for 6-7, and D for less than 5.
1. Carbon exists in three allotropic forms: diamond, graphite, and fullerenes.
2. Diamond is extremely hard due to its rigid, three-dimensional covalent network structure where each carbon atom is bonded to four others in a tetrahedral shape. It is formed under high temperature and pressure deep in the Earth.
3. Diamond has many uses such as cutting, grinding, drilling, and jewelry due to its properties including hardness, high melting point, thermal conductivity, and brilliance when cut and polished. Synthetic diamonds are also produced for industrial applications.
This document provides an overview of basic chemistry concepts related to naming and writing formulas for ionic compounds. It discusses:
1) How to name ionic compounds by writing the cation first followed by the anion with "-ide" ending, except for polyatomic ions.
2) How to write formulas for ionic compounds by ensuring charges are balanced between cations and anions using subscripts.
3) Special rules for writing formulas involving polyatomic ions and d-block metal cations, which can have multiple oxidation states requiring specifying the oxidation number.
4) How to calculate formula masses of compounds by multiplying the number of atoms of each element by the atomic mass and summing the products.
The document discusses the Diels-Alder reaction, a [2+4] cycloaddition reaction discovered in 1928 by Otto Diels and Kurt Alder. It involves the addition of a conjugated diene and an alkene to form a six-membered ring. The reaction proceeds through a transition state with aromatic character involving the overlap of 6π electrons.
There are 5 general types of chemical reactions:
1. Synthesis reactions combine two or more substances to form one new substance.
2. Decomposition reactions break down a single substance into two or more new substances.
3. Combustion reactions involve burning and produce carbon dioxide, water, and other products.
4. Single displacement reactions involve one element replacing another in a compound.
5. Double displacement reactions involve the switching of cations and anions between two compounds.
This document discusses:
1) Transforming worded chemical equations into balanced chemical equations. Examples include iron reacting with bromine to form iron bromide and hydrogen chloride splitting into hydrogen and chlorine.
2) Classifying chemical equations as synthesis, analysis, single replacement, or double replacement reactions. Examples classified include ammonia forming from nitrogen and hydrogen (analysis) and calcium oxide reacting with carbon dioxide to form calcium carbonate (synthesis).
3) Calculating the molar mass of various compounds from their chemical formulas. Examples given are the molar mass of copper(II) sulfate, tin(III) chloride, magnesium oxide, sulfuric acid, and aluminum sulfide.
F.Sc.2.Chemistry.Ch.6.Test Solved - Malik XufyanMalik Xufyan
This document contains the solved test questions from Class 12 Chemistry Chapter 5 on transition elements and coordination compounds. It includes short answer questions covering topics such as the properties of transition elements, oxidation states, corrosion prevention methods, and the nomenclature and preparation of coordination compounds. The test also has longer answer questions on the manufacturing of steel via open hearth and Bessemer processes, electrochemical theory of corrosion, and properties of transition elements such as binding energies and atomic radii.
This document provides answers to summary questions about chemical reactions and kinetics experiments.
1) It describes two experiments where the rate of reaction between nitric acid and marble chips was measured using different concentrations of nitric acid. The rate was faster for the higher concentration as there were more collisions between reactants.
2) It also describes an experiment where the surface area of zinc reacting with hydrochloric acid was varied. Doubling the surface area doubled the rate of reaction through more frequent collisions.
3) Catalyst experiments are discussed where manganese dioxide increased the rate of hydrogen peroxide decomposition but was not used up in the reaction.
This document contains review questions about matter and changes in chemistry. It covers topics like physical and chemical properties, physical and chemical changes, states of matter, mixtures and compounds. Some key points addressed are:
- The difference between mixtures and compounds
- Properties of substances, mixtures and compounds
- Physical and chemical changes and what distinguishes them
- The three common states of matter
- Chemical symbols and formulas
1. The document provides a topical test with 6 questions about chemical equations and stoichiometric calculations. It asks the student to write chemical equations for reactions involving sodium, magnesium carbonate, aluminum, copper nitrate, and iron. It also asks the student to calculate relative molecular mass, mass of atoms, relative molecular mass of a gas, a combustion reaction of magnesium, and the volume and number of oxygen molecules from the decomposition of hydrogen peroxide.
