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Study of Compounds Class 10 ICSE | Study of Compounds Chemistry ICSE Class 10 | @sirtarunrupani

Sir Tarun Rupani・76 minutes read

The text discusses the chemistry chapter on compounds, focusing on ammonia, nitric acid, and their properties, reactions, and laboratory preparations. It highlights key equations and methods for preparing hydrogen chloride gas, ammonia, and nitric acid, emphasizing their chemical properties and applications in various reactions and processes.

Insights

  • The lab preparation for hydrogen chloride gas involves homemade salt and concentrated sulfuric acid, emphasizing the importance of specific materials and conditions for safe experimentation.
  • Ammonia, a basic compound, is utilized as a drying and reducing agent in various reactions, showcasing its versatile nature and practical applications beyond its chemical properties.
  • Nitric acid, a strong oxidant, reacts with alkalis to form salts and water, underlining its role as a potent chemical agent that interacts with various substances to produce distinct outcomes.

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Recent questions

  • What are the properties of hydrogen chloride gas?

    Hydrogen chloride gas is colorless, pungent-smelling, and corrosive. It is highly soluble in water, as shown in the Fountain Experiment. The gas does not support combustion and reacts with metals to form acids. When reacted with water, hydrogen chloride gas produces hydrochloric acid.

  • How is ammonia prepared in a laboratory setting?

    Ammonia is prepared in the lab by using a round bottom flask, ammonium chloride, calcium oxide, and an alkali. The reaction between calcium hydroxide and ammonium chloride produces calcium chloride, water, and ammonia. Wet ammonia gas is collected using a drawing tower with calcium oxide as a drying agent.

  • What is the process of creating nitric acid?

    Nitric acid is created by heating potassium nitrate and concentrated sulfuric acid in a glass retort. The reaction produces vaporized nitric acid, which is then condensed back into liquid form using cold water. To remove the yellow color from nitric acid, dry air or carbon dioxide can be passed through it.

  • How is sulfuric acid produced industrially?

    Sulfuric acid is produced industrially through large-scale reactions. The process involves passing sulfur trioxide through an absorb tower with concentrated sulfuric acid to produce sulfuric acid. This acid is colorless, slightly sour, and acts as a dehydrating agent.

  • What are the uses of ammonia in various reactions?

    Ammonia is used as a drying agent and a reducing agent in different reactions. It is also utilized as a refrigerant in air conditioners and refrigerators to absorb heat from the atmosphere. Ammonia reacts with oxygen to produce nitrogen and water, showcasing its versatile applications in various chemical processes.

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Summary

00:00

Chemistry: Ammonia, Nitric Acid, and Reactions

  • The chapter of chemistry on compounds has four parts: ammonia, nitric acid, sulfuric acid, and concentration.
  • The focus today is on finishing the first two parts: ammonia and nitric acid.
  • Important equations from these chapters will be highlighted for memorization.
  • The lab preparation for hydrogen chloride gas involves homemade salt and concentrated sulfuric acid.
  • The reaction should be done at a temperature below 200 degrees to avoid glass rod cracking.
  • Properties of hydrogen chloride gas include being colorless, pungent-smelling, and corrosive.
  • The gas is highly soluble in water, as demonstrated in the Fountain Experiment.
  • Chemical properties of hydrogen chloride gas include not supporting combustion and reacting with metals to form acids.
  • Reacting hydrogen chloride gas with water produces hydrochloric acid.
  • The gas collected in the lab preparation can be used to create acyl acid by mixing with water.

18:09

"Collecting HS Gas with Inverted Funnel"

  • HS gas is produced and collected using an inverted funnel to prevent desoldering and backflow of water.
  • The rim of the funnel should be at the surface of the water to increase surface area and solubility.
  • Inverted funnel arrangement is crucial to prevent water from rising and causing issues.
  • HS gas is converted to HS acid by dissolving in water.
  • Dry AC refers to dry hydrochloric acid, which is soluble in water to form an aqueous solution.
  • Acids like HClO3 can be dangerous and corrosive, causing harm if not handled properly.
  • Chemical tests like litmus paper and reactions with metals can help identify acids like HS.
  • Dilute HClO3 does not react with nitrates but forms white precipitates with lead and mercury nitrates.
  • Concentrated HClO3 reacts with silver nitrate to produce white precipitates.
  • Ammonia is a basic compound found in various forms, including gas, liquid, and as a laboratory reagent.

