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3 marksMole Concept

CSEC Chemistry · January 2013 · Paper 2 · Question 1(c)(iii)

Calculate the maximum volume of hydrogen gas, at room temperature and pressure (RTP), that would be produced when 1.0 gram of zinc metal reacts with excess dilute hydrochloric acid. (1 mole of a gas occupies 24 dm³ at RTP, RAM Zn = 65).

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Other parts of this question

  1. 1(a)Define the term 'rate of reaction'.[1 mark]
  2. 1(b)Read, from the diagrams in Figure 1 and record in Table 1, the volume of the gas produced for EACH experiment. Experiment 1 has been done for you.[3 marks]
  3. 1(c)(i)Write a balanced chemical equation, including state symbols, for the reaction between zinc metal and dilute hydrochloric acid.[2 marks]
  4. 1(c)(ii)Identify the oxidizing agent in the equation in (c) (i), and give a reason, in terms of oxidation numbers, why the agent is oxidizing.[2 marks]
  5. 1(d)Compare the volume of gas produced in Experiments 2, 3 and 4, to the volume produced in Experiment 1, and give an explanation in EACH case.[6 marks]
  6. 1(e)(i)With which granules, zinc or magnesium, will Experiment 1 be more reactive?[1 mark]
  7. 1(e)(ii)Using the same axes in Figure 2, sketch the curve when magnesium granules are used in Experiment 1.[1 mark]
  8. 1(f)(i)An outline of the steps for a procedure you can use[4 marks]
  9. 1(f)(ii)A list of the main observations that would be expected at EACH stage of the experiment[2 marks]

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