The document provides a lesson plan on chemistry topics including:
1. Diagnostic questions, answering techniques, and the particulate nature of matter will be covered.
2. Answering techniques include short answers, active sentences, keywords, and relating topics like acids/bases.
3. The particulate nature of matter is explained using kinetic particle theory including the properties of solids, liquids, and gases. Particle movement and intermolecular forces are related to physical properties.
London dispersion forces are the attractive force between two molecules with hydrogen bonded to the oxygen atom. CH4 has dispersion forces as its only intermolecular force. Adsorption is the process of a substance sticking to the surface of another. Surface tension is the energy required to expand the surface area of a liquid by a unit amount of area. The vapor pressure of any substance at its normal boiling point is 1 atm. The concentration of nitrate ion in a solution containing 0.900 M aluminum nitrate is 2.70 M. Sublimination is the direct conversion of a solid to a gas.
Student Study Guide Physical Science 416/436Neil MacIntosh
This student study guide was prepared to help English students in the province prepare for their Physical Sciences 416/436 MEQ written examination. The guide was first prepared in 1996 and has undergone revisions in 1997, 1998, and 1999. It provides references to course materials and includes sample exam questions to help students study. The authors request that teachers provide feedback to help improve the guide. Special thanks are given to those involved in creating and revising the guide over the years.
6th Lecture on Elements of groups 16, 17 & 18 | Chemistry Part I | 12th StdAnsari Usama
This document discusses interhalogen compounds and xenon compounds. It provides an overview of interhalogen compounds, including their classification, general characteristics, states at 25°C, methods of preparation, properties, uses, and structures. It then discusses compounds of xenon, including preparation of xenon fluorides, reactions of XeF2, xenon trioxide, oxyfluorides of xenon, and the structures of xenon compounds.
This document outlines key concepts about molecules and compounds including:
1) Compounds have constant compositions with the same proportions of elements. Formulas represent atoms in molecules with subscripts.
2) Elements exist as single atoms or diatomic/polyatomic molecules. Molecular compounds form between nonmetals, while ionic compounds form between metals and nonmetals.
3) Formulas for ionic compounds contain positive and negative ions to be electrically neutral. Naming involves the cation name and anion name or polyatomic ion name.
The document contains a short quiz asking students to:
1. Write the chemical formulas for potassium nitrate, sodium sulphate, and copper(II) sulphate.
2. Write the chemical equation for the reaction between magnesium carbonate and hydrochloric acid, which forms magnesium chloride, water, and carbon dioxide.
3. Identify the anion in phosphide ion and the cation in magnesium ion from multiple choice options.
HAZARDOUS MATERIALSQuestion 1Polar substances are de.docxjosephineboon366
HAZARDOUS MATERIALS
Question 1
Polar substances are described as:
[removed]
a congregation of positive and negative charges on opposite ends of the molecules.
[removed]
molecules that are diatomic.
[removed]
molecules that possess only single atoms, also known as monatomic.
[removed]
molecules that only have positively charged ions.
5 points
Question 2
Decide why the heat from a candle flame is barely tolerable when a person places his or her hand above the candle compared to when the hand is placed next to the candle.
[removed]
The highest temperature is at the tip of the candle flame.
[removed]
Hot air rises upward, not sideways, by the mechanism of convection.
[removed]
Hot air rises upward, not sideways by the mechanism of conduction.
[removed]
The highest temperature is at the base of the candle flame.
5 points
Question 3
The fuel used in some racing cars contains isoamyl nitrite. Select which one of the characteristics below is classified as a chemical change/property?
