S.P. Singh solutions for कन्साइस केमिस्ट्री [अंग्रेजी] कक्षा १० आईसीएसई chapter 9 - Study of Compounds B. Ammonia [Latest edition]

State the type of bonding present in ammonia, show by a diagram.

What is the formula for liquid ammonia?

Account for the basic nature of liquid ammonia compound.

Write a balanced chemical equation for the lab preparation of ammonia.

How is ammonia dried and collected in the laboratory?

Ammonia cannot be collected over water. Give reason.

Explain with a diagram the preparation of aqueous ammonia.

Why drying agents such as P₂O₅ and CaCl₂ are not used to dry NH₃?

A substance ‘A’ was heated with slaked lime and a gas ‘B’ with the pungent smell was obtained. Name the substances A and B and give a balanced equation.

Ammonia is manufactured by Haber Process.

Under what conditions do the reactants combine to form ammonia? Give a balanced equation for the reaction.

Ammonia is manufactured by Haber Process.

In what ratio by volume, are the above gases used?

Ammonia is manufactured by Haber Process.

State one possible source of each reactant used in Haber process.

Ammonia is manufactured by Haber Process.

State whether the formation of ammonia is promoted by the use of high pressure or low pressure?

Ammonia is manufactured by Haber Process.

Mention two possible ways by which ammonia produced is removed from unchanged gases.

Ammonia is manufactured by Haber Process.

What is the function of finely divided iron?

Ammonia is manufactured by Haber Process.

What is the function of molybdenum in the above process?

Ammonia is manufactured by Haber Process.

What is the percentage formation of ammonia?

Ammonia is manufactured by Haber Process.

How can this percentage formation be increased?

Give reasons:

Ammonium compounds do not occur as minerals.

Give reasons:

Ammonium nitrate is not used in the preparation of ammonia.

Give reasons:

Conc. H₂SO₄ is a good drying agent, yet it is not used to dry NH_3.

Give reasons:

In the lab, preparation of ammonia calcium hydroxide is used in excess.

Give reasons:

In the lab, preparation of ammonia flask is fitted in slanting position.

State the following condition required in the Haber’s process:

Temperature

State the following condition required in the Haber’s process:

Pressure

State the following condition required in the Haber’s process:

Catalyst

Choose the correct word or phrase from the options to complete the following sentence and write balanced equation for the same.

Ammonium chloride is a soluble salt prepared by ______.

Choose the correct word or phrase from the options to complete the following sentence and write balanced equation for the same.

When ammonium chloride is heated, it undergoes ______.

Choose the correct word or phrase from the options to complete the following sentence and write balanced equation for the same.

Heating ammonium chloride with sodium hydroxide produces ______.

An element has 2 electrons in its N shell. It reacts with a non-metal of atomic number 7. The compound formed reacts with warm water and produces a basic gas. Identify the elements and write a balanced chemical reaction.

The following reactions are carried out:

A: \[\ce{Nitrogen + metal -> compound X}\]

B: \[\ce{X + water -> ammonia + another compound}\]

C: \[\ce{Ammonia + metal oxide -> metal + water + N2}\]

One metal that can be used for reaction A is magnesium.

1. Write the formula of the compound X formed.
2. Write the correctly balanced equation for reaction B where X is the compound formed.
3. What property of ammonia is demonstrated by reaction C?

Correct the following:

A reddish brown precipitate is obtained when ammonium hydroxide is added to ferrous sulphate.

Correct the following:

Liquid ammonia is a solution of NH₃.

Correct the following:

Finely divided platinum is used in the Haber process.

Correct the following:

Conc. H₂SO₄ is a drying agent for NH₃.

Correct the following:

Ammonium salts, on heating, decompose to give ammonia.

Ammonia can be obtained by adding water to ______.

The catalyst used in Haber’s process is ______.

Nitrogen gas can be obtained by heating ______.

Ammonia can be obtained by adding water to ______.

The gas collected by downward displacement of air is ______.

In the Haber’s process, the ratio of reactants nitrogen and hydrogen is ______.

When ammonia reacts with an excess of chlorine, the main product formed is ______.

Ammonia is used in ______.

In the following set up for burning ammonia in oxygen, ammonia tube is fitted higher and oxygen tube is kept lower because?

