Sulphur dioxide can be prepared in the laboratory by adding dilute sulphuric acid to sodium sulphite. This produces sulphur dioxide gas along with sodium sulphate and water. Sulphur dioxide can be detected using acidified potassium dichromate solution, which turns from orange to green upon reaction. Excess sulphur dioxide bubbled through sodium hydroxide forms sodium hydrogen sulphite. Sulphur dioxide is used to manufacture sulphuric acid via the contact process, where it is oxidized to sulphur trioxide and absorbed in concentrated sulphuric acid.
Sulfuric acid is a highly corrosive and toxic mineral acid that is produced industrially via the contact process. It involves burning sulfur to produce sulfur dioxide, converting the sulfur dioxide to sulfur trioxide via reaction with oxygen over a vanadium catalyst, and then reacting the sulfur trioxide with water to form sulfuric acid. Sulfuric acid is a strong acid that is widely used in industry for processes like oil refining, fertilizer production, and metal processing due to its oxidizing and dehydrating properties. It can cause severe burns upon contact with skin or tissues.
This document provides instructions for preparing several common laboratory gases and chemicals. It describes how to produce carbon monoxide by heating oxalic acid crystals with concentrated sulfuric acid. Hydrogen iodide is prepared by dropping water onto a mixture of red phosphorus and iodine. Hydrogen gas is produced through the reaction of zinc and dilute sulfuric acid. Hydrogen sulfide gas can be prepared using iron sulfide and hydrochloric acid in Kipp's apparatus. Sulfur dioxide is formed from copper turnings and concentrated sulfuric acid. Ozone is generated by passing oxygen through an electric discharge. Physical and chemical properties are also outlined for each substance.
Sodium, magnesium, and aluminium react with oxygen to form ionic oxides. Sodium oxide and magnesium oxide are basic due to their oxide ions and react with water to form alkaline solutions. Aluminium oxide is amphoteric as it displays both acidic and basic properties, reacting with both acids and bases. Silicon dioxide does not react with water or acids due to its covalent bonding. Phosphorus and sulphur form acidic oxides that react with water to produce acids. Chlorine forms oxides that react with water to form acids or salts.
Sulfuric acid is produced through a multi-step process known as the contact process. First, sulfur or sulfur dioxide is obtained through burning sulfur or smelting sulfide ores. This is then converted to sulfur trioxide through reaction with oxygen over a vanadium pentoxide catalyst. The sulfur trioxide is absorbed into concentrated sulfuric acid to form oleum, and this is then diluted with water to produce sulfuric acid. Waste heat is recovered and gases are treated before emission to prevent environmental damage from the production of this important industrial chemical.
Sulfur exists in many forms including elemental sulfur and in compounds. It is a nonmetal that is extracted using the Frasch process. Sulfur has several allotropes depending on temperature and exists as S-8 rings at room temperature. Important sulfur compounds include sulfur dioxide, sulfur trioxide, hydrogen sulfide, and sulfuric acid. Sulfuric acid is the most widely produced sulfur compound and is used mainly in fertilizer production.
Sulfuric acid is a highly corrosive and toxic mineral acid that is produced industrially via the contact process. It involves burning sulfur to produce sulfur dioxide, converting the sulfur dioxide to sulfur trioxide via reaction with oxygen over a vanadium catalyst, and then reacting the sulfur trioxide with water to form sulfuric acid. Sulfuric acid is a strong acid that is widely used in industry for processes like oil refining, fertilizer production, and metal processing due to its oxidizing and dehydrating properties. It can cause severe burns upon contact with skin or tissues.
This document provides instructions for preparing several common laboratory gases and chemicals. It describes how to produce carbon monoxide by heating oxalic acid crystals with concentrated sulfuric acid. Hydrogen iodide is prepared by dropping water onto a mixture of red phosphorus and iodine. Hydrogen gas is produced through the reaction of zinc and dilute sulfuric acid. Hydrogen sulfide gas can be prepared using iron sulfide and hydrochloric acid in Kipp's apparatus. Sulfur dioxide is formed from copper turnings and concentrated sulfuric acid. Ozone is generated by passing oxygen through an electric discharge. Physical and chemical properties are also outlined for each substance.
Sodium, magnesium, and aluminium react with oxygen to form ionic oxides. Sodium oxide and magnesium oxide are basic due to their oxide ions and react with water to form alkaline solutions. Aluminium oxide is amphoteric as it displays both acidic and basic properties, reacting with both acids and bases. Silicon dioxide does not react with water or acids due to its covalent bonding. Phosphorus and sulphur form acidic oxides that react with water to produce acids. Chlorine forms oxides that react with water to form acids or salts.
Sulfuric acid is produced through a multi-step process known as the contact process. First, sulfur or sulfur dioxide is obtained through burning sulfur or smelting sulfide ores. This is then converted to sulfur trioxide through reaction with oxygen over a vanadium pentoxide catalyst. The sulfur trioxide is absorbed into concentrated sulfuric acid to form oleum, and this is then diluted with water to produce sulfuric acid. Waste heat is recovered and gases are treated before emission to prevent environmental damage from the production of this important industrial chemical.
Sulfur exists in many forms including elemental sulfur and in compounds. It is a nonmetal that is extracted using the Frasch process. Sulfur has several allotropes depending on temperature and exists as S-8 rings at room temperature. Important sulfur compounds include sulfur dioxide, sulfur trioxide, hydrogen sulfide, and sulfuric acid. Sulfuric acid is the most widely produced sulfur compound and is used mainly in fertilizer production.
Chlorine and its compounds are discussed. Chlorine can be prepared in the laboratory by reacting concentrated hydrochloric acid with manganese(IV) oxide or potassium manganate(VII). Chlorine is a greenish-yellow gas that is denser than air and acts as a strong oxidizing agent and bleach. It reacts with many metals and non-metals to form chlorides. Common uses of chlorine include water disinfection and manufacturing of bleaches, plastics and pesticides.
This document discusses various oxyacids of sulfur. It begins by defining oxyacids of sulfur as compounds containing sulfur, hydrogen and oxygen. It then lists and describes 9 common oxyacids of sulfur - sulphurous acid, sulphuric acid, peroxomonosulphuric acid, peroxodisulphuric acid, thiosulphuric acid, dithionous acid, dithionic acid, polythionic acid and pyrosulphuric acid. The document focuses on describing the structure, methods of preparation, properties and uses of the most important oxyacids - sulphurous acid and sulphuric acid.
Sulfuric acid is produced via the contact process, which involves three main steps:
1) Sulfur is burned to produce sulfur dioxide gas.
2) Sulfur dioxide is converted to sulfur trioxide gas over a vanadium pentoxide catalyst.
