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CAPE Chemistry Unit 1 · 2008 · Paper 2

36 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.

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  1. 1(a)(i)2 marksDefine the term 'standard enthalpy of formation', ΔHᶠθ.
  2. 1(a)(ii)2 marksThe enthalpy of formation of both carbon monoxide and aluminium oxide cannot be determined directly by experimental means. Suggest ONE reason in EACH case for the above observation. CO: Al₂O₃:
  3. 1(b)(i)3 marksWrite the enthalpy change represented by ΔH₁, ΔH₂ and ΔH₃ in Figure 1. ΔH₁ : ΔH₂ : ΔH₃ :
  4. 1(b)(ii)3 marksCalculate the enthalpy of solution for KBr, given the following information. ΔH₁ = + 672 kJ mol⁻¹ ΔH₂ = - 656 kJ mol⁻¹
  5. 1(c)(i)2 marksWhat kind of bonding is present in halides of X?
  6. 1(c)(ii)1 markWhat kind of bonding is present in halides of Y?
  7. 1(d)(i)3 marksIdentify THREE errors in the above method.
  8. 2(a)4 marksOn the grid provided on page 7, plot a graph of the concentration of butyl chloride, [C₄H₉Cl] on the y-axis against time in seconds, on the x-axis.
  9. 2(b)1 markUsing your graph, estimate the concentration of butyl chloride at t = 400 s.
  10. 2(c)(i)4 marksUsing suitable well-labelled diagrams, explain how EACH of the following affects reaction rates: Catalysts
  11. 2(c)(ii)4 marksUsing suitable well-labelled diagrams, explain how EACH of the following affects reaction rates: Temperature
  12. 2(d)2 marksName TWO industrial processes in which catalysts are used.
  13. 3(a)(i)5 marksInsert arrows in EACH of the boxes in Figure 2 to show the electronic configuration of the species.
  14. 3(a)(ii)a)3 marksExplain EACH of the following statements in terms of electronic configurations. Fe²⁺ ions are readily oxidized to Fe³⁺ ions.
  15. 3(a)(ii)b)1 markExplain EACH of the following statements in terms of electronic configurations. Mn²⁺ ions are NOT readily oxidized to Mn³⁺ ions.
  16. 3(a)(ii)c)1 markExplain EACH of the following statements in terms of electronic configurations. Zn is NOT considered to be a transition element.
  17. 3(b)(i)4 marksComplete the table below by writing the colour of the species labelled A, B, C and D.
  18. 3(b)(ii)1 markState the reagent used for the conversion in Reaction 1 (D → B).
  19. 3(c)2 marksExplain how an aqueous solution of iron(II) sulphate functions as an antidote for cyanide poisoning.
  20. 4(a)3 marksList THREE assumptions made about gas molecules in the kinetic theory.
  21. 4(b)(i)2 marksState the TWO conditions under which the ideal gas equation adequately describes the behaviour of gases.
  22. 4(b)(ii)3 marksCarefully explain the deviations produced by real gases.
  23. 4(c)1 markSketch a graph of volume (V) against the inverse of pressure (1/P) for a constant number of moles of an ideal gas at constant temperature.
  24. 4(d)(i)4 marksAn organic compound, Y, contains carbon, hydrogen and oxygen only. When vapourised at 101 kPa and 373 K, 1.00 g of Y occupies a volume of 667 cm³. Calculate the mass in grams of 1 mole of Y. (Gas constant, R = 8.314 J…
  25. 4(d)(ii)2 marksOn combustion in excess oxygen, 1 mole of Y produces carbon dioxide and water in the mole ratio 2:3. Deduce the formula of Y.
  26. 5(a)(i)2 marksWith reference to the Bronsted-Lowry theory, explain EACH of the following: Weak acid
  27. 5(a)(ii)1 markWith reference to the Bronsted-Lowry theory, explain EACH of the following: Strong acid
  28. 5(b)2 marksDescribe the significance of pH (- log [H⁺]) and Kₐ (acid dissociation constant) values.
  29. 5(c)4 marksCalculate the pH of the HC₃H₅O₃ / C₃H₅O₃⁻ buffer solution.
  30. 5(d)6 marksWith the aid of balanced equations, explain how the HC₃H₅O₃ / C₃H₅O₃⁻ buffer works in maintaining its pH.
  31. 5(e)1 markWhen preparing a buffer solution of a specific pH, state ONE consideration to be taken into account in selecting a suitable weak acid.
  32. 6(a)(i)4 marksState and account for the trend in the values of the atomic radii across the period from Na to Cl.
  33. 6(a)(ii)5 marksThe trend in the melting points of the elements in Table 3 is related to structure and bonding. Describe the trend in the structure of the elements, and the trend in the bonding of the elements in Table 3.
  34. 6(b)(i)2 marksCompare the reaction of the Group II elements, Be and Ca, with water.
  35. 6(b)(ii)3 marksDescribe what happens when barium is treated with water and write the equation for the reaction.
  36. 6(c)1 markState ONE use of calcium carbonate.

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