P Oxygen is lighter than ammonia.

Q Ammonia is lighter than oxygen.

R Ammonia and oxygen mixture is explosive and by keeping them in this position, limited oxygen will react with ammonia.

Which of the following is true?

Assertion (A): Ammonia does not conduct electricity in gaseous or liquid state.

Reason (R): Ions in ammonia gas or liquid ammonia are not free to move.

1. Both A and R are true and R is the correct explanation of A.
2. Both A and R are true but R is not the correct explanation of A.
3. A is true but R is false.
4. A is false but R is true.

Assertion (A): Ammonia is dried by passing through a drying tower containing CaO.

Reason (R): Ammonia being basic in nature reacts with other drying agents.

1. Both A and R are true and R is the correct explanation of A.
2. Both A and R are true but R is not the correct explanation of A.
3. A is true but R is false.
4. A is false but R is true.

Assertion (A): Ammonia and its compounds do not occur in minerals.

Reason (R): Ammonia is not soluble in water.

1. Both A and R are true and R is the correct explanation of A.
2. Both A and R are true but R is not the correct explanation of A.
3. A is true but R is false.
4. A is false but R is true.

Assertion (A): In the preparation of ammonia, hydrogen is obtained by Bosch process.

Reason (R): Hydrogen and nitrogen are used in the ratio 1: 3.

1. Both A and R are true and R is the correct explanation of A.
2. Both A and R are true but R is not the correct explanation of A.
3. A is true but R is false.
4. A is false but R is true.

Assertion (A): Haber’s process is used to manufacture ammonia.

Reason (R): The catalyst used in this process is vanadium oxide or platinum.

1. Both A and R are true and R is the correct explanation of A.
2. Both A and R are true but R is not the correct explanation of A.
3. A is true but R is false.
4. A is false but R is true.

Assertion (A): Ammonia is recovered by liquification process in Haber’s process.

Reason (R): Nitrogen and hydrogen liquify with difficulty as compared to ammonia.

1. Both A and R are true and R is the correct explanation of A.
2. Both A and R are true but R is not the correct explanation of A.
3. A is true but R is false.
4. A is false but R is true.

Assertion (A): Liquid ammonia is used as a refrigerant in ice plants.

Reason (R): CFC, the main refrigerant, causes global warming.

1. Both A and R are true and R is the correct explanation of A.
2. Both A and R are true but R is not the correct explanation of A.
3. A is true but R is false.
4. A is false but R is true.

Match the following:

Ammonia gas is collected by ______.

Ammonia reacts with excess chlorine to form ______.

Complete the blanks (i) to (v) in the passage given, using the following words. 

[Ammonium, reddish brown, hydroxyl, nitrogen dioxide, ammonia, dirty green, alkaline, acidic].

In the presence of a catalyst nitrogen and hydrogen combine to give (i) ______ gas. When the same gas is passed through water it forms a solution, which will be (ii) ______ in nature, and will contain the ions (iii) ______ and (iv) ______. A (v) ______ coloured precipitate of iron [II] hydroxide is formed when the above solution is added to iron [II] sulphate solution.

Name the gas which is prepared by Haber’s process.

Name two gases which give dense white fumes with ammonia.

Name one salt of ammonia that is used in a dry cell.

Name one salt of ammonia that is used in explosives.

Name one salt of ammonia that is used in medicine.

Name an acidic gas which reacts with a basic gas liberating a neutral gas.

Name a metallic chloride soluble in ammonium hydroxide.

Name the gas obtained when ammonia burns in an atmosphere of oxygen without any catalyst.

Name a nitride of a divalent metal which reacts with warm water liberating ammonia.

Name an amphoteric oxide reduced by the basic gas.

Name a white salt produced by an acid gas and a basic gas.

Name the gas evolved in each case [formula is not acceptable]. The gas that burns in oxygen with a green flame.

Name the gas produced when excess ammonia reacts with chlorine.

Name the white crystalline solid that is soluble in water which liberates a pungent smelling gas when heated with sodium hydroxide solution.

Identify an alkaline gas which produces dense white fumes when reacted with HCl gas.

Name the gas evolved when the following mixtures are heated.

Calcium hydroxide and ammonium chloride.

Name the gas evolved when the following mixtures are heated.

Sodium nitrite and ammonium chloride.