3) Sulfur trioxide is dissolved in concentrated sulfuric acid to form oleum, which is then diluted with water to produce 98% sulfuric acid.
H2 S and SO2 removal and possible valorizationSerge Vigneron
H2S is a common pollutant in gas and air. This presentation is a review of different techniques to remove H2S ,and possible ways of valorization to sulfuric acid via SO2.
4th Lecture on Elements of groups 16, 17 & 18 | Chemistry Part I | 12th StdAnsari Usama
The document provides information about sulfur dioxide (SO2) and sulfuric acid (H2SO4). It discusses the preparation, physical and chemical properties, structure, and uses of SO2. The preparation of H2SO4 using the contact process is described. The physical properties, acidic and dehydrating nature, and reactions of H2SO4 are covered. Important industrial uses of H2SO4 are also mentioned.
This document provides a 22 question practice exam on the preparation of salts from acids and bases/metal oxides/carbonates. It tests understanding of the key steps in salt preparation including addition of excess reactant, filtration, evaporation and crystallization. Questions cover the preparation of specific salts such as copper(II) sulfate, magnesium sulfate and ammonium sulfate.
Step 3 is to ensure all of the acid has reacted by adding copper(II) oxide in excess. Step 4 is to remove any unreacted excess copper(II) oxide by filtering.
This document summarizes the contact process for producing sulfuric acid. It involves three main steps: 1) sulfur is burned to produce sulfur dioxide, 2) the sulfur dioxide is converted to sulfur trioxide in the presence of a catalyst, and 3) the sulfur trioxide is dissolved in concentrated sulfuric acid to produce oleum, which is then diluted with water to form concentrated sulfuric acid. The major raw materials are sulfur, air, and water. Sulfuric acid has many industrial uses such as fertilizer and metal production.
1. Qualitative inorganic analysis involves the detection and identification of anions in samples. Anions are divided into six groups including carbonates, sulphur-containing anions, halides, cyanogen, arsenic/phosphorus, and nitrogen-containing.
2. Carbonates and bicarbonates react with acids to produce carbon dioxide gas. Sulphur-containing anions such as sulphides, sulphites, thiosulphates and sulphates are identified through reactions that produce precipitates, gases, or color changes with reagents like barium chloride, silver nitrate, and iron (III) chloride.
3. Common tests involve observing properties like solubility, as
Nitrogen and its compounds can be prepared through several laboratory methods. Nitrogen gas can be obtained by removing oxygen from air using heated copper turnings, leaving only nitrogen. Ammonia gas is commonly prepared by heating a mixture of ammonium chloride and calcium hydroxide. Ammonia is generally unreactive but will burn or react with substances like oxygen, hydrogen chloride, and metals/metal oxides. It is widely used to manufacture fertilizers and explosives.
Carbon dioxide is a colorless, odorless gas composed of carbon and oxygen that constitutes about 0.041% of the atmosphere. It was first observed in the 17th century by Jan Baptist Van Helmont during a charcoal burning experiment. Carbon dioxide has a linear molecular shape with a bond angle of 180 degrees. It is diamagnetic with no dipole moment due to its molecular structure. Carbon dioxide is used in many applications including fire extinguishers, refrigeration, winemaking, and enhancing the hardness of metal castings. It can be prepared in the laboratory by reacting calcium carbonate with hydrochloric acid.
The document provides information about various chemistry concepts related to air and water:
- It describes chemical tests to identify water and the purification of water supplies through filtration and chlorination.
- The composition of clean air is described as 78% nitrogen, 21% oxygen and small quantities of other gases. Common air pollutants like carbon monoxide and their sources are stated.
- Fractional distillation is outlined as the process used to separate oxygen and nitrogen from liquid air based on their different boiling points.
- Rusting is described as a reaction between iron, air and water that can be prevented by methods like painting and galvanizing to exclude oxygen.
Carbon dioxide was discovered by Van Helmont and proved to be an oxide of carbon by Antoine Lavoisier. It can be prepared by heating carbon or fuels like methane, or by heating carbonates like calcium carbonate. It is a colorless, odorless gas that is heavier than air and turns limewater milky. It is used in carbonated drinks, fire extinguishers, by plants during photosynthesis, and to preserve foods like meat and vegetables.
Acid deposition occurs when sulfur dioxide and nitrogen oxides emitted from the burning of fossil fuels react with water, oxygen, and other chemicals in the atmosphere to form acids. These acids can fall to Earth as rain, snow, fog or dry particles. Natural processes also produce acid deposition, but human activities such as burning coal and oil have increased acid deposition levels. Acid rain has a pH lower than 5.6 and can damage sensitive forests and lakes. The main pollutants that cause acid rain are sulfur dioxide and nitrogen oxides.
Preparation of salts (multiple choice) qpRubaHusain
Step 3 is to ensure all of the acid has reacted by adding copper(II) oxide in excess. Step 4 is to remove any excess copper(II) oxide by filtration to obtain pure copper(II) sulfate crystals.
The correct sequence of steps is: dissolving → filtration → evaporation → crystallisation.
Salts can be prepared by reacting dilute acids with metals, bases, or carbonates. Copper(II) chloride could be prepared by reacting copper with hydrochloric acid or by reacting copper carbonate with hydrochloric acid.
1. Dilute hydrochloric acid was used to react with various substances including copper oxide, iron nails, magnesium strips, and egg shells. These reactions all produced observable changes and gaseous products like hydrogen and carbon dioxide.
2. The acid reacted with the copper oxide on a coin, removing the layer to expose bare copper. Reactions with iron nails removed rust and bubbles formed, while magnesium vigorously reacted with bubbles. Egg shells reacted to produce carbon dioxide bubbles.
3. Additional details are provided about the chemical reactions, products, and observations for each substance tested with the hydrochloric acid.
1. Photosynthesis converts sunlight into chemical energy through two stages - the light-dependent reactions which produce ATP and NADPH using chlorophyll, and the light-independent Calvin cycle which uses these products to fix carbon and produce glucose.
2. The light-dependent reactions take place in the thylakoid membranes of the chloroplast and involve the absorption of light by photosystems and electron transport chains to generate a proton gradient for ATP synthesis via chemiosmosis.
3. The light-independent Calvin cycle occurs in the chloroplast stroma and uses the ATP and NADPH from the light reactions to reduce carbon dioxide and produce glucose through a series of reduction
1. Photosynthesis converts sunlight into chemical energy through light-dependent and light-independent reactions. 2. The light-dependent reactions use sunlight to produce ATP and NADPH through electron transport. 3. The light-independent Calvin cycle uses ATP and NADPH to fix carbon from CO2 into organic three-carbon sugars like G3P.
