Energetics · CSEC Chemistry

76 past-paper questions on Energetics, part of Principles of Chemistry, from every CSEC Chemistry paper on Quelpr.

1. 1(a)(i)2 marks· Chemistry Q1 1(a)(i)Define the term 'heat of neutralization'.
2. 1(a)(i)4 marks· Chemistry Q1 1(a)(i)Identify the parts labelled A, B, C, D on the diagram.
3. 1(a)(i)4 marks· Chemistry Q1 1(a)(i)Use the data from Table 1 to plot a graph of temperature against volume of acid using the axes provided in Figure 1 on page 3. Two of the points have been plotted for you.
4. 1(a)(i)c)2 marks· Chemistry Q1 1(a)(i)c)Distinguish between an exothermic and an endothermic reaction.
5. 1(a)(ii)1 mark· Chemistry Q1 1(a)(ii)From the graph in (a)(i), determine the volume of acid required to neutralize 25 cm³ of potassium hydroxide.
6. 1(a)(ii)3 marks· Chemistry Q1 1(a)(ii)Use the data in Table 1 to plot a graph of temperature against volume of acid for Experiment 1 using the axes provided on page 5. The first two points have been plotted for you.
7. 1(a)(ii)a)2 marks· Chemistry Q1 1(a)(ii)a)Using the readings in Figure 2, complete Table 1 to show the final thermometer readings, and the changes in temperature.
8. 1(a)(ii)b)3 marks· Chemistry Q1 1(a)(ii)b)On the graph paper provided on page 5, plot the temperature change (ΔT) against mass of zinc added.
9. 1(a)(iii)1 mark· Chemistry Q1 1(a)(iii)From the graph, determine the volume of sulphuric acid required to completely neutralize 25 cm³ of sodium hydroxide.
10. 1(a)(iii)1 mark· Chemistry Q1 1(a)(iii)Determine the temperature difference during the reaction.
11. 1(a)(iii)2 marks· Chemistry Q1 1(a)(iii)Using the thermometer readings in Figure 1, complete Table 1 by recording the temperature for the addition of 10 cm³ and 20 cm³ of the H₂SO₄.
12. 1(a)(iii)c)1 mark· Chemistry Q1 1(a)(iii)c)From your graph, deduce the temperature change (ΔT) that will occur when 1.0 g of zinc is added to the copper(II) sulphate solution.
13. 1(a)(iv)3 marks· Chemistry Q1 1(a)(iv)Given that the difference in temperature from the start of the reaction to the point of neutralization is 18 °C, calculate the heat change at the point of neutralization for the reaction between sodium hydroxide and…
14. 1(a)(iv)3 marks· Chemistry Q1 1(a)(iv)Calculate the heat change at the point of neutralization for the reaction between potassium hydroxide and hydrochloric acid. [The specific heat capacity of solution is 4.2 kJkg⁻¹ °C⁻¹. Assume that the density of the…
15. 1(a)(iv)3 marks· Chemistry Q1 1(a)(iv)Plot the points for temperature against volume of acid added using the axes on page 3.
16. 1(a)(v)3 marks· Chemistry Q1 1(a)(v)Draw the TWO lines of best fit through the points in (iv) above where the temperature is increasing and where the temperature is decreasing and hence determine the end point of the reaction. Volume of H₂SO₄ at end point
17. 1(b)(i)9 marks· Chemistry Q1 1(b)(i)Use the readings shown in Figure 2 to complete Table 1.
18. 1(b)(i)2 marks· Chemistry Q1 1(b)(i)Define the term 'heat of solution'.
19. 1(b)(ii)1 mark· Chemistry Q1 1(b)(ii)Assuming that the heat absorbed by the conical flask = (mass of the conical flask) × (0.861 J g⁻¹ °C⁻¹) × (temperature change), calculate the heat absorbed by the conical flask used in the experiment.
20. 1(b)(ii)1 mark· Chemistry Q1 1(b)(ii)Figure 2 shows the thermometer readings for the initial and final temperatures obtained for Experiment 2. Record the reading, in °C, on each thermometer in the space provided.
21. 1(b)(iii)1 mark· Chemistry Q1 1(b)(iii)Assuming that the heat absorbed by the water = (mass of water in the conical flask) × (4.2 J g⁻¹ °C⁻¹) × (temperature change), calculate the heat absorbed by the water in the conical flask.
22. 1(b)(iii)3 marks· Chemistry Q1 1(b)(iii)Write a suitable procedure that could be carried out for Experiment 2.
