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Mole Concept · CSEC Chemistry

169 past-paper questions on Mole Concept, part of Principles of Chemistry, from every CSEC Chemistry paper on Quelpr.

Practise Mole Concept
  1. 1(a)1 mark· Chemistry Q1 1(a)Define the term 'standard solution'.
  2. 1(a)(i)4 marks· Chemistry Q1 1(a)(i)Use the information given in Figure 1 above to complete Table 1 below.
  3. 1(a)(i)9 marks· Chemistry Q1 1(a)(i)Complete Table 1 by recording the titration results obtained from the experiment in Figure 1.
  4. 1(a)(i)7 marks· Chemistry Q1 1(a)(i)In the space below construct Table 1 to record the titration results. You should include the initial and final burette volumes and the volume of solution X used.
  5. 1(a)(ii)1 mark· Chemistry Q1 1(a)(ii)Calculate the average volume of solution M used in the titration.
  6. 1(a)(ii)2 marks· Chemistry Q1 1(a)(ii)Write a balanced equation to show the decomposition of hydrogen peroxide by manganese(IV) oxide (MnO₂).
  7. 1(a)(ii)2 marks· Chemistry Q1 1(a)(ii)Write a balanced equation for the reaction between magnesium and hydrochloric acid.
  8. 1(a)(ii)1 mark· Chemistry Q1 1(a)(ii)Write a chemical equation for the reaction that occurs during the titration.
  9. 1(a)(ii)1 mark· Chemistry Q1 1(a)(ii)What is the volume of X to be used for calculation?
  10. 1(a)(iii)3 marks· Chemistry Q1 1(a)(iii)Calculate the mass of magnesium that will COMPLETELY react with 50 cm³ of 1.5 mol dm⁻³ HCl. (Relative atomic mass of Mg = 24; H = 1; Cl = 35.5)
  11. 1(a)(iii)1 mark· Chemistry Q1 1(a)(iii)The number of moles of hydrochloric acid used in the titration
  12. 1(a)(iii)2 marks· Chemistry Q1 1(a)(iii)Calculate the concentration of hydrochloric acid in solution M, in mol dm⁻³. (Relative atomic mass: H = 1; Cl = 35.5)
  13. 1(a)(iii)2 marks· Chemistry Q1 1(a)(iii)Write a balanced chemical equation to show the production of the anhydrous salt from the reaction between copper(II) oxide and dilute sulphuric acid.
  14. 1(a)(iii)1 mark· Chemistry Q1 1(a)(iii)Calculate the concentration of sulphuric acid in solution X in mol dm⁻³. (Relative atomic mass: H = 1; S = 32; O = 16)
  15. 1(a)(iii)2 marks· Chemistry Q1 1(a)(iii)Calculate the minimum mass of zinc required to completely react with 100 cm³ of 0.20 mol dm⁻³ copper(II) sulphate. Relative atomic mass of Zn = 65.
  16. 1(a)(iv)1 mark· Chemistry Q1 1(a)(iv)The number of moles of sodium hydroxide in 25.0 cm³ of the solution
  17. 1(a)(iv)4 marks· Chemistry Q1 1(a)(iv)Given that the relative formula mass of copper(II) oxide is 80, complete the data in Table 1 by calculating the mass of the salt formed in Experiment 3. (Relative Atomic Mass: Cu = 64; S = 32; O = 16; H = 1) Show your…
  18. 1(a)(iv)2 marks· Chemistry Q1 1(a)(iv)Write a balanced equation for the reaction between calcium carbonate and nitric acid.
  19. 1(a)(iv)1 mark· Chemistry Q1 1(a)(iv)Calculate the number of moles of hydrochloric acid used in the titration.
  20. 1(a)(iv)3 marks· Chemistry Q1 1(a)(iv)Describe how you would prepare 50 cm³ of different concentrations of hydrochloric acid from the solution of 1.5 mol dm⁻³ hydrochloric acid provided.
  21. 1(a)(iv)1 mark· Chemistry Q1 1(a)(iv)Calculate the number of moles of sulphuric acid used in the titration.
  22. 1(a)(iv)1 mark· Chemistry Q1 1(a)(iv)Use the information in (iii) above to explain why the different masses of zinc used in Experiments 4 and 5 give approximately the same change in temperature.