36:58

"Lab Preparation and Manufacturing of Ammonia"

  • Soluble bases include sodium hydroxide, potassium hydroxide, and calcium hydroxide, which are alkalis.
  • Ammonium salt, specifically ammonium chloride, is commonly used to react with alkalis like calcium hydroxide.
  • The reaction between calcium hydroxide and ammonium chloride produces calcium chloride, water, and ammonia.
  • Lab preparation of ammonia involves using a round bottom flask, ammonium chloride, calcium oxide, and an alkali.
  • The reaction produces wet ammonia gas, which is collected using a drawing tower with calcium oxide.
  • The use of calcium oxide is crucial as a drying agent due to its basic nature and lack of reaction with ammonia.
  • The volume ratio of ammonium chloride to calcium oxide is essential for the reaction.
  • Ammonia can also be prepared from metal nitrate by reacting magnesium nitride with warm water.
  • The process involves passing dry ammonia gas through a drawing tower with calcium oxide to produce liquid ammonia.
  • Manufacturing ammonia in bulk quantities requires the Haber-Bosch process, involving nitrogen, hydrogen, a compressor, a catalytic chamber, and finally divided iron as a catalyst.

51:54

Chemical properties and uses of ammonia

  • Ammonia reacts with oxygen in a jar to produce nitrogen and water.
  • The reaction of ammonia with oxygen proves the presence of nitrogen in ammonia.
  • The reaction is irreversible and exothermic, releasing a lot of heat.
  • Catalytic oxidation of ammonia with platinum S catalyst produces nitrogen dioxide.
  • Ammonia reduces copper oxide to copper, proving the presence of hydrogen in ammonia.
  • Ammonia reacts with chlorine to form nitrogen, proving its reducing agent properties.
  • Ammonia reacts with acid to form ammonium salt, showing its weak base nature.
  • Ammonia is used as a drying agent and a reducing agent in various reactions.
  • Ammonia is used as a refrigerant in ACs and refrigerators to absorb heat from the atmosphere.
  • Nitric acid is formed in the rain through the combination of nitrogen and oxygen during lightning.

01:08:35

Creating Nitric Acid from Potassium Nitrate

  • To create nitric acid, a glass retort is needed along with potassium nitrate (niter) and concentrated sulfuric acid.
  • The two compounds are heated to produce vaporized nitric acid, which is then condensed back into liquid form using cold water.
  • The reaction involves potassium nitrate reacting with concentrated sulfuric acid to form potassium hydrogen sulfate and nitric acid.
  • The temperature during the reaction should not exceed 200 degrees to prevent damage.
  • Nitric acid vapor is collected and condensed back into liquid form by cooling with cold water.
  • To remove the yellow color from nitric acid, dry air or carbon dioxide can be passed through it.
  • Excess water can be added to nitric acid to make it colorless.
  • Only concentrated sulfuric acid should be used in the preparation of nitric acid due to its non-volatile nature.
  • Nitric acid is an oxidant that decomposes at temperatures above 200 degrees, producing nitrogen dioxide, water, and oxygen.
  • Nitric acid is a monobasic acid that reacts with alkalis to form salts and water, making it a strong oxidant that reacts with metals to produce hydrogen gas.

01:25:05

Sulfur Extraction and Acid Production Process

  • To extract sulfur from pyrite, both compounds must be clean and dry to avoid impurities.
  • The reaction process involves passing the compounds through a chamber to remove any dust particles.
  • The gas produced is cooled and passed through a dust chamber to settle any remaining impurities.
  • The gas is then used in the contact tower to combine with oxygen and form sulfur trioxide.
  • Sulfur trioxide is then passed through an absorb tower with concentrated sulfuric acid to produce sulfuric acid.
  • Sulfuric acid can further react with carbon to form pyrosulfuric acid, which can be stored and diluted as needed.
  • The industrial method involves large-scale reactions to produce sulfuric acid efficiently.
  • Sulfuric acid is colorless and slightly sour, showing acidic properties and acting as a dehydrating agent.
  • Concentrated sulfuric acid can react with carbohydrates to dehydrate them and produce carbon.
  • Dilute sulfuric acid reacts with metals to form salts and hydrogen, neutralizing the acid.

01:40:48

"Four Chapters on Compound Study"

  • Text discusses four chapters on the study of compounds with a focus on an important topic by Tech Care God Bless You.
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