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The Mole Concept · CAPE Chemistry Unit 1

83 past-paper questions on The Mole Concept, part of Fundamentals in Chemistry, from every CAPE Chemistry Unit 1 paper on Quelpr.

Practise The Mole Concept
  1. 1(a)(i)1 mark· CAPE Chemistry Unit 1 · 2005 · Paper 1Define empirical formula.
  2. 1(a)(ii)1 mark· CAPE Chemistry Unit 1 · 2005 · Paper 1Define molecular formula.
  3. 1(b)2 marks· CAPE Chemistry Unit 1 · 2005 · Paper 1Give an example of a compound for which the molecular formula is different from the empirical formula, writing the respective formulae.
  4. 1(c)6 marks· CAPE Chemistry Unit 1 · 2005 · Paper 1Use the data provided to determine the molecular formula of X.
  5. 4(c)(i)2 marks· CAPE Chemistry Unit 1 · 2005 · Paper 1Write the chemical equation for this reaction.
  6. 3(a)1 mark· CAPE Chemistry Unit 1 · 2005 · Paper 2Suggest a suitable titrant reagent for estimating salicylic acid.
  7. 3(b)6 marks· CAPE Chemistry Unit 1 · 2005 · Paper 2Describe the procedure for preparing the standard titrant solution to estimate the salicylic acid in each tablet.
  8. 5(c)(i)2 marks· CAPE Chemistry Unit 1 · 2005 · Paper 2Write a balanced equation for the reaction of hydrazine with chlorine to produce hydrogen chloride and nitrogen.
  9. 5(c)(ii)2 marks· CAPE Chemistry Unit 1 · 2005 · Paper 2Given ΔH = -420 kJ mol^-1 for the reaction in (c)(i), calculate the enthalpy change when 12.7 g of hydrazine reacts completely.
  10. 7(c)(i)6 marks· CAPE Chemistry Unit 1 · 2005 · Paper 2Calculate the empirical and molecular formulae of compounds A and B.
  11. 8(a)(i)4 marks· CAPE Chemistry Unit 1 · 2005 · Paper 2Calculate the mean and standard deviation of the calcium carbonate hardness values, showing the relevant formulae.
  12. 8(a)(ii)1 mark· CAPE Chemistry Unit 1 · 2005 · Paper 2State what the standard deviation indicates regarding the variability in the water hardness values.
  13. 8(a)(iii)1 mark· CAPE Chemistry Unit 1 · 2005 · Paper 2State how the reliability of the hardness data collected from the sites can be improved.
  14. 8(b)(i)2 marks· CAPE Chemistry Unit 1 · 2005 · Paper 2Compare the two results with regard to precision and suggest an explanation for the discrepancy.
  15. 8(b)(ii)1 mark· CAPE Chemistry Unit 1 · 2005 · Paper 2Identify the additional information needed to evaluate the accuracy of the result obtained at this site.
  16. 8(c)5 marks· CAPE Chemistry Unit 1 · 2005 · Paper 2Discuss the importance of choosing appropriate volumetric apparatus when titrating 100 cm^3 water samples with EDTA using Eriochrome Black T indicator.
  17. 8(d)6 marks· CAPE Chemistry Unit 1 · 2005 · Paper 2Describe the experimental procedure for calibrating and determining the accurate volume delivered by a volumetric pipette.
  18. 9(b)(iv)3 marks· CAPE Chemistry Unit 1 · 2005 · Paper 2Describe the procedure for constructing a calibration curve for this spectrophotometric analysis.
  19. 9(c)(i)3 marks· CAPE Chemistry Unit 1 · 2005 · Paper 2Calculate the molar concentration in mol dm^-3 of the standard iron(II) solution.
  20. 9(c)(iii)1 mark· CAPE Chemistry Unit 1 · 2005 · Paper 2Calculate the concentration of iron(II) in the unknown sample in mol dm^-3.
  21. 1(d)(i)1 mark· CAPE Chemistry Unit 1 · 2021 · Paper 2Define the term 'Molar mass'.
  22. 1(d)(ii)1 mark· CAPE Chemistry Unit 1 · 2021 · Paper 2Define the term 'Mole'.
  23. 1(e)(i)2 marks· CAPE Chemistry Unit 1 · 2021 · Paper 2Calculate the original number of moles of NaOH in 100 cm³ of 0.500 mol dm⁻³ aqueous sodium hydroxide.
  24. 1(e)(ii)2 marks· CAPE Chemistry Unit 1 · 2021 · Paper 2Calculate the number of moles of HCl in 27.3 cm³ of 0.600 mol dm⁻³ hydrochloric acid.
  25. 1(e)(iii)1 mark· CAPE Chemistry Unit 1 · 2021 · Paper 2Deduce the number of moles of unreacted NaOH neutralized by the hydrochloric acid.
  26. 1(e)(iv)2 marks· CAPE Chemistry Unit 1 · 2021 · Paper 2Calculate the number of moles of NaOH which reacted with the ammonium sulfate.
  27. 1(e)(v)3 marks· CAPE Chemistry Unit 1 · 2021 · Paper 2Use your answer in (e)(iv) to calculate the number of moles and the mass of ammonium sulfate in the sample.