  23. 1(a)(ix)2 marks· Chemistry Q1 1(a)(ix)Calculate the number of moles of copper that would be formed.
  24. 1(a)(v)1 mark· Chemistry Q1 1(a)(v)Write a balanced equation for the reaction between the hydrochloric acid and sodium hydroxide solutions.
  25. 1(a)(v)3 marks· Chemistry Q1 1(a)(v)Using the data from Table 1 and the axes provided on page 4, plot a graph of the mass of anhydrous salt produced against the mass of copper(II) oxide used.
  26. 1(a)(v)3 marks· Chemistry Q1 1(a)(v)Calculate the volume of gas that can be obtained from reacting 1.8 g of calcium carbonate with dilute nitric acid at R.T.P. [1 mole of gas occupies 24 000 cm³ at R.T.P. R.A.M: C = 12; O = 16; Ca = 40]
  27. 1(a)(v)3 marks· Chemistry Q1 1(a)(v)Calculate the concentration (mol dm⁻³) of a saturated solution of potassium iodide at 30 °C. (RAM: K = 39, I = 127).
  28. 1(a)(v)2 marks· Chemistry Q1 1(a)(v)From the information given on page 3 in the introduction to this question, write a balanced chemical equation for the reaction between aqueous sodium thiosulphate and hydrochloric acid.
  29. 1(a)(v)2 marks· Chemistry Q1 1(a)(v)Write a balanced equation for the reaction between the sulphuric acid and sodium hydroxide solutions.
  30. 1(a)(v)2 marks· Chemistry Q1 1(a)(v)Write a balanced equation for the reaction of magnesium with hydrochloric acid.
  31. 1(a)(v)1 mark· Chemistry Q1 1(a)(v)The number of moles of sodium hydroxide in 250 cm³ of solution
  32. 1(a)(v)a)2 marks· Chemistry Q1 1(a)(v)a)Calculate EACH of the following: The number of moles of sulphuric acid in 20 cm³ of the sulphuric acid used
  33. 1(a)(v)b)2 marks· Chemistry Q1 1(a)(v)b)Determine the number of moles of oxygen produced in 45 seconds at RTP (room temperature and pressure). (1 mole of gas occupies 24 dm³ at RTP: Relative Atomic Mass O = 16)
  34. 1(a)(v)b)2 marks· Chemistry Q1 1(a)(v)b)Calculate EACH of the following: The number of moles of sodium hydroxide in the volume of sodium hydroxide used in (a) (iv)
  35. 1(a)(v)c)1 mark· Chemistry Q1 1(a)(v)c)Calculate EACH of the following: The number of moles of sodium hydroxide in 1 dm³ of this solution
  36. 1(a)(vi)2 marks· Chemistry Q1 1(a)(vi)Write a balanced equation for this reaction.
  37. 1(a)(vi)1 mark· Chemistry Q1 1(a)(vi)Using the graph plotted in (v) above, determine the mass of salt that would be formed from 2.95 g of copper(II) oxide.
  38. 1(a)(vi)2 marks· Chemistry Q1 1(a)(vi)Determine the number of moles of sodium hydroxide in the 25 cm³ of solution used.
  39. 1(a)(vi)2 marks· Chemistry Q1 1(a)(vi)Mass of sodium hydroxide dissolved in 250 cm³ of water (Relative atomic mass: Na = 23, O = 16, H = 1)
  40. 1(a)(vi)1 mark· Chemistry Q1 1(a)(vi)Determine the number of moles of sodium hydroxide in the 25 cm³ of solution used.
  41. 1(a)(vi)a)1 mark· Chemistry Q1 1(a)(vi)a)Calculate the number of moles of Mg in 0.12 g (Relative Atomic Mass of Mg = 24).
  42. 1(a)(vi)b)2 marks· Chemistry Q1 1(a)(vi)b)The volume of hydrogen gas produced at r.t.p. when all the magnesium ribbon reacts with the acid (1 mole of gas at r.t.p. occupies 24 dm³).
  43. 1(a)(vii)1 mark· Chemistry Q1 1(a)(vii)Explain why there is no change in the mass of salt produced for Experiments 4 and 5.
  44. 1(a)(vii)1 mark· Chemistry Q1 1(a)(vii)Calculate the number of moles of NaOH used in the reaction.