From the list of gases - ammonia, ethane, hydrogen chloride, hydrogen sulphide. Select the gas which is used as a reducing agent in reducing copper oxide to copper.

A gas ‘P’ gives dense white fumes with chlorine. Its aqueous solution gives a blue colour with copper (II) hydroxide. Give the name and formula of the gas P.

Copy and complete the following table relating to important industrial process:

Copy and complete the following equations:

1. \[\ce{AlN + H2O ->}\]
2. \[\ce{2NH3 + 3PbO ->}\]
3. \[\ce{NH3 + 3Cl2 ->}\]
4. \[\ce{NH3 + CO2 ->}\]

1. 1. Which property of ammonia is illustrated by equation (c)?
   2. What important fertiliser is prepared from equation (d)? State the conditions.

Pick the odd member from the list, giving reasons:

Pick the odd member from the list, giving reasons:

State two relevant observations of the following:

Ammonium hydroxide solution is added to zinc nitrate solution in minimum quantities and then in excess.

What do you observe when ammonium hydroxide is added to the aqueous solution of FeSO₄? Write a balanced equation for this.

What do you observe when ammonium hydroxide is added to the aqueous solution of Iron (III) chloride? Write a balanced equation for this.

What do you observe when ammonium hydroxide is added to the aqueous solution of Lead nitrate? Write a balanced equation for this.

What do you observe when ammonium hydroxide is added to the aqueous solution of Zinc nitrate? Write a balanced equation for this.

When ammonium hydroxide is added to solution B, a pale blue precipitate is formed. This pale blue precipitate dissolves in excess ammonium hydroxide, giving an inky blue solution. What is the cation [positive ion] present in solution B? what is the probable colour of solution B?

Write the equation for the action of heat on ammonium chloride.

State whether the reaction is an example of thermal decomposition or thermal dissociation.

Write the equation for the action of heat on ammonium nitrate.

State whether the reaction is an example of thermal decomposition or thermal dissociation.

Name two gases which can be used in the study of the fountain experiment.

State the common property demonstrated by the fountain experiment.

Name the other ion formed when ammonia dissolves in water. Give one test that can be used to detect the presence of the ion produced.

State the conditions required for the given reaction to take place:

Catalytic oxidation of ammonia to nitric oxide.

Give reasons for the following:

Liquid ammonia is used as a refrigerant in ice plants.

Give reasons for the following:

Aqueous solution of ammonia is used for removing grease stains from woollen clothes.

Give reasons for the following:

Aqueous solution of ammonia gives a pungent smell.

Give reasons for the following:

Aqueous solution of ammonia conducts electricity.

Give a balanced equation:

Ammonium hydroxide is added to ferrous sulphate solution.

Write a balanced equation for the action of warm water on magnesium nitride.

Give the equation for the reaction:

Ammonium chloride is heated with sodium hydroxide.

Write a balanced chemical equation:

Chlorine reacts with excess of ammonia.

Give a balanced equation for the reaction:

Ammonia and oxygen in the presence of a catalyst.

Give a balanced equation for the reduction of hot copper (II) oxide to copper using ammonia gas.

Write a balanced chemical equation for the following:

An equation to illustrate the reducing nature of ammonia.

Give a balanced chemical equation for the following:

Lab. preparation of ammonia using an ammonium salt.

Give a balanced chemical equation for the following:

Reaction of ammonia with excess of chlorine.

Give a balanced chemical equation for the following:

Reaction of ammonia with sulphuric acid.

Write a balanced chemical equation for the following:

When an excess of ammonia is treated with chlorine.

Write a balanced equation for a reaction in which ammonia is oxidized by:

A metal oxide

Write a balanced chemical equation for a reaction in which ammonia is oxidised by the following:

A gas which is not oxygen.

Write a relevant equation to show that ammonia acts as a reducing agent.

Rewrite the correct statement with the missing word/s:

Magnesium nitride reacts with water to liberate ammonia.

Distinguish between the following (using ammonia solution):

Calcium chloride and zinc chloride

Distinguish between the following (using ammonia solution):

Ferric salt and ferrous salt

Distinguish between the following (using ammonia solution):

Zinc nitrate and lead nitrate

Give a balanced equation for the following conversion:

Ammonia to nitrogen using an acidic gas.

