Chemistry Chapter on Ammonia and Reactions
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Questions and Answers

What gas is evolved during the heating of nitrates?

  • Oxygen
  • Sulfur dioxide
  • Nitrogen dioxide (correct)
  • Carbon dioxide

Which of the following is NOT a use of nitric acid?

  • Production of sulfuric acid (correct)
  • Purification of gold
  • Manufacturing of fertilizers
  • Manufacturing of explosives

What type of reaction occurs when freshly prepared FeSO4 is mixed with conc. H2SO4 and HNO3?

  • Precipitation reaction
  • Redox reaction (correct)
  • Complexation reaction
  • Neutralization reaction

What is concentrated sulfuric acid commonly referred to as?

<p>Acid of vitriol (A), King of Chemicals (C)</p> Signup and view all the answers

What does the brown ring that occurs at the junction of nitric acid and concentrated sulfuric acid indicate?

<p>Presence of iron(II) compounds (D)</p> Signup and view all the answers

What method is used to prepare ammonia from magnesium nitride?

<p>Treating with warm water (D)</p> Signup and view all the answers

Why must water vapour be removed from the evolved ammonia gas?

<p>Because ammonia is soluble in water (C)</p> Signup and view all the answers

What is the vapor density of ammonia?

<p>8.5 (A)</p> Signup and view all the answers

What process is used for the large-scale production of ammonia?

<p>Haber's process (C)</p> Signup and view all the answers

In Haber’s process, what is the ratio of hydrogen to nitrogen used?

<p>3:1 (D)</p> Signup and view all the answers

What temperature range is maintained during the Haber process?

<p>450 - 500°C (B)</p> Signup and view all the answers

What role does quicklime play in the preparation of ammonia?

<p>It removes water vapour from ammonia (C)</p> Signup and view all the answers

What type of reaction occurs during the production of ammonia in the Haber process?

<p>Exothermic and reversible (D)</p> Signup and view all the answers

What is the name of the process by which atmospheric nitrogen is converted to nitrogenous compounds in the soil?

<p>Nitrogen fixation (C)</p> Signup and view all the answers

Which acids are used in the laboratory preparation of nitric acid?

<p>Sodium nitrate and concentrated sulfuric acid (A)</p> Signup and view all the answers

What is the physical state of nitric acid when formed in the laboratory?

<p>Colorless liquid with a suffocating smell (D)</p> Signup and view all the answers

At what temperature does nitric acid boil?

<p>355.6 K (A)</p> Signup and view all the answers

What is the primary difference between hydrogen chloride and hydrochloric acid?

<p>Hydrogen chloride does not turn litmus paper red, while hydrochloric acid does. (A)</p> Signup and view all the answers

Which statement correctly describes the chemical behavior of nitric acid?

<p>It reacts with carbonates to form soluble nitrates. (A)</p> Signup and view all the answers

What type of agent is nitric acid primarily considered to be?

<p>Strong oxidizing agent (B)</p> Signup and view all the answers

Which of the following statements about hydrochloric acid is correct?

<p>It is colorless and has a pungent smell. (A)</p> Signup and view all the answers

Which noble metals does nitric acid not oxidize?

<p>Gold and platinum (A)</p> Signup and view all the answers

What is formed when hydrochloric acid reacts with thiosulphates?

<p>Sulphur dioxide gas and yellow precipitate. (B)</p> Signup and view all the answers

How can 98% concentration of HNO3 be achieved in the preparation process?

<p>By distillation with concentrated sulfuric acid (B)</p> Signup and view all the answers

What is the boiling point of hydrochloric acid?

<p>110 °C (B)</p> Signup and view all the answers

What action does hydrochloric acid have on metals?

<p>It forms metallic chlorides and releases hydrogen gas. (B)</p> Signup and view all the answers

How can you distinguish between thiosulphates and sulphites using hydrochloric acid?

<p>The formation of a yellow precipitate occurs with thiosulphates. (D)</p> Signup and view all the answers

Which indicators show a color change when testing for the acid nature of hydrochloric acid?

<p>Moist litmus, methyl orange, and phenolphthalein. (C)</p> Signup and view all the answers

What is aqua regia composed of?

<p>Three parts concentrated HCl and one part concentrated HNO3. (A)</p> Signup and view all the answers

What is formed when zinc reacts with very dilute nitric acid at room temperature?