  45. 1(a)(vii)2 marks· Chemistry Q1 1(a)(vii)Calculate the concentration of sodium hydroxide, in g dm⁻³. (Molar mass of sodium hydroxide = 40 g mol⁻¹)
  46. 1(a)(vii)2 marks· Chemistry Q1 1(a)(vii)Calculate the concentration of NaOH in g dm⁻³. (Relative atomic mass: Na = 23; O = 16; H = 1)
  47. 1(a)(viii)1 mark· Chemistry Q1 1(a)(viii)Calculate the percentage purity of the sodium hydroxide solution.
  48. 1(a)(viii)2 marks· Chemistry Q1 1(a)(viii)Calculate the concentration of H₂SO₄ in mol dm⁻³.
  49. 1(a)(x)1 mark· Chemistry Q1 1(a)(x)Calculate the mass of copper that would be formed. (Relative atomic mass: Cu = 64; 1 F = 96 500 C)
  50. 1(b)1 mark· Chemistry Q1 1(b)Complete Table 1 by calculating the mass of the hydrated iron(II) sulfate used.
  51. 1(b)(i)2 marks· Chemistry Q1 1(b)(i)Write a balanced chemical equation for the reaction between calcium carbonate and hydrochloric acid.
  52. 1(b)(i)3 marks· Chemistry Q1 1(b)(i)Calculate the concentration, in mol dm⁻³, of KIO₃ in Solution 1. [RAM: K = 39.1, I = 126.9, O = 16.0]
  53. 1(b)(ii)3 marks· Chemistry Q1 1(b)(ii)Calculate the volume of carbon dioxide that would be produced at RTP from 1.0 g of CaCO₃ chips. [RMM: CaCO₃ = 100; 1 mole of a gas occupies 24 000 cm³ at RTP.]
  54. 1(b)(ii)2 marks· Chemistry Q1 1(b)(ii)The final concentration of NaHSO₃ in all experiments was 0.0008 mol dm⁻³. Using the information provided in Table 1 on page 6, determine the concentration of NaHSO₃ in Solution 2.
  55. 1(b)(iii)2 marks· Chemistry Q1 1(b)(iii)Write a suitable ionic equation for the reaction occurring in Beaker A.
  56. 1(b)(v)2 marks· Chemistry Q1 1(b)(v)Write a balanced equation for the formation of the normal salt from sulfuric acid and sodium hydroxide.
  57. 1(b)(vi)3 marks· Chemistry Q1 1(b)(vi)Calculate the number of moles of sulfuric acid used to neutralize the sodium hydroxide.
  58. 1(b)(vii)3 marks· Chemistry Q1 1(b)(vii)Use your answer in (b) (vi) to determine the number of moles of gas produced at 2.5 minutes. [one mole of gas occupies 22.4 dm³ at standard temperature and pressure.]
  59. 1(b)(vii)2 marks· Chemistry Q1 1(b)(vii)Calculate the mass of the normal salt expected from the reaction.
  60. 1(c)2 marks· Chemistry Q1 1(c)Write a balanced chemical equation to show the decomposition of hydrogen peroxide.
  61. 1(c)(i)3 marks· Chemistry Q1 1(c)(i)Record the final burette volumes from the diagrams in Figure 1 in the appropriate spaces in Table 2.
  62. 1(c)(i)2 marks· Chemistry Q1 1(c)(i)Write a balanced chemical equation, including state symbols, for the reaction between zinc metal and dilute hydrochloric acid.
  63. 1(c)(ii)3 marks· Chemistry Q1 1(c)(ii)Calculate the volume of KMnO4 solution used in EACH titration and enter them in Table 2.
  64. 1(c)(ii)2 marks· Chemistry Q1 1(c)(ii)Write a balanced chemical equation with state symbols for the reaction that occurred between magnesium and sulfuric acid in the experiments.
  65. 1(c)(iii)1 mark· Chemistry Q1 1(c)(iii)Determine the average volume of KMnO4 solution used in the titrations.
  66. 1(c)(iii)3 marks· Chemistry Q1 1(c)(iii)Calculate the maximum volume of hydrogen gas, at room temperature and pressure (RTP), that would be produced when 1.0 gram of zinc metal reacts with excess dilute hydrochloric acid. (1 mole of a gas occupies 24 dm³ at…
  67. 1(d)1 mark· Chemistry Q1 1(d)Using the information from (c)(ii), calculate the average number of moles of potassium dichromate used in the experiment.