The document discusses activities of integration, which are assessments that evaluate students' ability to solve problems by integrating knowledge from a chapter. It provides examples of activities of integration, such as writing a letter inviting teachers to an end-of-year party. It also discusses the components of activities of integration, such as the problem/scenario and expected output. Additionally, it covers how to develop an assessment grid to score activities of integration based on relevance, accuracy, coherence and excellence. Teachers are then instructed to work in groups to create an activity of integration for any S1 topic along with its corresponding assessment grid.
Chlorine and its compounds are discussed. Chlorine can be prepared in the laboratory by reacting concentrated hydrochloric acid with manganese(IV) oxide or potassium manganate(VII). Chlorine is a greenish-yellow gas that is denser than air and acts as a strong oxidizing agent and bleach. It reacts with many metals and non-metals to form chlorides. Common uses of chlorine include water disinfection and manufacturing of bleaches, plastics and pesticides.
This document discusses various oxyacids of sulfur. It begins by defining oxyacids of sulfur as compounds containing sulfur, hydrogen and oxygen. It then lists and describes 9 common oxyacids of sulfur - sulphurous acid, sulphuric acid, peroxomonosulphuric acid, peroxodisulphuric acid, thiosulphuric acid, dithionous acid, dithionic acid, polythionic acid and pyrosulphuric acid. The document focuses on describing the structure, methods of preparation, properties and uses of the most important oxyacids - sulphurous acid and sulphuric acid.
Sulfuric acid is produced via the contact process, which involves three main steps:
1) Sulfur is burned to produce sulfur dioxide gas.
2) Sulfur dioxide is converted to sulfur trioxide gas over a vanadium pentoxide catalyst.
3) Sulfur trioxide is dissolved in concentrated sulfuric acid to form oleum, which is then diluted with water to produce 98% sulfuric acid.
H2 S and SO2 removal and possible valorizationSerge Vigneron
H2S is a common pollutant in gas and air. This presentation is a review of different techniques to remove H2S ,and possible ways of valorization to sulfuric acid via SO2.
4th Lecture on Elements of groups 16, 17 & 18 | Chemistry Part I | 12th StdAnsari Usama
The document provides information about sulfur dioxide (SO2) and sulfuric acid (H2SO4). It discusses the preparation, physical and chemical properties, structure, and uses of SO2. The preparation of H2SO4 using the contact process is described. The physical properties, acidic and dehydrating nature, and reactions of H2SO4 are covered. Important industrial uses of H2SO4 are also mentioned.
This document provides a 22 question practice exam on the preparation of salts from acids and bases/metal oxides/carbonates. It tests understanding of the key steps in salt preparation including addition of excess reactant, filtration, evaporation and crystallization. Questions cover the preparation of specific salts such as copper(II) sulfate, magnesium sulfate and ammonium sulfate.
Step 3 is to ensure all of the acid has reacted by adding copper(II) oxide in excess. Step 4 is to remove any unreacted excess copper(II) oxide by filtering.
This document summarizes the contact process for producing sulfuric acid. It involves three main steps: 1) sulfur is burned to produce sulfur dioxide, 2) the sulfur dioxide is converted to sulfur trioxide in the presence of a catalyst, and 3) the sulfur trioxide is dissolved in concentrated sulfuric acid to produce oleum, which is then diluted with water to form concentrated sulfuric acid. The major raw materials are sulfur, air, and water. Sulfuric acid has many industrial uses such as fertilizer and metal production.
1. Qualitative inorganic analysis involves the detection and identification of anions in samples. Anions are divided into six groups including carbonates, sulphur-containing anions, halides, cyanogen, arsenic/phosphorus, and nitrogen-containing.
2. Carbonates and bicarbonates react with acids to produce carbon dioxide gas. Sulphur-containing anions such as sulphides, sulphites, thiosulphates and sulphates are identified through reactions that produce precipitates, gases, or color changes with reagents like barium chloride, silver nitrate, and iron (III) chloride.
3. Common tests involve observing properties like solubility, as
Nitrogen and its compounds can be prepared through several laboratory methods. Nitrogen gas can be obtained by removing oxygen from air using heated copper turnings, leaving only nitrogen. Ammonia gas is commonly prepared by heating a mixture of ammonium chloride and calcium hydroxide. Ammonia is generally unreactive but will burn or react with substances like oxygen, hydrogen chloride, and metals/metal oxides. It is widely used to manufacture fertilizers and explosives.
Carbon dioxide is a colorless, odorless gas composed of carbon and oxygen that constitutes about 0.041% of the atmosphere. It was first observed in the 17th century by Jan Baptist Van Helmont during a charcoal burning experiment. Carbon dioxide has a linear molecular shape with a bond angle of 180 degrees. It is diamagnetic with no dipole moment due to its molecular structure. Carbon dioxide is used in many applications including fire extinguishers, refrigeration, winemaking, and enhancing the hardness of metal castings. It can be prepared in the laboratory by reacting calcium carbonate with hydrochloric acid.
The document provides information about various chemistry concepts related to air and water:
- It describes chemical tests to identify water and the purification of water supplies through filtration and chlorination.
- The composition of clean air is described as 78% nitrogen, 21% oxygen and small quantities of other gases. Common air pollutants like carbon monoxide and their sources are stated.
- Fractional distillation is outlined as the process used to separate oxygen and nitrogen from liquid air based on their different boiling points.
- Rusting is described as a reaction between iron, air and water that can be prevented by methods like painting and galvanizing to exclude oxygen.
Carbon dioxide was discovered by Van Helmont and proved to be an oxide of carbon by Antoine Lavoisier. It can be prepared by heating carbon or fuels like methane, or by heating carbonates like calcium carbonate. It is a colorless, odorless gas that is heavier than air and turns limewater milky. It is used in carbonated drinks, fire extinguishers, by plants during photosynthesis, and to preserve foods like meat and vegetables.
Acid deposition occurs when sulfur dioxide and nitrogen oxides emitted from the burning of fossil fuels react with water, oxygen, and other chemicals in the atmosphere to form acids. These acids can fall to Earth as rain, snow, fog or dry particles. Natural processes also produce acid deposition, but human activities such as burning coal and oil have increased acid deposition levels. Acid rain has a pH lower than 5.6 and can damage sensitive forests and lakes. The main pollutants that cause acid rain are sulfur dioxide and nitrogen oxides.
Preparation of salts (multiple choice) qpRubaHusain
Step 3 is to ensure all of the acid has reacted by adding copper(II) oxide in excess. Step 4 is to remove any excess copper(II) oxide by filtration to obtain pure copper(II) sulfate crystals.