  28. 1(e)(vi)1 mark· CAPE Chemistry Unit 1 · 2021 · Paper 2Write the ionic equation, including physical states, for the reaction between ammonium sulfate and aqueous sodium hydroxide.
  29. 1(f)(i)1 mark· CAPE Chemistry Unit 1 · May/June 2024 · Paper 2Calculate the number of moles of potassium manganate(VII) used in the titration.
  30. 1(f)(ii)1 mark· CAPE Chemistry Unit 1 · May/June 2024 · Paper 2Using the equation 2 MnO4^-(aq) + 5 NO2^-(aq) + 6 H^+(aq) -> 2 Mn^2+(aq) + 5 NO3^-(aq) + 3 H2O(l), deduce the number of moles of KNO2 present in the titre volume.
  31. 1(f)(iii)1 mark· CAPE Chemistry Unit 1 · May/June 2024 · Paper 2Calculate the number of moles of KNO2 that was present in the residue from the decomposition of Sample A.
  32. 1(f)(iv)2 marks· CAPE Chemistry Unit 1 · May/June 2024 · Paper 2Calculate the mass of KNO2 present in the residue from Sample A.
  33. 1(f)(v)3 marks· CAPE Chemistry Unit 1 · May/June 2024 · Paper 2Using the equation for the decomposition of KNO3, determine the mass of KNO2 formed if 6.20 g KNO3 were completely decomposed.
  34. 1(f)(vi)2 marks· CAPE Chemistry Unit 1 · May/June 2024 · Paper 2Using the results from (f)(iv) and (v), calculate the percentage of KNO2 formed.
  35. 1(f)(vii)5 marks· CAPE Chemistry Unit 1 · May/June 2024 · Paper 2Outline the experimental steps taken in the laboratory to prepare the 0.02 mol dm^-3 potassium manganate(VII) solution used for this titration.
  36. 3(d)(i)2 marks· CAPE Chemistry Unit 1 · May/June 2024 · Paper 2Describe the changes which occur at the end point of the titration.
  37. 1(c)(i)1 mark· CAPE Chemistry Unit 1 · May/June 2026 · Paper 2Define mole of a substance.
  38. 1(c)(ii)1 mark· CAPE Chemistry Unit 1 · May/June 2026 · Paper 2Define molar mass.
  39. 1(d)(i)4 marks· CAPE Chemistry Unit 1 · May/June 2026 · Paper 2Calculate the empirical formula of the product of the reaction between 10.0 g of lithium and excess oxygen that gave 21.5 g of lithium oxide.
  40. 1(g)2 marks· CAPE Chemistry Unit 1 · May/June 2026 · Paper 2Calculate the volume of 4.10 g of Ar at STP. [1 mole of gas occupies 22.4 dm³ at STP.]
  41. 1(h)5 marks· CAPE Chemistry Unit 1 · May/June 2026 · Paper 2Outline the experimental steps that can be used to determine the volume of a 0.1152 M solution of H2SO4 which would be required to neutralize 25.00 mL of a 0.1913 M KOH solution.
  42. 1(a)(i)2 marks· Chemistry · Unit 1 Q1 1(a)(i)Define the term mole.
  43. 1(a)(i)1 mark· Chemistry · Unit 1 Q1 1(a)(i)Calculate the mass of carbon in 3.52 g of carbon dioxide
  44. 1(a)(i)2 marks· Chemistry · Unit 1 Q1 1(a)(i)Define the term 'mole'.
  45. 1(a)(ii)2 marks· Chemistry · Unit 1 Q1 1(a)(ii)Define the term 'molar mass' (include the units).
  46. 1(a)(ii)1 mark· Chemistry · Unit 1 Q1 1(a)(ii)Calculate the mass of hydrogen in 1.62 g of water.
  47. 1(a)(ii)1 mark· Chemistry · Unit 1 Q1 1(a)(ii)Define the term molar mass.
  48. 1(a)(iii)1 mark· Chemistry · Unit 1 Q1 1(a)(iii)State the units of molar mass.
  49. 1(b)2 marks· Chemistry · Unit 1 Q1 1(b)Use the answers obtained in (a) (i) and (a) (ii) to calculate the empirical formula of A.
  50. 1(b)(i)2 marks· Chemistry · Unit 1 Q1 1(b)(i)Write a balanced chemical equation for the reaction between calcium oxide and ammonium chloride.
  51. 1(b)(i)2 marks· Chemistry · Unit 1 Q1 1(b)(i)Write a balanced equation to represent the reaction above.
  52. 1(b)(i)2 marks· Chemistry · Unit 1 Q1 1(b)(i)Calculate the number of moles of phosphorous (V) acid that reacted.
  53. 1(b)(i)a)2 marks· Chemistry · Unit 1 Q1 1(b)(i)a)Calculate the number of moles of M₂CO₃.
  54. 1(b)(i)b)2 marks· Chemistry · Unit 1 Q1 1(b)(i)b)Calculate the relative molecular mass of M₂CO₃.