  68. 1(d)(i)1 mark· Chemistry Q1 1(d)(i)As shown in the equation, 1 mole MnO4⁻ reacts with 5 moles of Fe²⁺. Using the result in (c)(iv), calculate the number of moles of Fe²⁺ ions in the 25.0 cm³ aliquot that reacted with the MnO4⁻.
  69. 1(d)(ii)1 mark· Chemistry Q1 1(d)(ii)Determine the number of moles of Fe²⁺ in the 250.0 cm³ volumetric flask.
  70. 1(d)(iv)1 mark· Chemistry Q1 1(d)(iv)Calculate the number of moles of KMnO4 in the average volume determined in (c)(iii).
  71. 1(e)1 mark· Chemistry Q1 1(e)From the equation given on page 4, determine the number of moles of iron ions (Fe²⁺) that react with 1 mole of dichromate ions (Cr₂O₇²⁻).
  72. 1(e)1 mark· Chemistry Q1 1(e)Given that 1 mole of FeSO4 contains 1 mole of Fe²⁺ ions, use the result from (d)(ii) to calculate the mass of anhydrous FeSO4 in the 250 cm³ volumetric flask. [The relative molecular mass of anhydrous FeSO4 is 152.]
  73. 1(e)(i)2 marks· Chemistry Q1 1(e)(i)Write a balanced chemical equation, including state symbols, for the reaction between zinc metal and sulfuric acid.
  74. 1(e)(ii)3 marks· Chemistry Q1 1(e)(ii)Calculate the total volume of hydrogen gas that would be produced at RTP from 0.55 g of zinc granules. [RAM: Zn = 65.4; 1 mole of a gas occupies 24 000 cm³ at RTP]
  75. 1(e)(iii)1 mark· Chemistry Q1 1(e)(iii)Determine the volume of oxygen produced after 10 s using the value obtained from (e) (ii).
  76. 1(f)1 mark· Chemistry Q1 1(f)Calculate the number of moles of iron in the iron salt sample.
  77. 1(f)1 mark· Chemistry Q1 1(f)Calculate the mass of water in the hydrated FeSO4 using the following formula: Mass of water = mass of hydrated FeSO4 [from (b)] - mass of anhydrous FeSO4 [from (e)].
  78. 1(g)1 mark· Chemistry Q1 1(g)Calculate the mass of iron in the iron salt sample. [Molar mass of Fe is 55.8 g mol⁻¹.]
  79. 1(g)1 mark· Chemistry Q1 1(g)Calculate the number of moles of water in the hydrated sample. [The relative molecular mass of water is 18.0.]
  80. 1(h)1 mark· Chemistry Q1 1(h)Calculate the percentage of iron in the iron salt sample.
  81. 1(h)1 mark· Chemistry Q1 1(h)Using the results from (d)(ii) and (g), calculate the value of n in the formula FeSO4•nH₂O. n = number of moles of water in hydrated sample / number of moles of anhydrous FeSO4.
  82. 2(a)2 marks· Chemistry Q2 2(a)Assuming that the limestone granules are pure calcium carbonate, write a balanced equation for its reaction with hydrochloric acid.
  83. 2(a)3 marks· Chemistry Q2 2(a)Calculate the number of moles of Al(OH)₃ in 250 g of Suspension P. (Relative Atomic Mass: Al = 27, O = 16, H = 1).
  84. 2(a)(i)2 marks· Chemistry Q2 2(a)(i)Define EACH of the following terms: Mole; Molar mass.
  85. 2(a)(ii)1 mark· Chemistry Q2 2(a)(ii)Calculate the mass Lesley would have to weigh to obtain 0.20 moles of aspirin.
  86. 2(a)(iii)1 mark· Chemistry Q2 2(a)(iii)Jared, another student in Lesley's class, weighed 18.0 g of aspirin. Calculate the number of moles of aspirin he weighed.
  87. 2(a)(iv)2 marks· Chemistry Q2 2(a)(iv)Write a balanced equation to show the formation of the normal salt stated in (a)(iii).
  88. 2(a)(vi)2 marks· Chemistry Q2 2(a)(vi)Write a balanced equation to show the formation of the acid salt stated in (a)(v).