[removed]
Isoamyl nitrite is a yellowish liquid having an ethereal odor.
[removed]
At 77
�
F (25
�
C) isoamyl nitrite has a specific gravity in the range 0.865-0.875
.
[removed]
Isoamyl nitrite is nearly insoluble in water.
[removed]
Isoamyl nitrite decomposes when exposed to light.
5 points
Question 4
The lead (Pb) concentration detected from a water-supply well is 0.15 mg/l (assume specific gravity of the well water is 1.0 at 25 deg C). If the drinking water standard is 15 ppb, what is your evaluation of this data?
[removed]
The Pb concentration is equivalent to 0.015 ppb and therefore meets the drinking water standard.
[removed]
The Pb concentration is equivalent to 15 ppb and therefore meets the drinking water standard.
[removed]
The Pb concentration is equivalent to 150 ppb and therefore does not meet the drinking water standard.
[removed]
The Pb concentration is equivalent to 1,500 ppb and therefore does not meet the drinking water standard.
5 points
Question 5
An area measuring 400 ft
�
120 ft is engulfed in a raging forest fire. During a single pass over the fire, a water-bearing helicopter drops sufficient water to extinguish a burning area measuring 20 m
�
20 m. Assuming the fire remains confined within the original area, how many passes must four helicopters make to extinguish the fire?
[removed]
3
[removed]
2
[removed]
4
[removed]
5
5 points
Question 6
The vaporization of the liquid elements of gasoline constitutes a __________ change.
Words:0
5 points
Question 7
Radon, which is a radioactive gas, is a member of the __________ gas family. Name one other element in this group or family: __________.
5 points
Question 8
Carbon disulfide is immiscible with water and sinks below the water because its specific gravity is __________ than 1.0.
5 points
Question .
This document discusses a lesson on polymerization. It includes objectives about hydrocarbons, saturated and unsaturated compounds, and addition polymerization. Students are asked questions to test their understanding, including defining hydrocarbons, the difference between saturated and unsaturated compounds, explaining the bromine test for alkenes, drawing formulas for ethene and its polymer, and modeling polymerization. The document provides feedback on student responses and discussion of polymer properties.
This document contains an exam for a first year engineering chemistry course. It includes two parts - Part A with 10 multiple choice questions worth 4 marks each, and Part B with 4 out of 6 long answer questions worth 10 marks each. The long answer questions cover topics like quantum numbers, acid-base theories, water treatment processes, polymerization reactions, and environmental pollution.
https://www.deped.gov.ph/wp-content/uploads/2019/01/General-Chemistry-1-and-2.pdf
General Chemistry
GenChem
STEM
Science, Technology, Engineering, and Mathematics
K to 12 Senior High School STEM Specialized Subject – General Chemistry 1 and 2
Quarter 1 – General Chemistry 1
Matter and Its Properties
Measurements
Atoms, Molecules and Ions
Stoichiometry
Percent Composition and Chemical Formulas
Chemical reactions and chemical equations
Mass Relationships in Chemical Reactions
Gases
Dalton’s Law of partial pressures
Gas stoichiometry
Kinetic molecular theory of gases
Quarter 2 – General Chemistry 1
Electronic Structure of Atoms
Electronic Structure and Periodicity
Chemical Bonding
Organic compounds
Quarter 3 – General Chemistry 2
Intermolecular Forces and Liquids and Solids
Physical Properties of Solutions
Thermochemistry
Chemical Kinetics
Quarter 4 – General Chemistry 2
Chemical Thermodynamics
Chemical Equilibrium
Acid-Base Equilibria and Salt Equilibria
Electrochemistry
1. The document outlines the course content and objectives for Engineering Chemistry & Environmental Studies. It covers topics such as fundamentals of chemistry, solutions, acids and bases, principles of metallurgy, electrochemistry, corrosion, water technology, polymers, and fuels.