<p>Zinc nitrate and hydrogen gas (C)</p> Signup and view all the answers

What precaution should be noted regarding chromium and aluminium in concentrated nitric acid?

<p>They do not react due to a passive film of oxide (B)</p> Signup and view all the answers

What is the main outcome of the Brown Ring Test?

<p>It identifies nitrate ions (D)</p> Signup and view all the answers

Which gases are produced when copper reacts with concentrated nitric acid?

<p>Nitrogen dioxide and water (A)</p> Signup and view all the answers

What is the primary catalyst used in the contact process for the conversion of sulphur dioxide to sulphur trioxide?

<p>Vanadium pentoxide (C)</p> Signup and view all the answers

Which of the following compounds can be found in the combined state of sulphur?

<p>Barytes (D)</p> Signup and view all the answers

Which of the following statements about the physical properties of sulphuric acid is true?

<p>It has a specific gravity of 1.84 at 298 K. (C)</p> Signup and view all the answers

What temperature range is generally maintained during the conversion of sulphur dioxide to sulphur trioxide for optimal yield?

<p>410-450 °C (D)</p> Signup and view all the answers

What occurs when oleum is diluted with water?

<p>It produces sulphuric acid. (D)</p> Signup and view all the answers

Which of the following characteristics is NOT associated with sulphuric acid?

<p>High volatility (C)</p> Signup and view all the answers

What is the dissociation constant (Ka1) indicative of for sulphuric acid in aqueous solution?

<p>It is a strong acid. (A)</p> Signup and view all the answers

What is the final product of the reaction between sulphur trioxide and sulphuric acid?

<p>Pyrosulphuric acid (B)</p> Signup and view all the answers

Flashcards

Hydrochloric Acid

An aqueous solution of hydrogen chloride gas.

Hydrogen Chloride

Dry or liquid hydrogen chloride gas, not an aqueous solution.

Difference between HCl and Hydrochloric Acid

HCl is a gas, while hydrochloric acid is a solution of HCl in water. HCl is non-acidic in the dry state, but acidic when dissolved in water.

Laboratory Preparation of Hydrochloric Acid

Passing HCl gas into water, causing the water to rise, then fall, until saturated.

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Physical Properties of Hydrochloric Acid

Colourless, pungent smell, sour taste, corrosive, and soluble in water (boiled at 110°C).

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Chemical Properties of Hydrochloric Acid

Strongly acidic (turns litmus red, methyl orange pink). Reacts with metals, thiosulphates and some nitrates to produce various products.

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Aqua Regia

A mixture of concentrated nitric acid and hydrochloric acid used to dissolve gold and platinum.

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Indicators in Hydrochloric Acid

Substances used to determine the acidity. (Example: Litmus, Methyl Orange, Phenolphthalein)

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Nitric acid reaction with copper (dilute)

3Cu + 8HNO3(dilute) → 3Cu(NO3)2 + 2NO +4H2O. Copper reacts with dilute nitric acid to produce copper(II) nitrate, nitric oxide, and water.

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Nitric acid reaction with copper (concentrated)

Cu + 4HNO3(conc.) → Cu(NO3)2 +2NO2 +2H2O. Copper reacts with concentrated nitric acid to yield copper(II) nitrate, nitrogen dioxide, and water.

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Brown Ring Test

A test for nitrates, using the reduction of nitrate to nitric oxide (NO) by Fe2+ ions, which then forms a brown colored complex.

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Aqua Regia composition

A mixture of concentrated nitric acid (1 part) and concentrated hydrochloric acid (3 parts).

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Passivation of Chromium/Aluminum by HNO3

Chromium and aluminum resist reaction with concentrated nitric acid due to the formation of a protective oxide film on the surface, preventing further reaction.

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Ammonia preparation from metal nitrides

Ammonia can be produced by reacting warm water with metal nitrides like magnesium nitride, sodium nitride, and aluminium nitride.

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Collection method for ammonia gas

Ammonia gas is collected by downward displacement of air due to its lower density than air. It is not collected over water due to its high solubility in water.

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Aqueous ammonia solution

Dissolving ammonia gas in water produces an aqueous solution, also known as ammonium hydroxide.