  89. 2(b)3 marks· Chemistry Q2 2(b)Calculate the mass of ethanoic acid formed when Jared's 18.0 g of aspirin is hydrolysed. [Molar mass of ethanoic acid = 60.0 g mol⁻¹]
  90. 2(b)(i)2 marks· Chemistry Q2 2(b)(i)P reacts with water to produce a solution of its hydroxide and hydrogen gas. Write a balanced equation for the reaction between P and water.
  91. 2(b)(i)2 marks· Chemistry Q2 2(b)(i)Write a balanced ionic equation to represent the reaction that occurs in Experiment 4.
  92. 2(b)(ii)1 mark· Chemistry Q2 2(b)(ii)to calculate the moles of gas produced at STP [1 mole of any gas at STP has a volume of 22 400 cm³.]
  93. 2(b)(iii)2 marks· Chemistry Q2 2(b)(iii)to calculate the mass of limestone granules used. [Relative molecular mass of CaCO₃ is 100.]
  94. 2(b)(iv)2 marks· Chemistry Q2 2(b)(iv)Write an ionic equation (with state symbols) for the reaction which took place in Test 3.
  95. 2(b)(iv)4 marks· Chemistry Q2 2(b)(iv)A current of 5 amperes is passed through the molten lead bromide for 5 minutes. Calculate the mass of lead that would be deposited. (RAM: Pb = 207; Faraday's constant, F = 96 500 C mol⁻¹)
  96. 2(b)(v)2 marks· Chemistry Q2 2(b)(v)From your answer to (b) (iii), calculate the heat change when 1 mole of ammonium nitrate dissolves in water.
  97. 2(c)3 marks· Chemistry Q2 2(c)Calculate the percentage of carbon - 14 in 1 mole of tetrachloromethane, ¹⁴₆C³⁷₁₇Cl₄.
  98. 2(c)(i)2 marks· Chemistry Q2 2(c)(i)Write a balanced chemical IONIC equation for the reaction that is responsible for the colour change.
  99. 2(d)(i)2 marks· Chemistry Q2 2(d)(i)Calculate the quantity of electricity passed in coulombs.
  100. 2(d)(ii)3 marks· Chemistry Q2 2(d)(ii)If 5.0 grams of calcium nitrate are decomposed completely, calculate the volume of nitrogen dioxide produced at RTP. [One mole of a gas occupies 24 000 cm³ at RTP; RMM of Ca(NO₃)₂ = 164]
  101. 2(d)(ii)3 marks· Chemistry Q2 2(d)(ii)Calculate the mass of copper deposited. [Relative Atomic Mass of Cu = 64, Faraday's constant = 96500 coulombs]
  102. 2(d)(iii)2 marks· Chemistry Q2 2(d)(iii)Based on your answer in (d)(i) on page 9 and the information given in the question, calculate the mass of compound that will be formed when 54g of B reacts completely with A.
  103. 2(f)4 marks· Chemistry Q2 2(f)Determine the mass of copper (in grams) which will be deposited at the cathode when 5A of current passes through the electrolytic cell for half an hour. [R.A.M. Cu = 64; 1 Faraday = 96 500 C]
  104. 3(a)(i)3 marks· Chemistry Q3 3(a)(i)Calculate the empirical formula of B (Relative Atomic Mass: C = 12; O = 16; H = 1).
  105. 3(a)(ii)2 marks· Chemistry Q3 3(a)(ii)Write a balanced equation to show the decomposition of hydrogen peroxide by manganese (IV) oxide, MnO₂.
  106. 3(b)(i)2 marks· Chemistry Q3 3(b)(i)Calculate the molecular formula for A and B. (The relative formula mass of both A and B = 60).
  107. 3(b)(i)2 marks· Chemistry Q3 3(b)(i)Write a balanced equation for the reaction between chlorine and ammonia.
  108. 3(b)(ii)b)5 marks· Chemistry Q3 3(b)(ii)b)For 0.80 mol dm⁻³ H₂O₂ and 4.0 g of catalyst, determine the number of moles of O₂ produced in 16 seconds. [Atomic mass: O = 16]
  109. 3(b)(ii)c)5 marks· Chemistry Q3 3(b)(ii)c)For 0.80 mol dm⁻³ H₂O₂ and 4.0 g of catalyst, determine the volume of O₂ produced at S.T.P. in 16 seconds. [1 mole of gas occupies 22.4 dm³ at S.T.P.]