The correct sequence of steps is: dissolving → filtration → evaporation → crystallisation.
Salts can be prepared by reacting dilute acids with metals, bases, or carbonates. Copper(II) chloride could be prepared by reacting copper with hydrochloric acid or by reacting copper carbonate with hydrochloric acid.
1. Dilute hydrochloric acid was used to react with various substances including copper oxide, iron nails, magnesium strips, and egg shells. These reactions all produced observable changes and gaseous products like hydrogen and carbon dioxide.
2. The acid reacted with the copper oxide on a coin, removing the layer to expose bare copper. Reactions with iron nails removed rust and bubbles formed, while magnesium vigorously reacted with bubbles. Egg shells reacted to produce carbon dioxide bubbles.
3. Additional details are provided about the chemical reactions, products, and observations for each substance tested with the hydrochloric acid.
1. Photosynthesis converts sunlight into chemical energy through two stages - the light-dependent reactions which produce ATP and NADPH using chlorophyll, and the light-independent Calvin cycle which uses these products to fix carbon and produce glucose.
2. The light-dependent reactions take place in the thylakoid membranes of the chloroplast and involve the absorption of light by photosystems and electron transport chains to generate a proton gradient for ATP synthesis via chemiosmosis.
3. The light-independent Calvin cycle occurs in the chloroplast stroma and uses the ATP and NADPH from the light reactions to reduce carbon dioxide and produce glucose through a series of reduction
1. Photosynthesis converts sunlight into chemical energy through light-dependent and light-independent reactions. 2. The light-dependent reactions use sunlight to produce ATP and NADPH through electron transport. 3. The light-independent Calvin cycle uses ATP and NADPH to fix carbon from CO2 into organic three-carbon sugars like G3P.
The document discusses activities of integration, which are assessments that evaluate students' ability to solve problems by integrating knowledge from a chapter. It provides examples of activities of integration, such as writing a letter inviting teachers to an end-of-year party. It also discusses the components of activities of integration, such as the problem/scenario and expected output. Additionally, it covers how to develop an assessment grid to score activities of integration based on relevance, accuracy, coherence and excellence. Teachers are then instructed to work in groups to create an activity of integration for any S1 topic along with its corresponding assessment grid.
This document provides guidance on managing large classes in competency-based education. By the end of the session, participants will explore the concept of large classes in competency-based education and elicit hands-on strategies for managing them. The document aims to help participants understand what constitutes a large class, ensure learning outcomes are achieved for all students in large classes, and provide subject group activities to discuss best practices.
Biostatistics uses statistical methods to analyze biological data, especially related to health and medicine. It is used widely in areas like public health, cancer research, pharmacology, ecology, genetics, and more. Some key uses of biostatistics include testing hypotheses, interpreting experimental results, determining treatment effectiveness, examining disease trends, and predicting outcomes. Proper use of biostatistical methods helps biologists design experiments, analyze results, and draw valid conclusions from their research.
The document discusses the rate of reaction and factors that affect it. It defines rate of reaction as the change in amount of reactant or product per unit time. The rate depends on concentration, temperature, surface area, and other factors. Higher concentrations and temperatures increase the rate by increasing collisions between reactant particles. Smaller particle sizes also increase the rate by providing more surface area for reactions. Graphs and experiments are described to illustrate these relationships.
This document discusses taxonomy and binomial nomenclature. It defines taxonomy as the science of identifying and classifying organisms, and notes that over 1.7 million species have been described. Binomial nomenclature, introduced by Carolus Linnaeus in 1758, assigns every species a two-part scientific name - the genus followed by a specific epithet. This standardized naming system ensures organisms have unique, unambiguous Latinized names. International codes govern naming conventions for different taxonomic groups like plants, animals and viruses.
The document summarizes key aspects of photosynthesis, including:
- Photosynthesis occurs in chloroplasts within plant cells and involves the absorption of light energy by chlorophyll to convert carbon dioxide and water into glucose and oxygen.
- Chlorophyll is the primary photosynthetic pigment that absorbs light in the blue and red wavelengths while reflecting green light, giving plants their green color.
- Other pigments like carotenoids help capture a broader range of wavelengths and transfer energy to chlorophyll.
- The light-dependent and light-independent reactions of photosynthesis utilize the energy from light absorption to fix carbon into sugars.
This document discusses nutrition and balanced diets. It defines the three main functions of food as energy-yielding, body-building, and protective. It explains the three food groups and emphasizes the importance of a varied, balanced diet containing portions from each group. Key nutrients like proteins, fats, carbohydrates, vitamins, minerals, antioxidants and their major food sources are outlined. The biological value and quality of different protein sources is also summarized.
This document discusses food and nutrients. It defines food as any substance that can provide nutrients to the body. Nutrients are chemical substances that help the body stay healthy and energetic. There are five main types of nutrients: carbohydrates, proteins, fats, vitamins, and mineral salts. Carbohydrates, proteins and fats provide energy, while all nutrients have roles in growth, repair, and regulation of functions. A balanced diet containing all nutrients is essential for health.
The document describes the Kingdom Monera, which consists mainly of eubacteria and cyanobacteria. Eubacteria are heterotrophic organisms that are named according to their shape, such as coccus (round), spirillum (spiral), and bacillus (rod-shaped). Cyanobacteria are autotrophic organisms commonly found in aquatic and terrestrial environments; they can exist as unicellular, colonial, or filamentous forms, and some can fix nitrogen through specialized cells called heterocysts.
Genetic disorders and diseases are caused by mutations in genetic material that can be inherited from parents or caused by environmental factors like radiation or chemicals. Mutations can occur when whole chromosomes are missing or extra chromosomes are present, or when sections of chromosomes are missing or in the wrong place. Examples of genetic disorders include Down syndrome, which results from an extra copy of chromosome 21, and sickle cell disease, phenylketonuria, Tay-Sachs disease, cystic fibrosis, and Huntington's disease, which are caused by recessive defective alleles inherited from both parents.
This document provides guidance on managing large classes in competency-based education. By the end of the session, participants will explore the concept of large classes in competency-based education and elicit hands-on strategies for managing them. The document aims to help participants understand what constitutes a large class, ensure learning outcomes are achieved for all students in large classes, and provide subject group activities to discuss best practices.
Methodologies and techniques to teach new curriculum in.pptxBagalanaSteven
This document outlines various methodologies and techniques that can be used to teach a new entrepreneurship curriculum in lower secondary schools. It discusses learner-centered teaching methods like discussion, case studies, brainstorming, buzz groups, demonstrations, guest speakers, role-playing, guided discovery, field trips and attachments. It also covers factors to consider when choosing a methodology, like the competencies being taught, available aids, learner age and interests. Techniques discussed for teaching the new curriculum include using simplified materials, integrating old content, avoiding duplication, using local examples, videos, engaging learners, fieldwork and ensuring timely coverage.