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Haber process

The industrial method for large-scale ammonia production that involves reacting hydrogen gas and nitrogen gas under high pressure, high temperature, and with a catalyst.

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Haber process conditions

The Haber process requires a high pressure (900 atm), a high temperature (450–500°C), and an iron catalyst.

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Catalyst in Haber process

Catalysts like iron oxide with molybdenum are used to speed up the rate of ammonia formation in the Haber-Bosch process without altering the equilibrium of the reaction.

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Reversible and exothermic reaction

The Haber process is a reversible reaction that releases heat (exothermic).

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Why ammonia is not collected over water

Ammonia gas is highly soluble in water, meaning it dissolves quickly into water, and thus collecting it atop a body of water would prove impractical.

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Heat on Nitrates

Heating nitrates produces nitrogen dioxide gas, causing brown fumes.

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Nitrate decomposition

The breakdown of nitrates leads to the release of brown nitrogen dioxide gas.

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Copper and Nitric Acid

Copper reacts with nitric acid to give nitrogen dioxide fumes.

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Nitrate and FeSO4

A brown ring reaction occurs when freshly prepared ferrous sulphate and concentrated nitric acid are mixed

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Nitric Acid Uses

Nitric acid is used to make explosives, fertilizers, dyes, drugs, synthetic fibres, and for purifying metals.

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Nitrogen Fixation

The process where atmospheric nitrogen is converted to nitrogenous compounds in the soil by bacteria.

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Laboratory Preparation of Nitric Acid

Nitric acid is prepared by distilling a mixture of sodium or potassium nitrate with concentrated sulfuric acid.

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Ostwald's Process

A large-scale method for preparing nitric acid involving the catalytic oxidation of ammonia.

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Nitric Acid Concentration

Nitric acid can be concentrated up to roughly 68% by distillation; 98% concentration is reached by dehydration with sulfuric acid.

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Nitric Acid Properties (Color/Smell)

Nitric acid is a colorless, sour-tasting liquid with a suffocating smell.

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Nitric Acid Solubility

Nitric acid is highly soluble in water.

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Nitric Acid Oxidizing Property

Nitric acid readily decomposes to liberate nascent oxygen, which acts as an electron acceptor, making it a strong oxidizing agent.

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Nitric Acid Oxidation of Metals

Nitric acid can oxidize most metals except noble metals (gold & platinum), producing respective salts and hydrogen gas. Product nature depends on acid concentration and temperature.

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Sulphuric Acid Occurrence

Sulphuric acid can be found naturally in hot water sulphur springs and in combined states like Barytes (BaSO4), Gypsum (CaSO4.2H2O), and Kieserite (MgSO4.H2O).

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Contact Process

A method used to manufacture sulfuric acid by converting sulfur dioxide to sulfur trioxide in the presence of a catalyst, followed by absorption in sulfuric acid to form oleum, and finally dilution with water.

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Favorable Conditions for SO2 to SO3 Conversion

This exothermic reaction favors a temperature of 410-450°C, a pressure of 1-2 atm, excess oxygen, and the use of a catalyst like V2O5.

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Oleum

A fuming sulfuric acid solution that contains dissolved sulfur trioxide (SO3) in sulfuric acid (H2SO4), represented as H2S2O7.

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Physical Properties of Sulfuric Acid

Sulfuric acid is a colorless, odorless, dense liquid with an oily texture. It has a specific gravity of 1.84 at 298 K, freezes at 283 K, and boils at 611 K. It dissolves in water with the release of significant heat.

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Chemical Properties of Sulfuric Acid

Its chemical reactivity is due to its low volatility, strong acidic character, strong affinity for water, and ability to act as an oxidizing agent.

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Dissociation of H2SO4 in Water

Sulfuric acid ionizes in water to release hydrogen ions (H+) and bisulfate ions (HSO4-) in the first step, which then further ionizes to release hydronium ions (H3O+) and sulfate ions (SO42-) in the second step. The dissociation constants (Ka1 and Ka2) indicate the strength of the acid.

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Why is H2SO4 a strong acid?

The large dissociation constant (Ka1) indicates that sulfuric acid (H2SO4) is largely dissociated into H+ and HSO4- ions. A larger dissociation constant means a stronger acid.