  110. 4(a)4 marks· Chemistry Q4 4(a)Deduce the molecular formula of X.
  111. 4(a)(i)2 marks· Chemistry Q4 4(a)(i)Calculate the relative atomic mass of Element M.
  112. 4(a)(ii)2 marks· Chemistry Q4 4(a)(ii)Write a balanced equation, including state symbols, to show the formation of the chloride of M.
  113. 4(a)(ii)2 marks· Chemistry Q4 4(a)(ii)Write a balanced equation to illustrate the reaction occurring in (a)(i) above.
  114. 4(a)(iii)5 marks· Chemistry Q4 4(a)(iii)A current of 5A is passed for 2 minutes through the molten BaBr₂. Calculate the mass of the product that will be formed at the cathode. (Relative atomic mass: Ba = 137, Br = 80) (1 Faraday = 96 500 C mol⁻¹)
  115. 4(b)(i)1 mark· Chemistry Q4 4(b)(i)Calculate the number of moles of KNO₃ used in the experiment. (RMM: KNO₃ = 101)
  116. 4(b)(ii)2 marks· Chemistry Q4 4(b)(ii)Calculate the mass of CaCO₃ used in the experiment. [RAM: Ca = 40, C = 12, O = 16]
  117. 4(b)(ii)3 marks· Chemistry Q4 4(b)(ii)Calculate the mass of copper that is deposited during the reaction. (Relative Atomic Mass: Cu = 64; 1F = 96 500 C)
  118. 4(c)5 marks· Chemistry Q4 4(c)A current of 5 A is passed for 10 minutes through the molten MgI₂. Calculate the mass of product that will be formed at the cathode. (Relative atomic masses: Mg = 24; I = 127) (1 Faraday = 96 500 C mol⁻¹)
  119. 4(c)(i)a)1 mark· Chemistry Q4 4(c)(i)a)The number of moles of KNO₃ used in the experiment.
  120. 5(a)2 marks· Chemistry Q5 5(a)Write a balanced equation for the reaction between hydrochloric acid and limestone.
  121. 5(a)(ii)4 marks· Chemistry Q5 5(a)(ii)Using balanced chemical equations, with state symbols, explain how the anhydride is converted to sulfuric acid in the manufacturing process.
  122. 5(a)(ii)2 marks· Chemistry Q5 5(a)(ii)Write an ionic equation for the reaction between Metal X and copper(II) sulphate. Include the relevant state symbols.
  123. 5(b)3 marks· Chemistry Q5 5(b)5.0 g of CaCO3 is allowed to react completely with hydrochloric acid. Using the balanced equation in (a), calculate the mass of gas that would be produced. [Relative Atomic Mass: Ca = 40, O = 16, C = 12]
  124. 5(b)(ii)2 marks· Chemistry Q5 5(b)(ii)Write an ionic equation for the reaction which occurs at the anode.
  125. 5(b)(ii)5 marks· Chemistry Q5 5(b)(ii)Calculate the mass of pure copper that would be produced during the experiment if a current of 5 A flowed for 30 minutes. (Molar mass of Cu: 64 g mol⁻¹)
  126. 5(c)4 marks· Chemistry Q5 5(c)Calculate the mass of copper produced if 0.12 dm³ of nitrogen is produced at room temperature and pressure (rtp). (Relative atomic mass of Cu = 64; One mole of gas occupies 24 dm³ at rtp.)
  127. 6(b)6 marks· Chemistry Q6 6(b)Write THREE relevant chemical equations to support your answer in (a). Include AT LEAST ONE equation from the action of yeast and ONE from the action of baking powder.
  128. 6(b)(i)3 marks· Chemistry Q6 6(b)(i)Write a balanced chemical equation, including state symbols, to show the formation of carbon monoxide.
  129. 6(b)(iv)2 marks· Chemistry Q6 6(b)(iv)Write the ionic equation, including state symbols, for the reaction between the iron and copper sulfate solution.
  130. 6(c)(i)3 marks· Chemistry Q6 6(c)(i)Write a balanced chemical equation, including state symbols, for the laboratory preparation of carbon dioxide gas from calcium carbonate.
