ICSE Class 10

General instructions: Answer all questions. Marks are shown in brackets [ ].

Objective

1. 1.
   Why should only all-glass apparatus be used for the preparation of nitric acid by heating concentrated sulphuric acid and potassium nitrate?

   1. A. Glass is inexpensive and widely available, making it a convenient choice for laboratory use.
   2. B. Glass is inert and can withstand the corrosive nature of nitric acid and high temperatures without reacting.
   3. C. Glass apparatus speeds up the reaction, ensuring faster production of nitric acid.
   4. D. Glass prevents the escape of gases, ensuring no loss of reactants during the process.
   [1]
2. 2.
   Which gas is evolved when sodium nitrate is heated?

   1. A. Nitrogen dioxide
   2. B. Nitric oxide
   3. C. Oxygen (O₂)
   4. D. Nitrous oxide
   [1]
3. 3.
   Concentration of nitric acid obtained in Ostwald's process.

   1. A. 10%
   2. B. 5%
   3. C. 15%
   4. D. 20%
   [1]
4. 4.
   Nitrogen gas can be obtained by heating:

   1. a. Ammonium nitrate.
   2. b. Ammonium nitrite.
   3. c. Magnesium nitride.
   4. d. Ammonium chloride.
   [1]
5. 5.
   What observation is made when hot and concentrated nitric acid is added to sawdust?

   1. A. Sawdust dissolves without any visible change
   2. B. Formation of a brown gas and flames
   3. C. Sawdust turns black without flames
   4. D. Effervescence of hydrogen gas
   [1]
6. 6.
   The compound responsible for the brown ring during the brown ring test of nitrate ion.

   1. a. Nitrosoiron(II) sulphate
   2. b. Iron(III) chloride
   3. c. Chromium sulphate
   4. d. Lead(II) chloride
   [1]
7. 7.
   Which statement correctly describes the acidic behavior of nitric acid with metallic oxides and hydroxides, along with the correct balanced equations for each reaction?

   1. A. Nitric acid reacts with metallic oxides and hydroxides to form salt and water. CuO + 2HNO₃ → Cu(NO₃)₂ + H₂O; NaOH + HNO₃ → NaNO₃ + H₂O
   2. B. Nitric acid reacts with metallic oxides and hydroxides to form salt and hydrogen gas. CuO + HNO₃ → Cu(NO₃) + H₂; NaOH + HNO₃ → NaNO₃ + H₂
   3. C. Nitric acid reacts with metallic oxides and hydroxides to form salt, water, and nitrogen dioxide. CuO + 4HNO₃ → Cu(NO₃)₂ + 2H₂O + 2NO₂; NaOH + 2HNO₃ → NaNO₃ + H₂O + NO₂
   4. D. Nitric acid reacts with metallic oxides and hydroxides to form metallic nitrates only. CuO + HNO₃ → CuNO₃; NaOH + HNO₃ → NaNO₃
   [1]
8. 8.
   A solid which bursts into flames on addition of concentrated nitric acid is :

   1. A. Turpentine oil
   2. B. Sawdust
   3. C. Alcohol
   4. D. Ferric sulphate
   [1]
9. 9.
   Write the balanced chemical equation for the reaction of very dilute nitric acid with magnesium. Which gas is evolved in this reaction?

   1. A. Nitrogen dioxide (NO₂)
   2. B. Hydrogen (H₂)
   3. C. Nitric oxide (NO)
   4. D. Ammonia (NH₃)
   [1]
10. 10.
    Which of the following correctly completes the statement: 'Magnesium reacts with nitric acid to liberate hydrogen gas.'?

    1. A. Magnesium reacts with very dilute nitric acid to liberate hydrogen gas.
    2. B. Magnesium reacts with concentrated nitric acid to liberate hydrogen gas.
    3. C. Magnesium reacts with any nitric acid to liberate hydrogen gas.
    4. D. Magnesium reacts with nitric acid to liberate nitrogen gas.
    [1]
11. 11.
    Which balanced chemical equation correctly represents the preparation of nitric acid from potassium nitrate?