The document provides information about internet services and protocols. It defines common internet services like the World Wide Web, email, file transfer protocol, newsgroups, chat rooms and video conferencing. It describes how to use email by outlining features such as To, CC, BCC, attachments and address formats. Internet protocols discussed include TCP/IP, HTTP, FTP, SMTP, POP3 and IMAP. The document also defines common terms related to using the internet like downloading, uploading, browsing, bookmarks and web servers. Students are instructed to take notes and contact teachers for any clarification needed.
This document discusses learning and assessment through projects. It begins with a KWL activity to understand what teachers know and want to know about projects. Projects empower students to engage with 21st century skills like critical thinking and problem solving. Performance tasks are shorter and more structured, while projects are longer term, interdisciplinary, and focus on real-life issues. Effective projects are based on challenges, require inquiry, and have authentic impact. Projects should be assessed using rubrics that evaluate content, process, quality, and impact. Teachers provide guidance and formative feedback throughout the project process.
This document discusses project-based learning (PBL), a teaching method where students design and carry out an extended project that results in a tangible product or presentation. It is intended to make learning more active and relevant. The key points are:
1) PBL involves students planning and completing a project on a topic of their choice, rather than passively receiving information.
2) Teachers guide students and facilitate learning, while students take responsibility for their own work.
3) Projects incorporate principles like freedom, reality, activity and experience to make learning more meaningful.
4) Successful projects follow steps like planning, execution, documentation and evaluation.
1. Teachers should record learner achievement in categories like formative assessments, activities of integration, projects, co-curricular activities, and end of cycle assessments.
2. To determine a learner's achievement level from an activity of integration score, the score is scaled down by multiplying by 3, and the identifier is found using a provided table to determine if the achievement is basic, moderate, or outstanding.
3. A sample learner report card is presented that includes competency scores and descriptors, comments on generic skills and values, and achievement and areas for improvement for each subject.
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.
How to Build a Module in Odoo 17 Using the Scaffold MethodCeline George
Odoo provides an option for creating a module by using a single line command. By using this command the user can make a whole structure of a module. It is very easy for a beginner to make a module. There is no need to make each file manually. This slide will show how to create a module using the scaffold method.
Executive Directors Chat Leveraging AI for Diversity, Equity, and InclusionTechSoup
Let’s explore the intersection of technology and equity in the final session of our DEI series. Discover how AI tools, like ChatGPT, can be used to support and enhance your nonprofit's DEI initiatives. Participants will gain insights into practical AI applications and get tips for leveraging technology to advance their DEI goals.
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.
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.
Main Java[All of the Base Concepts}.docxadhitya5119
This is part 1 of my Java Learning Journey. This Contains Custom methods, classes, constructors, packages, multithreading , try- catch block, finally block and more.
Exploiting Artificial Intelligence for Empowering Researchers and Faculty, In...Dr. Vinod Kumar Kanvaria
Exploiting Artificial Intelligence for Empowering Researchers and Faculty,
International FDP on Fundamentals of Research in Social Sciences
at Integral University, Lucknow, 06.06.2024
By Dr. Vinod Kumar Kanvaria
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.
Certified as an ISO/IEC 27001: Information Security Management Systems (ISMS) Lead Implementer, Data Protection Officer, and Cyber Risks Analyst, Denis brings a heightened focus on data security, privacy, and cyber resilience to every endeavor.
His expertise extends across a diverse spectrum of reporting, database, and web development applications, underpinned by an exceptional grasp of data storage and virtualization technologies. His proficiency in application testing, database administration, and data cleansing ensures seamless execution of complex projects.
What sets Denis apart is his comprehensive understanding of Business and Systems Analysis technologies, honed through involvement in all phases of the Software Development Lifecycle (SDLC). From meticulous requirements gathering to precise analysis, innovative design, rigorous development, thorough testing, and successful implementation, he has consistently delivered exceptional results.
Throughout his career, he has taken on multifaceted roles, from leading technical project management teams to owning solutions that drive operational excellence. His conscientious and proactive approach is unwavering, whether he is working independently or collaboratively within a team. His ability to connect with colleagues on a personal level underscores his commitment to fostering a harmonious and productive workplace environment.
Date: May 29, 2024
Tags: Information Security, ISO/IEC 27001, ISO/IEC 42001, Artificial Intelligence, GDPR
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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.
How to Setup Warehouse & Location in Odoo 17 InventoryCeline George
In this slide, we'll explore how to set up warehouses and locations in Odoo 17 Inventory. This will help us manage our stock effectively, track inventory levels, and streamline warehouse operations.
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বাংলাদেশ অর্থনৈতিক সমীক্ষা (Economic Review) ২০২৪ UJS App.pdf
Sulphur (1).pdf
1. Sulphur and its Compounds
Sulphur and its Compounds
Charles Kidega
Kidegalize Network
es.gulu1910@gmail.com
+256(0)702816081
2. Kidegalize
Introduction to sulphur
Sulphur (symbol S) is a yellow
non-metallic solid element.
It belongs to Group VI and Period
3 in the Periodic Table.
Sulphur occurs as a free element
underground and also occurs in
combined form as sulphides,
sulphates, sulphites, petroleum oil
and natural gas.
4. Kidegalize
Three concentric pipes are sunk
into the ground up to sulphur
deposits.
Superheated water at 170oC and
10atm is forced down the
outermost pipe to melt the sulphur.
Hot compressed air is pumped down
the innermost pipe.
5. Kidegalize
The pressure created by the air
pumps the molten sulphur out
through the middle pipe to the
surface.
The froth of molten sulphur,
water and air is forced up to the
central pipe by pressure and it is
run into large tanks where it
solidifies to yellow roll sulphur.
6. Kidegalize
Allotropes of sulphur
Sulphur has two major crystalline
forms:
• Rhombic sulphur which consist of
large bright yellow octahedral
shaped crystals. It has a density
of 2.06gcm-3, melts at 114oC
and stable below 96oC.
7. Kidegalize
Preparation of rhombic sulphur
Powdered Sulphur is dissolved in
methylbenzene or carbon disulphide
in a test tube and the mixture
shaken vigorously for sometime.
The mixture is filtered using dry
filter paper and the filtrate
collected in a beaker.
8. Kidegalize
The beaker is covered with a
filter paper with a few holes in it
to allow the methylbenzene or
carbon disulphide to evaporate
slowly.
When all the volatile solvent has
evaporated, bright yellow
octahedral crystals are deposited.
