ICSE CHEMISTRY CLASS 10 AMMONIA

SECTION A — MULTIPLE-CHOICE QUESTIONS (10 × 1 = 10 marks)

1. In the laboratory, ammonia is commonly prepared by heating ammonium chloride with:

A. dilute hydrochloric acid

B. calcium hydroxide

C. calcium carbonate

D. sodium chloride

2. The drying agent suitable for ammonia gas is:

A. concentrated sulphuric acid

B. anhydrous calcium chloride

C. quicklime

D. phosphorus pentoxide

3. Ammonia is collected by downward displacement of air because it is:

A. denser than air and insoluble in water

B. lighter than air and highly soluble in water

C. lighter than air and insoluble in water

D. denser than air and highly soluble in water

4. Which observation confirms that ammonia is alkaline in aqueous solution?

A. Blue litmus turns red

B. Red litmus turns blue

C. Limewater turns milky

D. A glowing splint relights

5. When ammonia gas comes in contact with hydrogen chloride gas, the visible product is:

A. brown fumes of nitrogen dioxide

B. white fumes of ammonium chloride

C. yellow sulphur

D. colourless water vapour

6. The catalyst used in the Haber process is usually:

A. nickel

B. manganese dioxide

C. finely divided iron

D. platinum gauze

7. The synthesis of ammonia in the Haber process is:

A. endothermic and irreversible

B. exothermic and reversible

C. endothermic and reversible

D. exothermic and irreversible

8. Which change favours a higher equilibrium yield of ammonia in the Haber process?

A. Decreasing pressure

B. Increasing pressure

C. Increasing temperature indefinitely

D. Removing nitrogen from the mixture

9. The volume ratio of nitrogen to hydrogen used in the Haber process is:

A. 1:1

B. 1:2

C. 1:3

D. 3:1

10. Ammonia forms ammonium ions in water because it:

A. donates a proton to water

B. accepts a proton from water

C. releases oxygen

D. decomposes water into hydrogen and oxygen

SECTION B — OBSERVATION-BASED QUESTIONS (2 × 2 = 4 marks)

11. A glass rod dipped in concentrated hydrochloric acid is held near a jar containing ammonia gas. (a) State the observation. (b) Name the white solid formed.

12. A few drops of water are introduced into a flask filled with dry ammonia gas, and the flask is connected to a water source containing red litmus solution. (a) Describe the fountain/colour change observed. (b) Explain why the change occurs.

SECTION C — CASE-STUDY QUESTIONS (2 × 3 = 6 marks)

13. Industrial manufacture of ammonia

A fertiliser plant combines nitrogen obtained from air with hydrogen, then passes the mixture over a catalyst at high pressure and a moderately high temperature. The reaction releases heat and reaches equilibrium.

(a) Write the balanced equation for the Haber process. (1)

(b) State the approximate pressure and temperature commonly used at school level. (1)

(c) Explain why a very low temperature is not used industrially, even though the forward reaction is exothermic. (1)

14. Laboratory preparation and collection

A student heats a mixture of ammonium chloride and calcium hydroxide. The gas produced is passed through a drying tower and collected in an inverted dry gas jar.

(a) Write the balanced equation for the laboratory preparation of ammonia. (1)

(b) Name the drying agent used. (1)

(c) Why must ammonia not be collected over water? (1)

The periodic properties ICSE

ICSE Class 10 Chemistry – Periodic Properties

1. The modern periodic law states that the properties of elements are periodic functions of their:

A) Atomic masses

B) Atomic numbers

C) Mass numbers

D) Neutron numbers

2. Which of the following has the smallest atomic radius?

A) Na

B) Mg

C) Al

D) Cl

3. Across a period from left to right, the atomic size generally:

A) Increases

B) Decreases

C) Remains constant

D) First increases and then decreases

4. Which element has the highest ionisation potential among the following?

A) Na

B) Mg

C) Al

D) Cl

5. The tendency of an atom to attract the shared pair of electrons towards itself is called:

A) Ionisation energy

B) Electron affinity

C) Electronegativity

D) Atomicity

6.Which of the following elements has the highest electronegativity?

A) F

B) Cl

C) Br

D) I

7.On moving down a group, the atomic size generally:

A) Decreases

B) Increases

C) Remains unchanged

D) Becomes zero

8. Which pair of elements belongs to the same group?

A) Na and Mg

B) Li and Na

C) Na and Cl

D) Mg and Cl

9.Metallic character generally ______ from left to right across a period.

