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Answer Question 1(a) - Name the substances in the Solvay process.

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  1. Answer Question 1(a) - Name the substances in the Solvay process.

    • a)
      • (i) Solution A: Brine (concentrated sodium chloride solution)
      • (ii) Substance B: Ammoniated brine
      • (iii) Solid S: Sodium hydrogen carbonate (NaHCO3\text{NaHCO}_3)

  2. Answer Question 1(b) - Write equations for reactions in Chamber 2 and Chamber 3.

    • b)
      • (i) Chamber 2: Recovery of ammonia. 2NH4Cl(aq)+Ca(OH)2(aq)→CaCl2(aq)+2NH3(g)+2H2O(l)\text{2NH}_4\text{Cl}(\text{aq}) + \text{Ca(OH)}_2(\text{aq}) \to \text{CaCl}_2(\text{aq}) + \text{2NH}_3(\text{g}) + \text{2H}_2\text{O}(\text{l})
      • (ii) Chamber 3: Formation of sodium hydrogen carbonate. NaCl(aq)+NH3(g)+H2O(l)+CO2(g)→NaHCO3(s)+NH4Cl(aq)\text{NaCl}(\text{aq}) + \text{NH}_3(\text{g}) + \text{H}_2\text{O}(\text{l}) + \text{CO}_2(\text{g}) \to \text{NaHCO}_3(\text{s}) + \text{NH}_4\text{Cl}(\text{aq})

  3. Answer Question 1(c) - Identify processes (i) and (ii).

    • c)
      • (i) Process (I): Carbonation or Precipitation (formation of sodium hydrogen carbonate)
      • (ii) Process (II): Thermal decomposition or Calcination (conversion of sodium hydrogen carbonate to sodium carbonate)

  4. Answer Question 1(d) - Explain how carbon(IV) oxide is obtained.

    • d) Carbon(IV) oxide (CO2\text{CO}_2) is obtained by the thermal decomposition of limestone (CaCO3\text{CaCO}_3) in a lime kiln: CaCO3(s)→CaO(s)+CO2(g)\text{CaCO}_3(\text{s}) \to \text{CaO}(\text{s}) + \text{CO}_2(\text{g}) It can also be obtained by burning coke (carbon): C(s)+O2(g)→CO2(g)\text{C}(\text{s}) + \text{O}_2(\text{g}) \to \text{CO}_2(\text{g})

  5. Answer Question 1(e) - Give two reasons for the efficiency of the Solvay process.

    • e)
      • Most of the raw materials, such as ammonia and carbon dioxide, are recycled within the process.
      • The process produces sodium carbonate, a valuable chemical, with calcium chloride as the only major by-product, which has some industrial uses.

  6. Answer Question 1(f) - Give two uses of sodium carbonate.

    • f)
      • Used in the manufacture of glass.
      • Used for softening hard water.
      • Used in the manufacture of detergents and soaps.
      • Used in the paper industry.

  7. Answer Question 2(a) - What happens to the brightness of the bulb during electrolysis?

    • a) The brightness of the bulb decreases. As electrolysis proceeds, the concentration of mobile ions (Cu2+\text{Cu}^{2+} and Cl−\text{Cl}^-) in the molten copper(II) chloride decreases as they are discharged at the electrodes. Fewer ions mean lower electrical conductivity, causing the bulb to dim.

  8. Answer Question 2(b) - Name suitable electrodes.

    • b) A suitable pair of electrodes is graphite or platinum.

  9. Answer Question 2(c) - Identify the anode and cathode.

    • c)
      • Anode: The electrode connected to the positive terminal of the battery (left electrode in the diagram).
      • Cathode: The electrode connected to the negative terminal of the battery (right electrode in the diagram).

  10. Answer Question 2(d) - Write the half equation for the reaction at the anode.

    • d) At the anode, chloride ions are oxidized to chlorine gas. 2Cl−(l)→Cl2(g)+2e−\text{2Cl}^-(\text{l}) \to \text{Cl}_2(\text{g}) + \text{2e}^-

  11. Answer Question 2(e) - State and explain one precaution.

    • e)
      • Wear safety goggles: Molten salts are very hot and corrosive; goggles protect eyes from splashes.
      • Carry out in a fume cupboard: Chlorine gas is produced at the anode, which is toxic and should not be inhaled.

  12. Answer Question 3 - Explain the reactions of carbon(IV) oxide with sodium hydroxide and calcium hydroxide.

    • When carbon(IV) oxide (CO2\text{CO}_2) is bubbled through sodium hydroxide (NaOH\text{NaOH}), it reacts to form sodium carbonate (Na2CO3\text{Na}_2\text{CO}_3) and water. Both products are soluble in water, so no visible change is observed. 2NaOH(aq)+CO2(g)→Na2CO3(aq)+H2O(l)\text{2NaOH}(\text{aq}) + \text{CO}_2(\text{g}) \to \text{Na}_2\text{CO}_3(\text{aq}) + \text{H}_2\text{O}(\text{l})
    • When CO2\text{CO}_2 is bubbled through calcium hydroxide (Ca(OH)2\text{Ca(OH)}_2, limewater), it reacts to form calcium carbonate (CaCO3\text{CaCO}_3) and water. Calcium carbonate is insoluble in water, which causes a white precipitate to form, making the solution cloudy. Ca(OH)2(aq)+CO2(g)→CaCO3(s)+H2O(l)\text{Ca(OH)}_2(\text{aq}) + \text{CO}_2(\text{g}) \to \text{CaCO}_3(\text{s}) + \text{H}_2\text{O}(\text{l})
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