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Study Notes

Hydrogen Chloride (HCl)

  • Discovered by Glauber in 1648
  • Prepared by heating sodium chloride with concentrated sulphuric acid
  • Small quantities found in volcanic gases and gastric juice
  • Lab preparation involves heating sodium chloride in a dry round-bottomed flask
  • Concentrated sulfuric acid is added dropwise from a thistle funnel
  • Gas is dried using concentrated sulfuric acid
  • Collected by upward displacement of water (lighter than air)
  • Extremely soluble in water, forming hydrochloric acid
  • Colourless and pungent-smelling gas
  • Boiling point: 189 K; Freezing point: 159 K
  • Forms dense white fumes with ammonia
  • Turns blue litmus red and decolourises pink phenolphthalein

Chemical Properties

  • Neither combustible nor supports combustion
  • Dissociates into hydrogen and chlorine at 500°C
  • Reacts with metals to form chlorides and hydrogen gas (e.g., Ca + 2HCl → CaCl2 + H2)
  • Reacts with metallic oxides, hydroxides, carbonates and sulphides
  • Decomposes salts of weaker acids

Hydrochloric Acid (HCl)

  • Formed by the dissolution of hydrogen chloride gas in water
  • Strong acid
  • Colourless and pungent-smelling
  • High boiling and melting points than hydrogen chloride due to intermolecular hydrogen bonding
  • Turns blue litmus to red
  • Corrosive

Ammonia (NH3)

  • Discovered by Claude Berthollet in 1785
  • Exists in free state (air and natural water) and in combined state(distillation of coal or wood) or volcanic eruptions
  • Trigonal pyramidal structure, with nitrogen at the apex and three hydrogen atoms
  • Formed by reaction with caustic alkali on warming ammonium salts with
  • Extremely soluble in water (forming liquor ammonia and reacts with metal oxides)
  • Lighter than air (vapour density: 8.5)
  • Used in the production of nitrogen fertilizers, dyes, and drugs

Preparation of Ammonia

  • Heating ammonium salts with a base (e.g., 2NH4Cl + Ca(OH)2 → 2NH3 + CaCl2 + 2H2O)

Properties of Ammonia

  • Pungent odour
  • Colourless
  • Basic
  • Turns red litmus blue
  • Soluble in water
  • Extremely soluble in water
  • Extremely soluble in water and can be collected by downward displacement of air.

Oxidation of Ammonia

  • In excess of oxygen, ammonia burns with a yellwo flame producing nitrogen and water
  • Catalysed oxidation using platinum filament, producing nitrogen oxides

Uses of Ammonia

  • Production of nitrogen fertilizers
  • Cleaning agent
  • Manufacturing of artificial silk
  • Laboratory reagent
  • Refrigerant (liquid ammonia)

Nitric Acid (HNO3)

  • Also known as aqua fortis
  • Laboratory preparation involves heating a mixture of sodium/potassium nitrate with concentrated sulfuric acid in a glass retort
  • Yellow-brown liquid
  • Highly soluble in water
  • Strong acid

Preparation of Nitric Acid

  • Prepared by the oxidation of ammonia in the presence of a catalyst
  • Laboratory preparation involves distillation of a mixture of sodium/potassium nitrate with concentrated sulphuric acid
  • Reacts with metal oxides, hydroxides, carbonates, and hydrogen carbonates, forming respective nitrates
  • Acts as a strong oxidising agent

Uses of Nitric Acid

  • Production of fertilizers
  • Manufacturing of explosives
  • Purification of gold
  • Rocket fuel
  • Laboratory reagent

Sulphuric Acid (H2SO4)

  • Also known as oil of vitriol
  • A vital industrial chemical
  • Acidic, corrosive liquid
  • Preparation done by contact process (burning sulphur to make SO2, reaction with O2 and catalyst to make SO3, reaction with water to make H2SO4)

Properties of Sulphuric Acid

  • Colourless, odourless, and oily liquid
  • Strong acid
  • Dehydrating agent
  • Strong oxidising agent.
  • Used in industries, metallurgical applications and other applications.

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Hydrochloric Acid PDF

Description

Test your knowledge on various aspects of ammonia production and related chemical reactions in this quiz. Topics include the preparation of ammonia, the properties of acids, and the reactions involving nitrates. Ideal for students studying advanced chemistry concepts.

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