A) Increases

B) Decreases

C) Remains the same

D) First decreases and then increases

10.An element has electronic configuration 2, 8, 7. It belongs to:

A) Group 1, Period 3

B) Group 17, Period 3

C) Group 17, Period 2

D) Group 18, Period 3

Answers

1. B) Atomic numbers

2. D) Cl

3. B) Decreases

4. D) Cl

5. C) Electronegativity

6. A) F

7. B) Increases

8. B) Li and Na

9. B) Decreases

10. B) Group 17, Period 3

ICSE MCQs Chemistry Ammonia - Study of Compounds

ICSE Chemistry MCQs

ICSE Chemistry – Ammonia

1. What is the molecular formula of ammonia?

A) NH₄

B) NH₃

C) N₂H₄

D) NO₃

Answer: B) NH₃

2. Ammonia is a:

A) Colourless gas with a pungent smell

B) Yellow gas with a sweet smell

C) Blue liquid

D) Colourless liquid with no smell

Answer: A) Colourless gas with a pungent smell

3. Ammonia is highly soluble in:

A) Kerosene

B) Water

C) Benzene

D) Carbon tetrachloride

Answer: B) Water

4. The laboratory preparation of ammonia involves heating:

A) Sodium chloride with sulphuric acid

B) Ammonium chloride with calcium hydroxide

C) Ammonium nitrate with water

D) Nitrogen with hydrogen

Answer: B) Ammonium chloride with calcium hydroxide

5. The drying agent commonly used for ammonia is:

A) Concentrated H₂SO₄

B) Anhydrous CaCl₂

C) Quicklime (CaO)

D) P₂O₅

Answer: C) Quicklime (CaO)