9. Kidegalize
• Monoclinic sulphur which consist
of pale yellow needle (prismatic)
shaped crystals. It has a density
of 1.98gcm-3, melts at 119oC
and stable above 96oC.
10. Kidegalize
Preparation of monoclinic sulphur
Heat powdered sulphur in an
evaporating dish and keep stirring
while adding more sulphur until the
dish is almost brimful.
After all the sulphur is molten, allow
it cool. When a thin solid crust
forms on the surface, pierce it using
glass rod to create two spaced holes.
11. Kidegalize
Pour out the liquid Sulphur through
one hole into a beaker. Carefully
cut away the crust and lift it out.
Thin needle-like pale yellow
crystals form both beneath the
crust and inside the dish.
12. Kidegalize
Remember: When one gram of
each allotrope is separately burnt
in air, the same mass volume of
sulphur dioxide is formed.
S(s) + O2(g) SO2(g)
This shows that rhombic and
monoclinic sulphur are allotropes of
sulphur.
13. Kidegalize
Reactions of sulphur
• Sulphur burns in air with a blue
flame to form Sulphur dioxide.
S(s) + O2(g) SO2(g)
• Sulphur reacts with heated
metals to form sulphides (black
solids).
Fe(s) + S(s) FeS(s)
Cu(s) + S(s) CuS(s)
14. Kidegalize
• Sulphur react with carbon to
form liquid carbon disulphide.
S(s) + C(s) CS2(l)
• Molten Sulphur reacts with
hydrogen to form hydrogen
sulphide.
S(l) + H2(g) H2S(g)
15. Kidegalize
• Concentrated sulphuric acid oxidizes
Sulphur to sulphur dioxide.
S(s) + 2H2SO4(l) 3SO2(g) + 2H2O(l)
• Sulphur is oxidized to sulphuric acid
by hot concentrated nitric acid.
S(s) + 6HNO3(l) H2SO4(aq) + 6NO2(g) + 2H2O(l)
16. Kidegalize
Uses of sulphur
• Manufacture of sulphuric acid.
• Manufacture of dyes and
fireworks.
• Vulcanisation of natural rubber.
• Manufacture of ointments and
tablets used to treat ringworm.
17. Kidegalize
Sulphur dioxide, SO2
Preparation of sulphur dioxide from
sodium sulphite and dilute sulphuric
acid
Dilute sulphuric acid from a tap
funnel is added to sodium sulphite in
a flask fitted with a delivery tube
and the mixture warmed gently.
Sulphur dioxide is produced according
to the equation.
18. Kidegalize H2SO4(aq) + Na2SO3(s) Na2SO4(aq) + H2O(l) + SO2(g)
The gas is passed through
concentrated sulphuric acid for
drying and then collected by
downward delivery because it is
denser than air.
20. Kidegalize
Remember
• Hydrogensulphite can be used
instead of sulphite.
• Hydrochloric acid can be used
instead of sulphuric acid.
• The gas is not collected over water
because it is very soluble in water.
• Copper and conc. sulphuric acid can
also be used.
22. Kidegalize
Physical properties
• It is denser than air.
• It is a colourless poisonous gas
with a choking irritating smell.
• It has a sweet smell.
• It is very soluble in water.
23. Kidegalize
Reactions of sulphur dioxide
• Sulphur dioxide turns damp blue
litmus paper red because it is
acidic.
• It dissolves in water to form
sulphurous acid.
H2O(l) + SO2(g) H2SO3(aq)
24. Kidegalize
• It combines with oxygen in the
presence of vanadium(V) oxide as
catalyst to form sulphur trioxide
gas.
2SO2(g) + O2(g) 2SO3(g)
25. Kidegalize
• Limited sulphur dioxide reacts with
sodium hydroxide solution to form
sodium sulphite.
2NaOH(aq) + SO2(g) Na2SO3(aq) + H2O(l)
Excess sulphur dioxide reacts with
sodium hydroxide solution to form
sodium hydrogensulphite (acidic salt).
NaOH(aq) + SO2(g) NaHSO3(aq)
27. Kidegalize
• Sulphur dioxide reduces acidified
potassium dichromate(VI) solution
to chromium(III) ions.
Observation: Orange solution turns
green.
Remember: The two reactions are
used to test for sulphur dioxide.
28. Kidegalize
• Sulphur dioxide reduces
concentrated nitric acid to
nitrogen dioxide(reddish brown)
when the mixture is warmed.
SO2(g) + 2HNO3(l) H2SO4(aq) + NO2(g)
• Sulphur dioxide bleaches dyes in
presence of water.
SO2(g) + 2H2O(l) + dye H2SO4(aq) + (dye + 2H)
29. Kidegalize
• Sulphur dioxide reduces halogens
to their hydrogen compounds.
SO2(g) + H2O(l) + Cl2(aq) H2SO4(aq) + HCl(aq)
Observation: Yellowish-green
chlorine, red bromine and brown
iodine turns colourless.
30. Kidegalize
Oxidation reactions of sulphur
dioxide
• Sulphur dioxide oxidizes burning
magnesium to magnesium oxide.
2Mg(s) + SO2(g) 2MgO(s) + S(s)
Observation: Yellow solid and white
solid observed.
32. Kidegalize
Uses of sulphur dioxide
• Manufacture of sulphuric acid by
contact process.
• Bleaching of pulp in the paper
factory during the manufacture
of paper.
• Preservation of tinned food and
drinks.
• Refrigeration as a refrigerant.
33. Kidegalize
Knowledge Check 1
Qn.1(UNEB 2006/P1/16)
The gas that changes the colour
of acidified potassium dichromate
solution orange to green is.
A. ammonia
B. Chlorine
C. carbon dioxide
D. sulphur dioxide
34. Kidegalize
Qn.2(UNEB 2013/P1/30)
Which one of the following is formed
when excess sulphur dioxide gas is
bubbled through sodium hydroxide
solution?
A. Sodium sulphate
B. Sodium sulphite.
C. Sodium hydrogen sulphite.
D. Sodium hydrogen sulphate.
35. Kidegalize
Qn.3(UNEB 2002/P1/15)
Sulphur dioxide is used in the
following ways except in the
A. bleaching of materials such as
wool and silk.
B. treating of wool pulp when
manufacturing paper.
C. large-scale production of sulphuric
acid.
D. manufacture of vulcanised rubber.
36. Kidegalize
Qn.4(UNEB 1995/P1/12)
Sulphur dioxide behaves as an
oxidising agent when it reacts with
A. concentrated nitric acid.
B. iron(III) sulphate.
C. hydrogen sulphate.
D. potassium dichromate.
37. Kidegalize
Qn.5(UNEB 2000/P1/13)
Which one of the following reagents
is used to test for sulphur dioxide?