23. 1(b)(iv)1 mark· Chemistry Q1 1(b)(iv)Calculate the TOTAL heat absorbed by the calorimeter. Total heat absorbed by the calorimeter = (heat absorbed by the conical flask) + (heat absorbed by water in the conical flask)
24. 1(b)(iv)3 marks· Chemistry Q1 1(b)(iv)Draw a labelled energy profile diagram for the reaction taking place in Experiment 2.
25. 1(b)(ix)3 marks· Chemistry Q1 1(b)(ix)The students noticed that when the sodium hydroxide solution was made in Part A, the volumetric flask got warm. Draw an energy profile diagram to show the heat change when sodium hydroxide dissolves in water.
26. 1(b)(v)1 mark· Chemistry Q1 1(b)(v)Calculate the heat of combustion of the candle wax. Heat of combustion = (total heat absorbed by the calorimeter) / (mass of candle burnt)
27. 1(b)(vi)1 mark· Chemistry Q1 1(b)(vi)What was the role of the can in this experiment?
28. 1(c)(i)2 marks· Chemistry Q1 1(c)(i)Procedure:
29. 1(c)(i)1 mark· Chemistry Q1 1(c)(i)Write up the Aim.
30. 1(c)(ii)3 marks· Chemistry Q1 1(c)(ii)Draw a fully labelled diagram of the apparatus required to conduct your experiment.
31. 1(c)(ii)2 marks· Chemistry Q1 1(c)(ii)Write up the Method or procedure.
32. 1(c)(iii)2 marks· Chemistry Q1 1(c)(iii)Data to be collected:
33. 1(c)(iii)1 mark· Chemistry Q1 1(c)(iii)Write up the Discussion of results: Data to be collected.
34. 1(c)(iii) continued2 marks· Chemistry Q1 1(c)(iii) continuedWrite up the Discussion of results: Steps for doing calculations.
35. 1(c)(iii) continued1 mark· Chemistry Q1 1(c)(iii) continuedWrite up the Discussion of results as it relates to aim.
36. 1(c)(iv)2 marks· Chemistry Q1 1(c)(iv)SAMPLE calculation to be performed to determine the heat of combustion per mole of the fuel:
37. 1(c)(v)2 marks· Chemistry Q1 1(c)(v)TWO possible sources of error in your experiment:
38. 1(f)2 marks· Chemistry Q1 1(f)Complete and label the energy profile diagram in Figure 3 to show how a catalyst affects the rate of reaction.
39. 2(b)(i)1 mark· Chemistry Q2 2(b)(i)State whether the process in Experiment III is exothermic or endothermic. The process is
40. 2(b)(ii)3 marks· Chemistry Q2 2(b)(ii)Draw a labelled energy profile diagram to show the heat changes involved in Experiment III.
41. 2(b)(iii)2 marks· Chemistry Q2 2(b)(iii)Calculate the heat change when 8 g of ammonium nitrate is dissolved in 50 cm³ of water. [Relative Atomic Mass: N = 14; H = 1; O = 16; the specific heat capacity of the solution is 4.2 kJ kg⁻¹ K⁻¹; density of water is…
42. 2(b)(iv)1 mark· Chemistry Q2 2(b)(iv)State ONE assumption necessary in your calculation in (b) (iii) above.
43. 3(c)3 marks· Chemistry Q3 3(c)Draw a fully labelled energy profile diagram to illustrate how the catalyst affects the rate of decomposition of hydrogen peroxide.
44. 4(a)3 marks· Chemistry Q4 4(a)What changes occur during a reaction that can account for this fact?
45. 4(a)(i)2 marks· Chemistry Q4 4(a)(i)Distinguish between the terms 'endothermic' and 'exothermic.'
46. 4(a)(ii)1 mark· Chemistry Q4 4(a)(ii)Generally, when chemical reactions take place, existing bonds are broken and new bonds are formed. Classify bond making AND bond breaking as either endothermic or exothermic processes.
47. 4(b)(i)1 mark· Chemistry Q4 4(b)(i)Define the term 'heat of neutralization'.
48. 4(b)(ii)2 marks· Chemistry Q4 4(b)(ii)It is observed that whenever a strong acid (such as HCl or HNO₃) is completely neutralized by a strong base (such as NaOH or KOH), the heat of neutralization (in kJ mol⁻¹) is the same. Account for this observation.
49. 4(b)(ii)2 marks· Chemistry Q4 4(b)(ii)Calculate the heat change for the reaction. Specific heat capacity of water = 4.2 J g⁻¹ °C⁻¹; Heat change = m × c × △T; Density of water = 1 g cm⁻³
50. 4(b)(iii)1 mark· Chemistry Q4 4(b)(iii)Calculate the enthalpy change for 1 mole of potassium nitrate.
51. 4(b)(iv)4 marks· Chemistry Q4 4(b)(iv)List TWO pieces of apparatus necessary to conduct the experiment in a school laboratory. State how EACH piece of apparatus is used.