  55. 1(b)(ii)2 marks· Chemistry · Unit 1 Q1 1(b)(ii)Calculate the mass of ammonium chloride needed to produce 1 dm³ of ammonia at RTP (room temperature and pressure). (Molar volume = 24 dm³ at RTP)
  56. 1(b)(ii)2 marks· Chemistry · Unit 1 Q1 1(b)(ii)Deduce the identity of M.
  57. 1(b)(ii)1 mark· Chemistry · Unit 1 Q1 1(b)(ii)Calculate the number of moles of sodium hydroxide that reacted.
  58. 1(b)(iii)1 mark· Chemistry · Unit 1 Q1 1(b)(iii)Calculate the number of moles of sodium hydroxide that reacted with 1 mole of the acid.
  59. 1(c)2 marks· Chemistry · Unit 1 Q1 1(c)The molar mass of A is 114 g mol-¹. Calculate its molecular formula.
  60. 1(c)5 marks· Chemistry · Unit 1 Q1 1(c)Outline the experimental steps required to carry out the reaction described in (b) on page 2.
  61. 1(c)1 mark· Chemistry · Unit 1 Q1 1(c)Derive the equation for the reaction that occurred in Part (b) above.
  62. 1(c)5 marks· Chemistry · Unit 1 Q1 1(c)Outline the experimental steps (including calculations) required to obtain an accurate value.
  63. 1(d)5 marks· Chemistry · Unit 1 Q1 1(d)Describe an experiment that would determine the concentration of the aqueous ammonia.
  64. 1(d)(i)1 mark· Chemistry · Unit 1 Q1 1(d)(i)State Avogadro's Law.
  65. 1(e)5 marks· Chemistry · Unit 1 Q1 1(e)Outline the experimental steps involved in carrying out the reaction described in (b) on page 2.
  66. 2(c)5 marks· Chemistry · Unit 1 Q2 2(c)A student was given a particular brand of club soda (carbonated beverage) to determine the carbonic acid content. Outline the experimental steps required for the investigation if the student is given 200 cm³ of 0.100…
  67. 2(c)2 marks· Chemistry · Unit 1 Q2 2(c)Ant stings can be treated with baking soda, NaHCO₃. Suggest, with the aid of an equation, how baking soda helps to relieve the effect of the sting.
  68. 31 mark· Chemistry · Unit 1 Q3 3The volume of gas produced when 1.2 g of Mg reacts with HCl at r.t.p is
  69. 4(a)(iii)2 marks· Chemistry · Unit 1 Q4 4(a)(iii)Given that the mass of gas produced in the air bag is 90.0 g, use the answer from (a)(ii) to calculate the molar mass of the gas and suggest its identity.
  70. 4(a)(iv)2 marks· Chemistry · Unit 1 Q4 4(a)(iv)Write the equation for the decomposition of NaN₃.
  71. 4(c)6 marks· Chemistry · Unit 1 Q4 4(c)Calculate the molar ratio of Cr₂O₇²⁻ to I⁻ and hence derive the ionic equation for the reaction which has occurred. Molar ratio: Ionic equation:
  72. 4(d)(ii)2 marks· Chemistry · Unit 1 Q4 4(d)(ii)On combustion in excess oxygen, 1 mole of Y produces carbon dioxide and water in the mole ratio 2:3. Deduce the formula of Y.
  73. 71 mark· Chemistry · Unit 1 Q7 7If 10 cm³ of nitrogen reacts with 30 cm³ of hydrogen at STP, what volume of NH₃ is produced?
  74. 7(a)3 marks· Chemistry · Unit 1 Q7 7(a)State THREE characteristics of ethanedioic acid that make it a suitable primary standard.
  75. 7(b)2 marks· Chemistry · Unit 1 Q7 7(b)In preparing the solution of ethanedioic for titration against the permanganate, two pieces of laboratory equipment with a high degree of accuracy are required. Name these TWO pieces of equipment.
  76. 7(c)(i)1 mark· Chemistry · Unit 1 Q7 7(c)(i)Calculate the number of moles MnO₄⁻ used.
  77. 7(c)(ii)1 mark· Chemistry · Unit 1 Q7 7(c)(ii)Calculate the number of moles Fe²⁺ in the 25.0 cm³ of aqueous M.
  78. 7(c)(iii)1 mark· Chemistry · Unit 1 Q7 7(c)(iii)Calculate the number of moles Fe²⁺ in 1.0 dm³ of M (aq).
  79. 7(c)(iv)1 mark· Chemistry · Unit 1 Q7 7(c)(iv)Calculate the mass of Fe²⁺ in 1 dm³ of M (aq).
  80. 7(c)(v)1 mark· Chemistry · Unit 1 Q7 7(c)(v)Calculate the % Fe²⁺ in the compound [The mass concentration of M is 40.90 g dm⁻³].
  81. 91 mark· Chemistry · Unit 1 Q9 9Which of the following equations represents the BALANCED equation for the titration?
  82. 91 mark· Chemistry · Unit 1 Q9 9For 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?
  83. 141 mark· Chemistry · Unit 1 Q14 14The simplest formula for a compound that contains 50% S and 50% O by mass is

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