  131. 1(a)(i) [P2]2 marks· CSEC Chemistry · January 2002 · Paper 2Write an ionic equation for the reaction taking place in the flask.
  132. 1(a)(iii) [P2]2 marks· CSEC Chemistry · January 2002 · Paper 2How many moles of hydrogen were collected at rtp? (1 mol of any gas at rtp has a volume of 24 dm³.)
  133. 1(a)(iv) [P2]1 mark· CSEC Chemistry · January 2002 · Paper 2How many moles of magnesium were used up?
  134. 1(b)(iii) [P2]1 mark· CSEC Chemistry · January 2002 · Paper 2In which test tube are the ions of neither solution M nor N in excess?
  135. 1(b)(v)a)1 mark· CSEC Chemistry · January 2002 · Paper 25.0 cm³ of solution N completely reacts with ______ cm³ of Solution M.
  136. 1(b)(v)b)1 mark· CSEC Chemistry · January 2002 · Paper 21 mole of lead ions completely reacts with ______ moles of iodide ions.
  137. 1(b)(vi) [P2]2 marks· CSEC Chemistry · January 2002 · Paper 2Use the answer in (v) b) to write the equation for the reaction taking place between lead ions and iodide ions.
  138. 3(b)2 marks· CSEC Chemistry · January 2002 · Paper 2Ethanol is oxidized in the body to CO2 and H2O, giving off 30 kJ per gram. Calculate the energy produced when 100 cm³ of an alcoholic drink (15% ethanol by weight, density 1 g/cm³) is consumed.
  139. 4(b)(ii) [P2]1 mark· CSEC Chemistry · January 2002 · Paper 2Determine the mass of carbon dioxide evolved.
  140. 4(b)(iii) [P2]2 marks· CSEC Chemistry · January 2002 · Paper 2Determine the mass of marble chips used.
  141. Q141 mark · multiple choice· CSEC Chemistry · January 2017 · Paper 1Ethanoic acid reacts with ethanol to form an ester and water. How many moles of ethanoic acid are required to produce 0.5\text{ mol} of the ester?
  142. Q271 mark · multiple choice· CSEC Chemistry · January 2017 · Paper 1\text{FeCl}_2 and \text{FeCl}_3 are two chlorides of iron. Which of the following statements about these two chlorides of iron is/are TRUE? I. The percentage of iron by mass in the two chlorides is different. II.…
  143. Q71 mark · multiple choice· CSEC Chemistry · January 2018 · Paper 1What mass of oxygen atoms contains the same number of moles as 112\text{ g} of sulfur atoms? [RAM: \text{O} = 16; \text{S} = 32]
  144. Q181 mark · multiple choice· CSEC Chemistry · January 2018 · Paper 1The relative atomic mass of carbon is 12 and that of oxygen is 16. Therefore, 88\text{ g} of carbon dioxide consists of
  145. Q141 mark · multiple choice· CSEC Chemistry · January 2019 · Paper 1How many moles of ethanoic acid are required to produce 0.5\text{ mol} of the ester?
  146. Q221 mark · multiple choice· CSEC Chemistry · January 2019 · Paper 1What mass of oxygen atoms contains the same number of moles as 112\text{ g} of sulfur atoms? [RAM: \text{O} = 16; \text{S} = 32]
  147. 1(d)2 marks· CSEC Chemistry · January 2021 · Paper 2Write a balanced chemical equation for the reaction between NaOH and H₂SO₄.
  148. 1(e)2 marks· CSEC Chemistry · January 2021 · Paper 2Calculate the number of moles of H₂SO₄ used in the reaction.
  149. 1(f)2 marks· CSEC Chemistry · January 2021 · Paper 2Calculate the number of moles of NaOH in 25 cm³ of the solution.
  150. 1(g)2 marks· CSEC Chemistry · January 2021 · Paper 2Calculate the concentration of NaOH, in mol dm⁻³.
  151. 1(h)1 mark· CSEC Chemistry · January 2021 · Paper 2Calculate the concentration of NaOH in g dm⁻³, given the molar mass of NaOH = 40 g mol⁻¹.
  152. 4(b)2 marks· CSEC Chemistry · January 2021 · Paper 2Calculate the number of atoms in 80.0 g of calcium. [Relative atomic mass of Ca = 40; Avogadro's constant = 6.0 × 10²³]
  153. 5(c)(ii)2 marks· CSEC Chemistry · January 2021 · Paper 2Hence, write a balanced chemical equation for Reaction 3.