52. 4(b)(v)3 marks· Chemistry Q4 4(b)(v)Draw a labelled energy profile diagram to represent the enthalpy change for the reaction. On your diagram, indicate the sign of △H for the reaction.
53. 4(c)(i)b)1 mark· Chemistry Q4 4(c)(i)b)The heat change for the reaction.
54. 4(c)(i)c)2 marks· Chemistry Q4 4(c)(i)c)The enthalpy change in kJ mol⁻¹ for the reaction.
55. 4(c)(ii)1 mark· Chemistry Q4 4(c)(ii)State ONE assumption you made in your calculation.
56. 4(c)(iii)3 marks· Chemistry Q4 4(c)(iii)Draw a labelled energy profile diagram to represent the enthalpy change for the reaction.
57. 5(b)(iii)3 marks· Chemistry Q5 5(b)(iii)Draw a fully labelled energy profile diagram of the reaction for the production of ammonia during the Haber process. You should name the reactants and products on your diagram.
58. 6(b)(iii)2 marks· Chemistry Q6 6(b)(iii)Energy use
59. 3(d) [P2]4 marks· CSEC Chemistry · January 2002 · Paper 2Explain how a simple sugar can be used to supply energy in the human body, including a chemical equation.
60. Q121 mark · multiple choice· CSEC Chemistry · January 2017 · Paper 1Two solutions are to be mixed in order to demonstrate endothermic change. Which of the following techniques would be MOST appropriate?
61. Q261 mark · multiple choice· CSEC Chemistry · January 2018 · Paper 1From the energy profile diagram above, it can be said that the reactants
62. Q121 mark · multiple choice· CSEC Chemistry · January 2019 · Paper 1Two solutions are to be mixed in order to demonstrate an endothermic change. Which of the following techniques would be MOST appropriate?
63. 1(a)3 marks· CSEC Chemistry · January 2021 · Paper 2Using the thermometer readings in Figure 1, complete Table 1 by recording the temperatures for additions of 5 cm³, 15 cm³ and 25 cm³ of H₂SO₄.
64. 1(b)(i)4 marks· CSEC Chemistry · January 2021 · Paper 2Plot the graph of temperature against volume of acid added using the axes provided in Figure 2.
65. 1(b)(ii)2 marks· CSEC Chemistry · January 2021 · Paper 2Draw two lines of best fit through the points on the graph: one where temperature is increasing and one where temperature is decreasing.
66. 1(b)(iii)2 marks· CSEC Chemistry · January 2021 · Paper 2Show the end point of the reaction on the graph and record the corresponding volume.
67. 1(i)2 marks· CSEC Chemistry · January 2021 · Paper 2State whether the reaction in the styrofoam cup was exothermic or endothermic and explain your answer.
68. Q361 mark · multiple choice· CSEC Chemistry · May/June 2010 · Paper 1When crystals of potassium nitrate are dissolved in water, the temperature of the solution decreases because
69. Q331 mark · multiple choice· CSEC Chemistry · May/June 2011 · Paper 1Which of the following statements would be TRUE of exothermic reactions? I. Heat energy is absorbed from the surroundings. II. Heat energy is given out to the surroundings. III. The products possess less energy than the…
70. Q331 mark · multiple choice· CSEC Chemistry · May/June 2013 · Paper 1The condensation of steam is an exothermic reaction. Which of the following statements are true for this reaction? I. Heat is absorbed. II. Heat is evolved. III. \Delta H is negative.
71. Q341 mark · multiple choice· CSEC Chemistry · May/June 2013 · Paper 1Item 34 refers to the Haber process for the production of ammonia, according to the equation \text{N}_2(\text{g}) + 3\text{H}_2(\text{g}) \rightarrow 2\text{NH}_3(\text{g}), \quad \Delta H = -92\text{ kJ mol}^{-1}…
72. Q241 mark · multiple choice· CSEC Chemistry · May/June 2015 · Paper 1When an exothermic reaction occurs, energy is
73. Q301 mark · multiple choice· CSEC Chemistry · May/June 2015 · Paper 1Which of the following diagrams BEST illustrates the course of an exothermic reaction?
74. Q271 mark · multiple choice· CSEC Chemistry · May/June 2016 · Paper 1Which of the following energy changes occurs during the breaking of a chemical bond?
75. Q131 mark · multiple choice· CSEC Chemistry · May/June 2017 · Paper 1Which of the following statements is TRUE of an endothermic reaction?
76. Q301 mark · multiple choice· CSEC Chemistry · May/June 2017 · Paper 1Which of the following diagrams illustrates the course of an exothermic reaction?