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2 marksEnergetics

CSEC Chemistry · January 2012 · Paper 2 · Question 1(a)(i)

Students conducted Experiment 1 to determine the heat of neutralization for the reaction between sodium hydroxide and sulfuric acid. The procedure involved measuring 25 cm³ of dilute sodium hydroxide into a styrofoam cup and 25 cm³ of sulfuric acid into a burette. Both solutions were left to reach room temperature before recording their initial temperatures. Sulfuric acid was added to the sodium hydroxide solution 3 cm³ at a time, with the mixture stirred after each addition, and the maximum temperature recorded in Table 1.

Define the term 'heat of neutralization'.

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Other parts of this question

  1. 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…[3 marks]
  2. 1(a)(iii)From the graph, determine the volume of sulphuric acid required to completely neutralize 25 cm³ of sodium hydroxide.[1 mark]
  3. 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…[3 marks]
  4. 1(b)(i)Define the term 'heat of solution'.[2 marks]
  5. 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…[1 mark]
  6. 1(b)(iii)Write a suitable procedure that could be carried out for Experiment 2.[3 marks]
  7. 1(b)(iv)Draw a labelled energy profile diagram for the reaction taking place in Experiment 2.[3 marks]
  8. 1(c)(i)Write a balanced half-equation to represent the change which takes place when Solution X reacts with aqueous iron(II) nitrate.[2 marks]
  9. 1(c)(ii)Explain whether Solution X is behaving as a reducing agent, an oxidizing agent or both.[3 marks]
  10. 1(c)(iii)Describe Observation 3 as indicated in Table 2.[2 marks]

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