2. The course aims to help students understand concepts related to atomic structure, chemical bonding, oxidation-reduction reactions, and calculations involving molarity, molality and normality of solutions. It also examines principles of metallurgy, electrochemistry, corrosion, water treatment processes and polymers.
3. Upon completing the course, students should be able to solve numerical problems, explain various chemical theories and industrial processes, and discuss the environmental impact
This document appears to be an exam for an engineering chemistry course. It contains 8 multiple choice questions across two parts (Part A and Part B). The questions cover topics like fuels and combustion, electrochemistry, corrosion, polymers, water analysis, and more. The maximum marks for the exam is 100. Students are instructed to answer 5 full questions by choosing at least 2 from each part, and to answer all objective type questions on the OMR sheet provided.
The document provides additional study material on value-based questions for Class 12 Chemistry in Delhi, India. It contains 37 questions related to chemistry concepts and applications that require identifying values such as safety, environmental protection, compassion, responsibility and integrity. The questions cover topics like scuba diving, cooking, osmosis, green chemistry, fuel cells, pollution, recycling, and more. They are intended to help students learn chemistry while also strengthening their understanding of important social and moral values.
This document contains an examination paper for Engineering Mathematics - II from December 2013/January 2014. It includes 8 questions with multiple choice and long answer questions. The topics covered include differential equations, Fourier series, Laplace transforms and partial differential equations. Students are required to answer 5 full questions by choosing at least two from each part. The paper tests the students' understanding of key concepts and their ability to solve problems in these topics.
This document is an exam for an engineering chemistry and environmental studies course. It contains 18 multiple choice questions across two sections. Section A contains 10 questions worth 4 marks each on topics like atomic structure, properties of ionic compounds, solutions, acids and bases, and electrolytes. Section B contains 4 out of 6 possible long-form questions worth 10 marks each, covering topics such as Bohr's atomic model, molarity, metal properties, electrolysis, corrosion, polymers, air pollution, and water hardness. Students are instructed to answer concisely in 5 sentences or less per short question and comprehensively for the long-form questions.
This document contains information about the II PUC Chemistry question bank and model question papers for the subject. It begins with a disclaimer noting that while efforts have been made to make the question bank comprehensive, errors may exist, and questions from the bank may not be the only ones appearing on examinations. It notes that the copyright of the question bank lies with the Director of the Department of Pre-University Education and it is for academic purposes only.
The document then provides the blueprints for two model question papers, outlining the distribution of questions from different topics across various parts of the papers. It allocates a total of 105 marks to the papers and divides them into parts A, B, C and D, with part A containing
Course Name (Legal Political and Ethical Dimensions of Business)MG.docxvanesaburnand
Course Name (Legal Political and Ethical Dimensions of Business)MGMT520
Week 2: Assignment Instructions
In each week the learning assignment is designed to demonstrate your competence with the Terminal Course Objectives of the course. Prior to working on the assignment, you should read through the week’s chapters and lesson.
Clearly identify your work with your name, the date, the week number and the assignment name, and upload work to the Dropbox.
The questions are designed to probe the higher levels of thinking and learning such as analyzing, evaluating and creating, and so there often are no “correct” answers. Instead of focusing and who wins or loses the case, you should analyze, evaluate and create alternative solutions to the various issues presented while arguing and debating the connections between business, law, politics and ethics.
Terminal Course Objective: G
Case Study: International and World Trade Law - Counterfeiting
Write a 1-2 page reflective paper (double spaced) on the following questions while discussing the connections between business, law, politics and ethics.
One: There has been a movement in the last decade encouraging people to “buy American.” Discuss the legal and ethical issues related to boycotting goods from other countries. What are the practical business implications of such a move?
Two: The World Trade Organization, or WTO, is the largest and most influential of the trade organizations. China and other heavy counterfeiting nations are part of this group. What could WTO-participating nations do to address the problems of counterfeiting? What should they do?