A. Chlorine water.
B. Acidified potassium permanganate.
C. Cobalt chloride.
D. An hydrous copper sulphate.
38. Kidegalize
Qn.6(UNEB 1992/P2/11)
(a)Draw a well labeled diagram to
show how a dry sample of
sulphur dioxide can be prepared
in the laboratory.
(b)Write an equation for the
reaction that takes place in (a).
39. Kidegalize
(c)Describe a test that can be
carried out to confirm the
presence of sulphur dioxide.
(d)Excess sulphur dioxide was
bubbled through a solution of
sodium hydroxide. Write an
equation for the reaction that
took place.
40. Kidegalize
Qn.7(UNEB 2002/P2/11)
(a)(i) Name one substance that is
reacted with hydrochloric
acid to produce sulphur
dioxide in the laboratory.
(ii) State the conditions for the
reaction.
41. Kidegalize
(iii) Name a substance that can be
used to dry the sulphur dioxide
formed.
(iv)Write equation for the reaction
leading to the formation of
sulphur dioxide.
42. Kidegalize
(b) State what would be observed
and explain what would happen
if sulphur dioxide is passed
through a solution containing
(i) acidified potassium
dichromate
(ii) a dye.
43. Kidegalize
(c) Briefly describe how sulphur
dioxide can be converted to
sulphuric acid.
Your answer should include
equations and conditions for the
reactions(s).
44. Kidegalize
Qn.7(UNEB 2003/P2/5)
(a) Write an ionic equation to show
how sulphur dioxide can be formed
from sodium sulphate and
hydrochloric acid.
(b)(i)Name one reagent that can be
used to test for sulphur dioxide.
(ii) State what would be observed
if sulphur dioxide was reacted with
the reagent you have named in (b)(i).
45. Kidegalize
(c) Sulphur dioxide was passed into
a beaker containing a red
flower and water.
(i) State what was observed.
(ii) Give a reason for your
answer in (c)(i).
46. Kidegalize
Qn.8(UNEB 2014/P2/11)
(a) (i) With the aid of a labeled
diagram, explain how a pure dry
sample of sulphur dioxide can be
prepared in the laboratory using
sodium sulphite and sulphuric acid.
(ii) Write an equation for the
reaction leading to the formation
of sulphur dioxide.
47. Kidegalize
(b) Name one reagent that would
be used to confirm the presence
of sulphur dioxide and state what
would be observed if the reagent
you have named was treated with
sulphur dioxide.
48. Kidegalize
(c) Write an equation to show the
reaction between sulphur dioxide
and
(i) water
(ii) oxygen in the presence of
hot platinum.
49. Kidegalize
(d) The product of the reaction in
c(ii) was mixed with water and
barium nitrate solution added to
the resultant mixture
(i) State what was observed.
(ii) Explain what took place
(No equation required)
50. Kidegalize
Qn.8(UNEB 2005/P2/9)
(a) Write an equation for the
formation of sulphur dioxide from
sulphuric acid and sodium sulphite.
(b)Sulphur dioxide was bubbled
through an acidified solution of
potassium dichromate.
(i) State what was observed.
(ii) Briefly explain your observation in
(b)(i).
51. Kidegalize
Qn.9(UNEB 2008/P2/5(a))
(i) Name one substance that when
reacted with dilute hydrochloric
acid can produce sulphur dioxide.
(ii) State the condition for the
reaction.
(iii) Write an ionic equation for the
reaction leading to the formation
of sulphur dioxide.
52. Kidegalize
Sulphuric acid, H2SO4
Manufacture of sulphuric acid by
contact process
Sulphur is burned in air to form
sulphur dioxide.
S(s) + O2(g) SO2(g)
The sulphur dioxide is mixed with
air. The mixture is dried and passed
over vanadium(V) oxide catalyst
heated at 500oC and pressure of
1atm.
53. Kidegalize
The sulphur dioxide is oxidized to
sulphur trioxide.
2SO2(g) + O2(g) 2SO3(g)
The sulphur trioxide formed is
absorbed into 98% concentrated
sulphuric acid forming a fuming
sulphuric acid (oleum).
SO3(g) + H2SO4(l) H2S2O7(l)
54. Kidegalize
The oleum formed is absorbed,
cooled and carefully diluted with
water to form sulphuric acid.
H2S2O7(l) + H2O(l) 2H2SO4(aq)
55. Kidegalize
The flow diagram for the Contact
Process
air burners cleaners driers
catalyst
absorbers
sulphuric acid
STEP 1 STEP 2 STEP 3
STEP 5
STEP 4
SO2 + air SO2 + air
SO
2
+
air
56. Kidegalize
• Step 1: Production of SO2.
• Step 2: Purification/removal of
impurities.
• Step 3: Drying SO2-air mixture
using concentrated sulphuric acid
• Step 4: Passing hot SO2-air
mixture over vanadium(V) oxide
catalyst.
• Step 5: Absorption of SO3 in
fuming sulphuric acid.
58. Kidegalize
Reactions of sulphuric acid
As a strong acid (dilute H2SO4)
• It ionizes completely in solution.
H2SO4(aq) 2H+(aq) + SO4
2-(aq)
• It turns blue litmus paper red.
• It reacts with metals to form
sulphates and hydrogen gas.
Mg(s) + H2SO4(aq) MgSO4(aq) + H2(g)
59. Kidegalize
• It reacts with carbonates and
hydrogencarbonates to form
sulphates, water and carbon dioxide
gas.
ZnCO3(s) + H2SO4(aq) ZnSO4(aq) + H2O(l) + CO2(g)
Remember: When CaCO3, PbCO3 or
BaCO3 are mixed with dilute H2SO4 a
reaction starts but soon stops because
the sulphates formed are insoluble.
60. Kidegalize
• It reacts with oxides and
hydroxides to form sulphates and
water only.
CuO(s) + H2SO4(aq) CuSO4(aq) + H2O(l)
2NaOH(aq) + H2SO4(aq) Na2SO4(aq) + 2H2O(l)
61. Kidegalize
As an oxidizing agent
• Hot concentrated sulphuric acid
oxidizes copper(brown solid),
carbon and Sulphur to copper(II)
sulphate (blue solution), carbon
dioxide and Sulphur dioxide
respectively.
63. Kidegalize
As a dehydrating agent
• Concentrated sulphuric acid at
180oC dehydrates alcohols to
form alkenes.
C2H5OH(aq) C2H4(g) + H2O(l)
Conc.H2SO4
64. Kidegalize
• When concentrated sulphuric
acid is added to sugar crystals,
the white solid turns black and a
colorless vapour given off.