    1. A. KNO₃ + H₂SO₄ → KHSO₄ + HNO₃ (below 200°C)
    2. B. KNO₃ + H₂SO₄ → K₂SO₄ + HNO₃ (above 200°C)
    3. C. KNO₃ + HCl → KCl + HNO₃
    4. D. 2KNO₃ + H₂SO₄ → K₂SO₄ + 2HNO₃
    [1]
12. 12.
    Complete and balance the following chemical equation for the reaction of lead with concentrated nitric acid: Pb + HNO₃ → (Conc.)

    1. A. Pb + HNO₃ → PbNO₃ + NO₂↑ + H₂O
    2. B. Pb + 4HNO₃ → Pb(NO₃)₂ + 2NO₂↑ + 2H₂O
    3. C. Pb + 2HNO₃ → Pb(NO₃)₂ + H₂↑
    4. D. 2Pb + HNO₃ → Pb₂NO₃ + NO↑ + H₂O
    [1]
13. 13.
    What is the term used to describe iron that has been treated with pure concentrated nitric acid, resulting in the cessation of further reaction?

    1. A. Active iron
    2. B. Passive iron
    3. C. Rusty iron
    4. D. Galvanized iron
    [1]
14. 14.
    Which of the following represents the balanced chemical equation for the reaction of hot and concentrated nitric acid on copper?

    1. A. Cu + 2HNO₃ (hot & conc.) → Cu(NO₃)₂ + H₂O + NO₂
    2. B. Cu + 4HNO₃ (hot & conc.) → Cu(NO₃)₂ + 2H₂O + 2NO₂
    3. C. 3Cu + 8HNO₃ (hot & conc.) → 3Cu(NO₃)₂ + 4H₂O + 2NO
    4. D. Cu + HNO₃ (hot & conc.) → CuNO₃ + H₂O + NO
    [1]
15. 15.
    Which of the following represents the balanced chemical equation for the reaction of dilute nitric acid with copper?

    1. A. Cu + 4HNO₃ → Cu(NO₃)₂ + 2H₂O + 2NO₂
    2. B. 3Cu + 8HNO₃ → 3Cu(NO₃)₂ + 4H₂O + 2NO
    3. C. 2Cu + 6HNO₃ → 2Cu(NO₃)₂ + 3H₂O + NO + NO₂
    4. D. Cu + HNO₃ → CuNO₃ + H₂O + NO
    [1]
16. 16.
    Which nitrate leaves no residue behind when heated?

    1. A. Sodium nitrate
    2. B. Ammonium nitrate
    3. C. Copper nitrate
    4. D. Lead nitrate
    [1]
17. 17.
    How can nitrous oxide be obtained from sodium nitrate?

    1. A. By heating sodium nitrate with ammonium sulfate
    2. B. By reacting sodium nitrate with hydrochloric acid
    3. C. By heating sodium nitrate alone
    4. D. By reacting sodium nitrate with copper
    [1]
18. 18.
    How many lone pair(s) involved in the formation of coordinate bond(s) in nitric acid?

    1. A. 4
    2. B. 2
    3. C. 3
    4. D. 1
    [1]
19. 19.
    Which of the following percentages correctly represents the concentration of nitric acid by weight in constant boiling nitric acid?

    1. A. 50% HNO₃ by weight
    2. B. 68% HNO₃ by weight
    3. C. 80% HNO₃ by weight
    4. D. 98% HNO₃ by weight
    [1]
20. 20.
    Which balanced equation shows the reaction of concentrated nitric acid with sulphur?

    1. A. S + 4HNO₃ → H₂SO₄ + 4NO₂ + H₂O
    2. B. S + 6HNO₃ → H₂SO₄ + 6NO₂ + 2H₂O
    3. C. S + 2HNO₃ → H₂SO₄ + 2NO↑
    4. D. S + HNO₃ → H₂SO₃ + NO₂↑
    [1]