Three: The United Nations Security Council, the main decision-making body at the UN, is comprised of five regular members: China, France, the Russian Federation, the United Kingdom and the United States. Ten more members are elected from the General Assembly. Given the make-up of the committee, what type of action might the UN take with regard to the counterfeiting issue?
Submit your assignment to the Dropbox.
· 10165 - CHEM - 131 - Section 001 - Spring 2016 - General Chemistry Lec II
Top of Form
Question 1
Correct
Mark 3.00 out of 3.00
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Question text
All of the following are clues that a chemical reaction has taken place except
The reactant is smaller.
a.A flame occurs.
b.A color change occurs.
c. A solid forms.
Question 2
Question text
Balance the following equation in standard form and determine the sum of the coefficients.
a.6
b.4
c.3
d.14
e.7
Question 3
Question text
Balance this equation using the smallest possible integers, S + HNO3 → H2SO4 + NO2 + H2O. What is the coefficient of water.
Select one:
a.2
b.6
c.8
d. 1
e.
Question 4
Question text
When the following equation is balanced using the smallest possible integers, what is the coefficent of oxygen gas?
C7H16(g) + O2(g) → CO2(g) + H2O(g)
a.5
b.11
c.2
d.14
e.8
Question 5
Question text
True or false? The equation N2 + 3H2 → 2NH3 means that 1 g of N.
This document summarizes a technical seminar presentation on oxygen carriers used in chemical looping combustion. Chemical looping combustion is a process for carbon dioxide capture that uses metal oxides as oxygen carriers in two interconnected fluidized bed reactors - an air reactor and a fuel reactor. In the fuel reactor, gaseous fuel reacts with the metal oxide to produce carbon dioxide, water and heat. The reduced metal oxide is then reoxidized in the air reactor. Nickel, copper, iron and manganese are common oxygen carriers that must be stable, fluidizable, resistant to agglomeration and mechanically durable. The selection of oxygen carrier is a key aspect, with nickel oxide and iron oxide being favorable but having different properties and reactivities
F.Sc. Part 1 Chemistry Paper Faisalabad Board 2013 (Malik Xufyan)Malik Xufyan
1. The document contains a chemistry exam paper with multiple choice and subjective questions.
2. The multiple choice section has 17 questions testing concepts like the properties of different compounds, stoichiometry, gas laws, and acid-base chemistry.
3. The subjective section requires explaining concepts such as crystal structures, hybridization, kinetic molecular theory, X-rays, electrolysis, acid-base equilibria, and order of reactions. It also involves solving stoichiometry and pH problems.
This document is a chemistry exam from Puntland State of Somalia consisting of 9 sections with a total of 100 marks. It covers various chemistry concepts such as the electronic configurations of elements, chemical equations, enthalpy, organic compounds, and industrial processes like the Haber process. The exam tests the students' understanding of fundamental chemistry principles through multiple choice and structured questions requiring explanations and calculations.
Similar to Class 8 Cbse Chemistry Sample Paper Term 1 Model 2 (20)
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The document outlines the syllabus for various subjects in ICSE Class 1, including Mathematics, English, EVS, and Computer Applications. For Mathematics, topics range from pre-number concepts to addition, subtraction, measurement, money, and multiplication. English topics cover stories, poems, rhymes. EVS focuses on the child, family, school, neighborhood, environment. Computer Applications introduces basic computer parts and functions like the keyboard, mouse, and Paint software.
The document outlines the syllabus for various subjects in ICSE Class 1 including English, EVS, Computer Applications, and French. The English syllabus includes 10 chapters on topics like stories, poems, and rhymes. The EVS syllabus has 18 chapters covering topics about the self, family, community, environment and safety. The Computer Applications syllabus includes 8 chapters introducing students to basic computer parts and functions. The French syllabus has 11 chapters focusing on introducing students to French culture, language, numbers and school.
