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2 marksRedox Reactions

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

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

Use the appropriate half equations (from those above) to write a balanced equation to show the reaction between hydrogen peroxide and chloric (I) (hypochlorous) acid.

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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)(ii)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…[6 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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