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CAPE Chemistry Unit 1 · 2007 · Paper 2

45 questions and parts from this paper. Open one to see it in full, then practise it on Quelpr and get it marked against the mark scheme.

Practise this paper
  1. 1(a)(i)2 marksDefine the term mole.
  2. 1(a)(ii)1 markDefine the term molar mass.
  3. 1(a)(iii)1 markState the units of molar mass.
  4. 1(b)(i)2 marksCalculate the number of moles of phosphorous (V) acid that reacted.
  5. 1(b)(ii)1 markCalculate the number of moles of sodium hydroxide that reacted.
  6. 1(b)(iii)1 markCalculate the number of moles of sodium hydroxide that reacted with 1 mole of the acid.
  7. 1(c)1 markDerive the equation for the reaction that occurred in Part (b) above.
  8. 1(d)(i)1 markState Avogadro's Law.
  9. 1(e)5 marksOutline the experimental steps involved in carrying out the reaction described in (b) on page 2.
  10. 2(a)(i)5 marksOutline the experimental steps he has to follow to obtain a reading of approximately 1.10 V on his voltmeter.
  11. 2(a)(ii)2 marksWrite the ionic half equation for the reaction occurring at EACH of the electrodes.
  12. 2(a)(iii)1 markIdentify the anode and the cathode.
  13. 2(a)(iv)1 markExplain the direction of electron flow.
  14. 2(a)(v)1 markWrite the cell diagram.
  15. 2(a)(vi)1 markWrite the equation to represent the cell reaction.
  16. 2(b)2 marksUse the Eº value for each electrode (in the data booklet) to determine the Eºcell.
  17. 2(c)2 marksSuggest TWO changes which could be made to the cell in (a) to cause the cell potential to be greater than 1.10V.
  18. 3(a)3 marksState THREE OTHER characteristic properties of transition elements.
  19. 3(b)(i)2 marksWhat are the colours of aqueous Co²⁺?
  20. 3(b)(ii)2 marksWhat are the colours of aqueous Mn²⁺?
  21. 3(c)1 markIf aqueous Co²⁺ is heated to dryness, what colour is observed?
  22. 3(d)1 markExplain what is meant by the term 'ligand'.
  23. 3(e)(i)2 marksWrite the formula of the species formed, and describe what occurs when ammonia solution is added to aqueous copper (II) sulphate (IV).
  24. 3(e)(ii)2 marksWrite the formula of the species formed, and describe what occurs when an excess of ammonia solution is added to (e)(i) on page 6.
  25. 3(f)4 marksUse the ligand exchange theory to account for this occurrence.
  26. 4(a)1 markState Hess's Law.
  27. 4(b)(i)2 marksDefine standard enthalpy change of formation.
  28. 4(b)(ii)2 marksDefine lattice energy.
  29. 4(c)(i)6 marksWhich enthalpy values correspond to EACH of the stages I, III and IV in the cycle above?
  30. 4(c)(ii)6 marksCalculate the lattice energy of MX(s).
  31. 4(d)4 marksAccount for the difference in the lattice energy for MgCl₂(s) and NaCl(s).
  32. 4(e)2 marksExplain why the molar enthalpy changes for the following reactions have identical values: HCl (aq) + NaOH (aq) → NaCl (aq) + H₂O(l); H₂SO₄ (aq) + 2KOH (aq) → K₂SO₄ (aq) + 2H₂O(l).
  33. 5(a)3 marksAccount for the observations in the statement below: Pure water is a poor conductor of electricity whereas water in the presence of a trace of H⁺(aq) is a good conductor.
  34. 5(b)(i)3 marksDerive the relationship for the ionic product of water, Kᵥ.
  35. 5(b)(ii)3 marksState how the value of Kᵥ varies with temperature.
  36. 5(c)(i)4 marksCalculate the pH of EACH of the solutions A, B and C, given that their concentrations are as shown in the table below.
  37. 5(c)(ii)4 marksPlace the solutions A, B and C in 5 (c) (i) on a pH scale relative to the pH of pure water.
  38. 5(d)(i)5 marksDefine the term 'buffer solution'.
  39. 5(d)(ii)5 marksWhich of the solutions, X or Y, would you use with the sodium hydroxide to prepare a buffer solution? Justify your answer.
  40. 5(d)(iii)5 marksExplain how small additions of H⁺ and OH⁻ ions are accommodated in the buffer solution prepared in 5 (d) (ii).
  41. 6(a)(i)5 marksCalculate the oxidation number of the first mentioned element in EACH of the following compounds, and explain the variation in these oxidation numbers: MgCl₂, [Al(OH)₄]⁻, SiF₆²⁻, PO₃³⁻.
  42. 6(b)(i)5 marksExplain the terms 'atomic radius' and 'ionic radius'.
  43. 6(b)(ii)5 marksAccount for the variation in atomic and ionic radii of the elements in Group II.
  44. 6(b)(iii)5 marksAccount for the variation in the solubility of the sulphate (VI) of the Group II elements.
  45. 6(c)5 marksExplain the variation in the acid/base character of the oxides of oxidation state +2 of the elements of Group IV.

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