Give a balanced equation for the following conversion:

Ammonia to brown gas.

Give a balanced equation for the following conversion:

Ammonia to nitrogen trichloride.

Give a balanced equation for the following conversion:

Ammonia solution to an amphoteric hydroxide.

Give a balanced equation for the following conversion:

A nitride of a trivalent metal to ammonia.

Give a balanced equation for the following conversion:

Lead oxide to lead.

Distinguish between the following pair of compound using the test given within bracket.

Iron (II) sulphate and iron (III) sulphate (using ammonium hydroxide)

Distinguish between the given pair of compounds using the test given within bracket:

A lead salt and a zinc salt (using excess ammonium hydroxide)

Write observations:

Ammonia gas is passed over heated copper (II) oxide.

State your observation when, in the absence of a catalyst, ammonia is burnt in an atmosphere of oxygen.

What would you observe in the following case:

Ammonium hydroxide is first added in a small quantity and then in excess to a solution of copper sulphate.

State your observation:

Water is added to the product formed when Al is burnt in a jar of nitrogen gas.

State one appropriate observation for excess of chlorine gas is reacted with ammonia gas.

State your observation of the following case:

When calcium hydroxide is heated with ammonium chloride crystals.

Is ammonia more dense or less dense than air?

What property of ammonia is demonstrated by the fountain experiment?

Write the balanced equation for the reaction between ammonia and sulphuric acid.

Ammonia solution in water gives a blue precipitate when it combines with a solution of copper salt. The blue precipitate further dissolves in excess of an ammonia solution to give the azure blue solution. Explain with the equation.

Give the chemical equation(s) to prove that NH₃ contains nitrogen and hydrogen.

When an ammonium salt is warmed with sodium hydroxide solution, a gas is evolved. State three ways in which you could identify this gas.

A gas ‘A’ reacts with another gas ‘B’ in the presence of a catalyst to give a colourless gas ‘C’. The gas ‘C’ when comes in contact with air produces a brown gas ‘D’. The solution of ‘A’ in water turns red litmus blue. Explain the observations.

Name the common refrigerant. How does it deplete the ozone layer?

What is the alternative of chlorofluorocarbon?

State the advantages of using ammonia as a refrigerant?

State the disadvantages of using ammonia as refrigerent?

1. Which feature of the ammonia molecule leads to the formation of the ammonium ion when ammonia dissolves in water?
2. Name the other ion formed when ammonia dissolves in water.
3. Give one test that can be used to detect the presence of the ion produced in (b).

1. Of the two gases, ammonia and hydrogen chloride, which is more denser? Name the method of collection of this gas.
2. Give one example of a reaction between the above two gases which produces a solid compound.

Study the flow chart given and give balanced equations to represent the reactions A, B and C:

\[\ce{Mg3N2 ->[A] NH3 <=>[B][C] NH4Cl}\]

In the manufacture of ammonia:

1. Name the process.
2. State the ratio of the reactants taken.
3. State the catalyst used.
4. Give the equation for the manufacture of the gas – ammonia.

Explain the following:

Ammonium nitrate is not used in the laboratory preparation of NH₃.

The following questions are based on the preparation of ammonia gas in the laboratory:

How is ammonia gas collected? Explain why it is not collected over water.

The diagram shows an experimental set up for the laboratory preparation of a pungent smelling gas. The gas is alkaline in nature.

1. Nature the gas collected in the jar.
2. Write the balance equation for the above preparation.
3. How is the gas being collected?
4. Name the drying agent used.
5. How will you find that the jar is full of gas?

Answer the following questions with respect to the given figure.

1. Identify gas P and gas Q.
2. Give a balanced equation to convert ammonia into gas P by a method other than decomposition. State the property of ammonia used in carrying out the conversion.
3. Name fertiliser S and give a balanced equation for its preparation.
4. Name process T and state the conditions that enable conversion of ammonia to nitric oxide.
5. Give a balanced equation for the conversion of brown gas to liquid U.
6. Name fertiliser A.
7. Name process R.

The diagram given below describes the manufacturing
process of a gas.

1. Name the process.
2. Identify A, B and C.
3. State the ratio of A and B.
4. Write the equation involved with their respective conditions.
5. How is the product separated from unreacted reactants?