C12H22O11(s) 12C(s) + 11H2O(g)
Conc.H2SO4
65. Kidegalize
• When concentrated sulphuric
acid is added to hydrated
copper(II) sulphate, the blue
solid turns white and a colorless
vapour given off.
CuSO4.5H2O(s) CuSO4(s) + 5H2O(g)
Conc.H2SO4
66. Kidegalize
• When concentrated sulphuric
acid is added to hydrated
iron(II) sulphate, the green
solid turns white and a colorless
vapour given off.
FeSO4.7H2O(s) FeSO4(s) + 7H2O(g)
Conc.H2SO4
67. Kidegalize
Uses of sulphuric acid
Sulphuric acid is used in the
manufacture of:
• fertilizers
• drugs
• dyes
• detergents
• plastics
69. Kidegalize
Knowledge Check 2
Qn.1(UNEB 2001/P1/12)
Which one of the following compounds
is used as a catalyst in the
manufacture of sulphur trioxide?
A. Alumina.
B. Vanadium(V) oxide.
C. Manganese (IV) oxide
D. Iron powder
70. Kidegalize
Qn.2(UNEB 2007/P1/19)
During the manufacture of
sulphuric acid, sulphur trioxide is
dissolved in
A. cold water
B. hot water
C. dilute sulphuric acid
D. concentrated sulphuric acid
72. Kidegalize
(a) Write an equation for the reaction
that takes place in step 1.
(b)Why is step II necessary?
(c) Name
(i) the drying agent in step III,
(ii) the catalyst IV.
(d) Describe the process that takes
place in step V.
73. Kidegalize
Qn.4(UNEB 2007/P2/9(b))
During the manufacture of sulphuric
acid by the contact process, sulphur
dioxide is heated with oxygen in the
presence of a catalyst.
(i) Name the catalyst.
(ii) Write the equation for the
reaction between sulphur dioxide
and oxygen.
75. Kidegalize
Dilute hydrochloric acid from a tap
funnel is added to iron(II) sulphide
covered with a little water in a
flat-bottomed flask fitted with a
delivery tube.
Hydrogen sulphide gas is produced
according to the equation:
FeS(s) + 2HCl(aq) H2S(g) + FeCl2(aq)
76. Kidegalize
The gas is collected over warm
water because it is soluble in cold
water.
Remember
• Concentrated hydrochloric acid
or dilute sulphuric acid can be
used instead of dilute
hydrochloric acid.
77. Kidegalize
• The gas is dried using silicon
dioxide or phosphorus pentoxide
packed in a u-tube and is
collected by downward delivery.
78. Kidegalize
Physical properties
• It is a colorless gas.
• It is slightly denser than air.
• It is slightly soluble in water.
• It has a rotten egg smell.
79. Kidegalize
Chemical properties
• It is an acidic gas and dissolves
in water forming weak acidic
solution.
• It burns in limited air supply to
form Sulphur and water.
2H2S(g) + O2(g) 2S(s) + H2O(l)
80. Kidegalize
• It burns in excess air supply to
form sulphur dioxide and water.
2H2S(g) + 3O2(g) 2SO2(s) + 2H2O(l)
• Hydrogen sulphide reduces
concentrated nitric acid to
nitrogen dioxide and itself
oxidized to sulphur.
2HNO3(l) + H2S(g) 2NO2(g) + 2H2O(l) + S(s)
81. Kidegalize
• Hydrogen sulphide reacts with
concentrated sulphuric acid to
form a yellow precipitate.
H2SO4(l) + 3H2S(g) 4H2O(l) + 4S(s)
• It reduces iron(III) chloride to
iron(II) chloride and itself
oxidized to Sulphur.
2FeCl3(aq) + H2S(g) 2FeCl2(aq) + 2HCl(aq) + S(s)
82. Kidegalize
• Hydrogen sulphide reduces acidified
potassium permanganate (purple) to
manganese(II) ions (colorless) and a
yellow solid is formed.
• Hydrogen sulphide reduces acidified
potassium dichromate(VI) (orange)
to chromium(III) ions (green) and a
yellow solid is formed.
83. Kidegalize
• Hydrogen sulphide reduces
hydrogen peroxide to water and
itself oxidized to sulphur.
H2S(g) + H2O2(aq) 2H2O(l) + S(s)
• Hydrogen sulphide reduces moist
Sulphur dioxide to Sulphur
(yellow solid)
2H2S(aq) + SO2(g) 2H2O(l) + 3S(s)
84. Kidegalize
• Hydrogen sulphide reacts with
bases as a dibasic acid.
2NaOH(aq) + H2S(g) Na2S(aq) + 2H2O(l)
• Hydrogen sulphide reacts with
lead(II) nitrate solution to form
black precipitate.
Pb(NO3)2(aq) + H2S(g) PbS(s) + 2HNO3(aq)
85. Kidegalize
• Hydrogen sulphide reacts with
copper(II) sulphate solution to
form dark brown precipitate.
CuSO4(aq) + H2S(g) CuS(s) + H2SO4(aq)
86. Kidegalize
Knowledge Check 3
Qn.1(UNEB 2008/P2/5(b))
A gas jar containing hydrogen
sulphide was inverted over a gas jar
containing moist sulphur dioxide.
(i) State what was observed.
(ii) Write an equation for the
reaction that took place.
87. Kidegalize
Qn.2
(a) When dilute hydrochloric acid was
added to iron(II) sulphide, a gas
W was evolved.
(i) Identify gas W.
(ii) Write an equation for the
reaction that took place.
(b) State
(i) how the gas could be
identified.
88. Kidegalize
(ii) why the gas is normally
prepared in a fume
cupboard.
(c) The gas was reacted with
sulphur dioxide.
(i) State what was observed.
(ii) Explain your answer in
(c)(i).
89. Kidegalize
Qn.3
(a)With a help of diagram,
describe how dry hydrogen
sulphide can be prepared in the
laboratory.
(b) Hydrogen sulphide gas was
bubbled into iron(III) chloride
solution.
90. Kidegalize
(i) State what was observed.
(ii) Write an equation for the
reaction.
(iii) Explain your observation in (i).
92. Kidegalize
Qn.5(UNEB 2006/P2/6)
(a) When dilute hydrochloric acid was
added to iron(II) sulphide , a gas
was evolved.
Write an equation for the reaction
that took place.
(b) State;
(i) how the gas was identified.
(ii) Why the gas is normally
prepared in a fume cupboard
93. Kidegalize
or outside the laboratory.
(c) The gas was reacted with
sulphur dioxide.
(i) State what was observed.
(ii) Give a reason for your
answer in (c)(i).