  154. 6(a)(iii)2 marks· CSEC Chemistry · January 2021 · Paper 2Write a chemical equation, including state symbols, for the reaction between hydrochloric acid and sodium hydrogen carbonate.
  155. 6(b)2 marks· CSEC Chemistry · January 2021 · Paper 2Write an ionic equation for the reaction of magnesium with dilute hydrochloric acid.
  156. Q61 mark · multiple choice· CSEC Chemistry · May/June 2010 · Paper 1What mass of oxygen gas contains the same number of moles as 56\text{ g} of sulphur? (Relative atomic mass: \text{S} = 32, \text{O} = 16)
  157. Q71 mark · multiple choice· CSEC Chemistry · May/June 2010 · Paper 12\text{ g} of magnesium are reacted with excess dilute acid according to the equation \text{Mg(s)} + 2\text{H}^+\text{(aq)} \rightarrow \text{Mg}^{2+}\text{(aq)} + \text{H}_2\text{(g)} (Relative atomic mass of…
  158. Q81 mark · multiple choice· CSEC Chemistry · May/June 2010 · Paper 1The values of x and y in the equation x\text{ KOH} + 3\text{ Br}_2 \rightarrow y\text{ KBr} + \text{KBrO}_3 + 3\text{ H}_2\text{O} are
  159. Q91 mark · multiple choice· CSEC Chemistry · May/June 2010 · Paper 1The mass concentration of a potassium chloride solution is 60\text{ g}\cdot\text{dm}^{-3}. What is the mass of potassium chloride in 25\text{ cm}^3 of this solution?
  160. Q81 mark · multiple choice· CSEC Chemistry · May/June 2011 · Paper 1Which of the following mixtures can be referred to as a standard solution?
  161. Q101 mark · multiple choice· CSEC Chemistry · May/June 2011 · Paper 1Which of the following compounds has the GREATEST percentage by mass of carbon present in one mole? (M_r = \text{relative molecular mass}; relative atomic mass: \text{H} = 1; \text{C} = 12; \text{O} = 16)
  162. Q221 mark · multiple choice· CSEC Chemistry · May/June 2011 · Paper 1The ionic equation for the reaction between an acid and a carbonate may be represented as
  163. Q71 mark · multiple choice· CSEC Chemistry · May/June 2015 · Paper 1Which of the following pairs represents equal quantities of atoms?
  164. Q91 mark · multiple choice· CSEC Chemistry · May/June 2015 · Paper 1Sodium reacts with water according to the equation 2\text{Na(s)} + 2\text{H}_2\text{O}(l) \rightarrow 2\text{NaOH(aq)} + \text{H}_2\text{(g)} (Molar volume of gas = 24\text{ litres at rtp}). The number of litres…
  165. Q91 mark · multiple choice· CSEC Chemistry · May/June 2016 · Paper 1Which of the following aqueous solutions contains 1 mole of hydrogen ions?
  166. Q261 mark · multiple choice· CSEC Chemistry · May/June 2016 · Paper 12.32 g of an oxide of iron were heated in dry hydrogen. When the reaction was completed, 1.68 g of iron were formed. [RAM: \text{Fe} = 56; \text{O} = 16] The oxide of iron was
  167. Q71 mark · multiple choice· CSEC Chemistry · May/June 2017 · Paper 1Which of the following represents a balanced equation for the reaction between aqueous silver nitrate and aqueous sodium chloride?
  168. Q91 mark · multiple choice· CSEC Chemistry · May/June 2017 · Paper 1Sodium reacts with water according to the equation 2\text{Na}(\text{s}) + 2\text{H}_2\text{O}(l) \rightarrow 2\text{NaOH}(\text{aq}) + \text{H}_2(\text{g}). (Molar volume of gas = 24\text{ litres at rtp}) The…
  169. Q251 mark · multiple choice· CSEC Chemistry · May/June 2017 · Paper 1Which of the following statements is TRUE for the equation below? \text{Mg}(\text{s}) + \text{H}_2\text{SO}_4(\text{aq}) \rightarrow \text{MgSO}_4(\text{aq}) + \text{H}_2(\text{g})

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