6. Ammonia cannot be dried using concentrated sulphuric acid because it:

A) Is insoluble in H₂SO₄

B) Reacts with H₂SO₄

C) Decomposes H₂SO₄

D) Evaporates H₂SO₄

Answer: B) Reacts with H₂SO₄

7. The gas collected in the laboratory preparation of ammonia is collected by:

A) Downward displacement of water

B) Upward displacement of air

C) Downward displacement of air

D) Over mercury

Answer: C) Downward displacement of air

8. Ammonia is lighter than:

A) Hydrogen

B) Oxygen

C) Helium

D) Nitrogen

Answer: B) Oxygen

9. Ammonia turns moist red litmus paper:

A) Blue

B) Green

C) Yellow

D) White

Answer: A) Blue

10. The aqueous solution of ammonia is commonly called:

A) Ammonium hydroxide

B) Ammonium chloride

C) Ammonium nitrate

D) Ammonium sulphate

Answer: A) Ammonium hydroxide

11. Ammonia reacts with hydrogen chloride gas to form:

A) NH₄OH

B) NH₄Cl

C) N₂

D) H₂

Answer: B) NH₄Cl

12. The reaction between NH₃ and HCl produces:

A) Brown fumes

B) White fumes

C) Green fumes

D) No visible change

Answer: B) White fumes

13. Ammonia is a:

A) Strong acid

B) Weak acid

C) Strong alkali

D) Weak alkali

Answer: D) Weak alkali

14. The catalyst used in the Haber process is mainly:

A) Copper

B) Iron

C) Nickel

D) Platinum

Answer: B) Iron

15. The Haber process is used for the manufacture of:

A) Nitric acid

B) Ammonia

C) Sulphuric acid

D) Hydrochloric acid

Answer: B) Ammonia

16. The reactants used in the Haber process are:

A) Nitrogen and oxygen

B) Nitrogen and hydrogen

C) Hydrogen and oxygen

D) Nitrogen and chlorine

Answer: B) Nitrogen and hydrogen

17. The balanced equation for the Haber process is:

A) N₂ + H₂ → NH₃

B) N₂ + 2H₂ → 2NH₃

C) N₂ + 3H₂ ⇌ 2NH₃

D) 2N₂ + H₂ ⇌ 2NH₃

Answer: C) N₂ + 3H₂ ⇌ 2NH₃

18. In the Haber process, increasing pressure favours the formation of:

A) Nitrogen

B) Hydrogen

C) Ammonia

D) Oxygen

Answer: C) Ammonia

19. Ammonia reacts with oxygen in the presence of platinum to form:

A) Nitrogen dioxide directly

B) Nitric oxide and water

C) Nitrogen and water

D) Nitric acid directly

Answer: B) Nitric oxide and water

20. The oxidation of ammonia in the Ostwald process is carried out using:

A) Copper catalyst

B) Iron catalyst

C) Platinum catalyst

D) Zinc catalyst

Answer: C) Platinum catalyst

21. Ammonia can reduce heated metal oxides such as:

A) CuO

B) Na₂O

C) K₂O

D) CaO

Answer: A) CuO

22. When ammonia reacts with copper(II) oxide on heating, the black CuO changes to:

A) Green copper carbonate

B) Reddish-brown copper

C) Blue copper sulphate

D) White copper chloride

Answer: B) Reddish-brown copper

23. Ammonia is used in the manufacture of:

A) Fertilisers

B) Glass only

C) Cement only

D) Sodium chloride

Answer: A) Fertilisers

24. Which property of ammonia makes it suitable for fountain experiment?

A) It is highly soluble in water

B) It is heavier than water

C) It is insoluble in water

D) It is a liquid at room temperature

Answer: A) It is highly soluble in water

25. Which of the following is NOT a property of ammonia?

A) It has a pungent smell

B) It is highly soluble in water

C) It is a basic gas

D) It is heavier than air

Answer: D) It is heavier than air

Icse chemistry class 10 worksheet

Icse chemistry class 10 worksheet- Study of Compounds 

1. PERIODIC PROPERTIES

1. Explain why atomic radius generally decreases from left to right across a period.

2. Arrange Na, Mg, Al and Si in increasing order of atomic radius. Explain your answer.

Case Study Question

A student compares four Period 3 elements: Na, Mg, Al and Cl. The atomic size becomes progressively smaller across the period.

(a) What causes the decrease in atomic size?

(b) Which of the four has the highest electronegativity?

(c) Which would form the largest positive ion?

(d) State the general trend of first ionisation energy across a period.

2. CHEMICAL BONDING

1. Using electron-dot structures, explain the formation of magnesium chloride, MgCl₂.

2. Differentiate between an electrovalent bond and a covalent bond with respect to formation and electrical conductivity.

Case Study Question

Compound X has a high melting point and conducts electricity when molten but not when solid. Compound Y has a low melting point and does not conduct electricity in either state.

(a) Identify the likely type of bonding in X and Y.

(b) Explain the electrical conductivity of X.

(c) Give one example of Y.

(d) State why X is brittle.

3. ELECTROLYSIS

1. Describe the electrolysis of molten lead(II) bromide and write the half-equations at both electrodes.

2. Explain the principle of electroplating. Describe how an iron article can be coated with copper.

Case Study Question

A student electrolyses aqueous copper(II) sulphate using copper electrodes.

(a) Which electrode gains mass?

(b) Which electrode loses mass?

(c) Write the cathode half-equation.

(d) Explain why the concentration of CuSO₄ solution remains approximately unchanged.

4. METALLURGY

1. Explain the functions of coke, limestone and hot air in the extraction of iron in a blast furnace.

2. Differentiate between roasting and calcination. Give one chemical equation for each process.

Case Study Question

An ore contains iron(III) oxide mixed with earthy impurities. In a blast furnace, coke and limestone are added.

(a) What is the function of coke?

(b) What is the function of limestone?

(c) What is slag?

(d) Write the equation for the reduction of Fe₂O₃ by CO.

5. HYDROGEN CHLORIDE

1. Describe the laboratory preparation of hydrogen chloride gas from sodium chloride. Write the balanced equation.

2. Explain why hydrogen chloride gas shows acidic properties only in the presence of moisture.

Case Study Question

A jar containing dry HCl gas is connected to a fountain apparatus and water is introduced.

(a) What happens to the water level?

(b) Why is HCl highly soluble in water?

(c) What happens to moist blue litmus?

(d) Write the reaction between HCl and NH₃.

6. NITRIC ACID

1. Describe the oxidising action of concentrated nitric acid on copper. Write the balanced equation and identify the gas evolved.

2. What is aqua regia? State its composition and one important use.

Case Study Question

Copper reacts with concentrated nitric acid and produces a blue solution with brown fumes.

(a) Identify the brown gas.

(b) Why is the solution blue?

(c) Is nitric acid acting as an oxidising agent? Explain.

(d) Write the balanced equation.

7. SULPHURIC ACID

1. Describe the Contact Process for the manufacture of sulphuric acid, mentioning the catalyst and important conditions.

2. Explain the dehydrating action of concentrated sulphuric acid using sugar as an example.

Case Study Question

In a Contact Process plant, SO₂ is converted to SO₃ before the final absorption step.

(a) Name the catalyst.

(b) Write the reversible equation for SO₂ oxidation.

(c) Why is SO₃ not absorbed directly in water?

(d) Name the substance formed when SO₃ is absorbed in concentrated sulphuric acid.

8. ACIDS AND BASES

1. Distinguish between strong and weak acids in terms of ionisation in water. Give one example of each.

2. A solution has [H⁺] = 1 × 10⁻⁴ mol L⁻¹. Calculate its pH and state whether it is acidic or alkaline.