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CAPE Chemistry Unit 1 · 2015 · Paper 1

43 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. 11 markWhich of the following statements is NOT a part of Dalton's atomic theory?
  2. 21 markThe intermolecular forces present in ice are
  3. 31 markWhich of the following pairs of elements combine to produce naturally occurring compounds with formulae type XY?
  4. 41 markWhich of the following diagrams represents a pi (π) bond?
  5. 51 markWhen an atom of 238 U is bombarded with a neutron, how many fundamental particles (protons - p, neutrons - n and electrons - e) does an atom of the PRODUCT contain?
  6. 61 markBased on the data in the table above, the relative isotopic mass of lead is
  7. 71 markIf 10 cm³ of nitrogen reacts with 30 cm³ of hydrogen at STP, what volume of NH₃ is produced?
  8. 81 markFrom the data above, it can be deduced that X is a
  9. 91 markFor complete reaction, 0.25 g of a monobasic acid requires 10 cm³ of 0.2 mol dm⁻³ sodium hydroxide. What is the relative molecular mass of the acid?
  10. 101 markWhich of the following processes represents an oxidation?
  11. 111 markWhich of the following groups of solids contains substances that ALL have giant structures?
  12. 121 markWhat is the activation energy of the REVERSE reaction?
  13. 131 markA gas in a syringe occupies a volume of 50 cm³ and has a pressure of 0.49 atmospheres. What is the pressure of the gas if the plunger of the syringe is pushed in, reducing the volume of the gas to 20 cm³? (1 atmosphere…
  14. 141 markThe simplest formula for a compound that contains 50% S and 50% O by mass is
  15. 151 markA student was asked to carry out an experiment to investigate the properties of ionic and covalent compounds. Which of the following experiments should the student use?
  16. 161 markWhat is the effect on a chemical reaction of introducing a catalyst in it?
  17. 171 markThe rate law for a given reaction is Rate = k[A]² [B]. What are the units for k?
  18. 181 markIn a standard hydrogen half-cell, a platinum electrode is used to
  19. 201 markThe reaction 2AB(g) → A₂(g) + B₂(g) has the rate law, Rate = k [AB]. If the half-life is 253 s, then the value of the velocity constant (k) at the temperature of the reaction is
  20. 211 markWhich of the acids in the table below is the WEAKEST?
  21. 221 markThe value of Kₚ for the equilibrium reaction H₂(g) + I₂(g) ⇌ 2HI(g) at 444 °C and 1 atm pressure is 50. What is the value of Kₚ if the pressure is changed to 2 atm and the temperature remains the same?
  22. 231 markEquilibrium is established in the reaction X(aq) + Y(aq) ⇌ Z(aq). If the equilibrium concentrations are [X] = 0.2 mol dm⁻³, [Y] = 0.3 mol dm⁻³ and [Z] = 0.6 mol dm⁻³, which of the following values is correct for the…
  23. 241 markWhich of the following graphs represents the order of reaction with respect to propanone?
  24. 251 markWhich metal sulfate would precipitate out of solution if equal volumes of 10⁻³ mol dm⁻³ solution containing the sulfate ion and the Group II metal are mixed?
  25. 261 markSilver chromate(VI), Ag₂CrO₄, is sparingly soluble in water. The units for the solubility product (Ksp) for silver chromate(VI) are
  26. 271 markBarium carbonate is more soluble in water than in aqueous sodium carbonate because
  27. 291 markMarine animals such as oysters and other shellfish rely on the slow precipitation of calcium carbonate to form their shells. Which of the following properties help this process?
  28. 301 markThe standard electrode potential of tin (Sn) is Sn²⁺(aq) + 2e⁻ → Sn(s), E° = -0.14 V. In which of the following equations is the metal UNABLE to reduce Sn²⁺?
  29. 311 markWhich of the following ions has the GREATEST polarizing power?
  30. 321 markWhich of the following properties increase on descending the Group II elements?
  31. 331 markSilicon carbide has a structure similar to that of diamond. What are the advantages derived from using silicon carbide ceramics when compared with steel?
  32. 341 markWhich of the following factors, BEST explain why barium carbonate, BaCO₃, is more stable than magnesium carbonate, MgCO₃, when heated?
  33. 351 markBased on its position in Group VII of the periodic table, astatine, at room temperature and pressure, is MOST likely a
  34. 361 markWhich of the following properties does NOT describe transition elements?
  35. 371 markWhich of the following elements in the third period has the SAME oxidation number in ALL of its known compounds?
  36. 381 markThe sharp increase from copper (Cu) to zinc (Zn) is caused by filled
  37. 391 markThe ionic equation for the formation of chromium hydroxide from chromium(III) sulfate and dilute NH₃(aq) is
  38. 401 markOn heating CaSO₄ strongly, it decomposes into CaO(s) and SO₂(g). CaCO₃ decomposes at a much lower temperature than CaSO₄. Which of the following factors BEST explains the greater thermal stability of CaSO₄?
  39. 411 markWhen concentrated H₂SO₄ is added to solid potassium iodide, the observations are white steamy fumes and
  40. 421 markWhich of the elements in the table can be classified as transition?
  41. 431 markElements can be classified by their response to externally applied magnetic fields as diamagnetic, paramagnetic and non-magnetic. Which of the following elements is considered to have a high degree of para-magnetism?
  42. 441 markWhich of the following compounds would produce the LOWEST pH when 0.5 mol of it is bubbled into 1 litre of water?
  43. 451 markWhat deduction can be made from the following reactions of iodine and chlorine with sodium thiosulfate? I₂(aq) + 2S₂O₃²⁻(aq) → 2I⁻(aq) + S₄O₆²⁻(aq) 4Cl₂(aq) + S₂O₃²⁻(aq) + 5H₂O(l) → 8Cl⁻(aq) + 2SO₄²⁻(aq) + 10H⁺(aq)

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