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6 marksRedox Reactions

CAPE Chemistry Unit 1 · 2006 · Paper 2 · Question 5(b)(ii)

Hydrogen peroxide, H2O2, can act as both an oxidising agent and a reducing agent, and chloric (I) acid (HOCl) can act as an oxidizing agent. O2 + 2H+ + 2e- → H2O2; 1/2 H2O2 + H+ + e- → H2O; HOCl + H+ + e- → 1/2 Cl2 + H2O

By making reference to the change in oxidation numbers of the elements in both the hydrogen peroxide AND the chloric (I) acid, determine which reactant is reduced and which is oxidised.

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Other parts of this question

  1. 5(a)(i)Explain EACH of the terms 'oxidation' and 'reduction', in terms of loss and or gain of electrons[2 marks]
  2. 5(a)(ii)Explain EACH of the terms 'oxidation' and 'reduction', in terms of change in oxidation number.[2 marks]
  3. 5(b)(i)Use the appropriate half equations (from those above) to write a balanced equation to show the reaction between hydrogen peroxide and chloric (I)…[2 marks]
  4. 5(c)(i)State what type of chemical reaction occurs and write an ionic equation for the reaction.[3 marks]
  5. 5(c)(ii)Which element has the greater reducing ability? Explain your answer, using a suitable half equation.[4 marks]
  6. 5(c)(iii)Tin shows no reaction with solutions of EITHER iron or nickel salts. Place the elements, tin, iron and nickel in order of INCREASING reducing ability.[1 mark]

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