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This document provides a sample paper for an Environmental Studies exam with questions in three sections. Section A contains 10 one-mark multiple choice questions about national festivals, plants, animals, and seasons. Section B has 10 two-mark questions requiring short answers about holidays, occupations, the sun, and animals. Section C consists of 5 three-mark questions requiring longer answers about things that fly, water sources and uses, and plant-eating animals. The last question is worth 5 marks and asks how plants help humans.
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This presentation was provided by Steph Pollock of The American Psychological Association’s Journals Program, and Damita Snow, of The American Society of Civil Engineers (ASCE), for the initial session of NISO's 2024 Training Series "DEIA in the Scholarly Landscape." Session One: 'Setting Expectations: a DEIA Primer,' was held June 6, 2024.
ISO/IEC 27001, ISO/IEC 42001, and GDPR: Best Practices for Implementation and...PECB
Denis is a dynamic and results-driven Chief Information Officer (CIO) with a distinguished career spanning information systems analysis and technical project management. With a proven track record of spearheading the design and delivery of cutting-edge Information Management solutions, he has consistently elevated business operations, streamlined reporting functions, and maximized process efficiency.
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Class 8 Cbse Chemistry Sample Paper Term 1 Model 2
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Summative Assessment – Semester I
Chemistry
Class: 8 Max Mks: 45
Time: 2 hrs
Chapters included are Hydrogen, Carbon and Its Compounds and Structure of Atoms
General Instructions:
All questions are compulsory
Questions 1 to 5 are multiple-choice questions and carry 1 mark each. Choose the appropriate option
and write the answer in the answer sheet.
Question 6 to 10 carry 1 mark each and must be answered in 1 or 2 sentences.
Questions 11 to 19 carry 2 marks each must be answered in 2 or 3 sentences.
Questions 20 to 23 carry 3 marks each and must be answered in 5 or 6 sentences.
Question 24 carries 5 marks and must be answered in 7 or 8 sentences.
1. The product which is not obtained from the fractional distillation of crude petroleum is
(a) Kerosene oil
(b) Lubricating oil
(c) Linseed oil
(d) Diesel oil
2. The property due to which gases and liquids accumulate on the outer surface of solids is
(a) Absorption
(b) Adsorption
(c) Adhesion
(d) Cohesion
3. The maximum number of electrons in L shell are
(a) 2
(b) 18
(c) 32
(d) 8
4. Hydrogen removes metals from
(a) Metal substances
(b) Metal oxides
(c) Metal nitrates
(d) Metal sulphides
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5. The nuclear fuel in stars is
(a) Helium
(b) Hydrogen
(c) Carbon
(d) Carbon and oxygen
6. Name the radio isotope used in the cure of thyroid cancer.
7. Write the content of carbon in anthracite variety of coal.
8. Name the form of carbon used in gas masks.
9. Name a metal that does not react with dilute sulphuric acid.
10. A slow moving particle used for splitting nucleus of an atom of uranium is _________.
11. What do you understand by the term valency and variable valency.
12. State two uses of natural gas.
13. Define combustible substances. Give one example.
14. Every _________ parts of water by weight contain _________ part of hydrogen by weight.
15. Define radioactivity. Give four examples of radioactive elements.
16. State two advantages of biogas.
17. Describe your observation when hydrogen burns in air.
18. Write the properties of isotopes.
19. Write the composition of petroleum gas and natural gas.
20. Write the reactions of hydrogen with chlorine gas and metallic oxides.
21. (i) What is LPG? The LPG is an odorless gas, yet the gas supplied for domestic consumption smells.
Explain.
(ii) State the advantages of LPG as a domestic fuel.
(iii) State one important precaution in using LPG gas as domestic fuel.
22. How modern theory of atom contradicts Dalton’s atomic theory?
23. (i) What is petroleum?
(ii) Name five major fraction obtained and one use of each when petroleum is refined.
24. Prove that H2 is a reducing agent.