Questions Q1. Given the following data: select the expression which gives the enthalpy change, in kj mol 1, for the reaction: ( 820 ½) = 140
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1 Questions Q1. Given the following data: select the expression which gives the enthalpy change, in kj mol 1, for the reaction: A ( 820 ½) = 140 B (+820 ½) 270 = +140 C (270 2) = 280 D +820 (270 2) = +280 (Total for question = 1 mark) Q2. The enthalpy change of combustion of ethanol was determined using the apparatus shown in the diagram below. In the experiment, the temperature increase of the water in the beaker is measured when a known mass of the ethanol is burned. (a) The results of the experiment are summarised in the table below.
2 (i) Calculate the heat energy produced by the combustion of the alcohol using the equation. heat energy produced (J) = mass of water x 4.18 x temperature change (ii) Calculate the number of moles of ethanol burned in this experiment (the formula of ethanol is C 2 H 5 OH). (iii) Use the equation below to calculate the enthalpy change of combustion of ethanol in kj mol 1. Give the value an appropriate sign. ΔH = heat energy produced number of moles (b) The data book value for the enthalpy change of combustion of ethanol is 1370 kj mol 1. (i) Calculate the percentage error in the value calculated in (a)(iii) in comparison with the data book value. (ii) List three ways in which the design of the experiment causes the results to be so different from the data book value. (You should be specific but detailed explanations are not required.) 1 2 3
3 (iii) Use the data book values for enthalpy changes of combustion given in the table below to calculate the enthalpy change of formation of ethanol. (Total for question = 13 marks) Q3. The equation for the complete combustion of butanone, C 2 H 5 COCH 3, is C 2 H 5 COCH 3 (l) + 5½O 2 (g) 4CO 2 (g) + 4H 2 O(l) ΔH = 2440 kj mol 1 From the above data, the standard enthalpy change of formation of butanone, in kj mol 1, is A 280 B +280 C 1760 D (Total for Question = 1 mark) Q4. (a) On strong heating, calcium carbonate decomposes to calcium oxide and carbon dioxide: Owing to the conditions under which the reaction occurs, it is not possible to measure the enthalpy change directly.
4 An indirect method employs the enthalpy changes when calcium carbonate and calcium oxide are neutralized with hydrochloric acid. (i) Write the equation for the reaction of calcium carbonate with hydrochloric acid. State symbols are not required. [ΔH 1 is the enthalpy change for this reaction] ΔH 1 (ii) The reaction of calcium oxide with hydrochloric acid is Use the equations in parts (i) and (ii) to complete the Hess's Law cycle below to show how you could calculate the enthalpy change for the decomposition of calcium carbonate, ΔH reaction. Label the arrows in your cycle. (iii) Complete the expression for ΔH reaction in terms of ΔH 1 and ΔH 2. ΔH reaction = (b) Suggest two reasons why the value obtained by carrying out these two experiments and using the equation gives a value different to the data booklet value for the decomposition reaction of calcium carbonate.
5 (Total for question = 7 marks) Q5. Propanone, C 3 H 6 O, undergoes complete combustion to form carbon dioxide and water. (a) In an experiment to calculate the enthalpy change of combustion for propanone, 2.90 g of propanone was burned completely in oxygen. The heat energy from this combustion raised the temperature of 200 g of water from 20.2 C to 78.4 C. The specific heat capacity of water is 4.18 J g 1 C 1. (i) Calculate the number of moles of propanone present in 2.90 g. [The molar mass of propanone is 58 g mol 1.] (ii) Use the expression to calculate the heat energy transferred to raise the temperature of 200 g of water from 20.2 C to 78.4 C. (iii) Use your answers to (a)(i) and (ii) to calculate a value for the enthalpy change of combustion of propanone. Give your answer to three significant figures and include a sign and units. (b) In another experiment, the enthalpy change of combustion for butanone, C 4 H 8 O, was
6 found to be 1300 kj mol 1. A Data Book value for the standard enthalpy change of combustion for butanone is 2440 kj mol 1. (i) Suggest a reason why the value obtained in the experiment is so different from the Data Book value. (ii) This Data Book value ( 2440 kj mol 1 ) refers to the following equation. How would the value be different if it referred to the formation of water in the gaseous state? Justify your answer. Difference Justification (c) Standard enthalpy changes of combustion can be used to calculate the standard enthalpy change of formation of a compound. (i) Define the term standard enthalpy change of formation, making clear the meaning of standard in this context. (ii) Use the standard enthalpy changes of combustion, ΔH c, given in the table below to find the standard enthalpy change of formation for ethanoic acid, CH 3 COOH, in kj mol 1.
7 (Total for question = 15 marks) Q6. This question is about methanol and the energy changes that accompany some of its reactions. (a) Complete the diagram (using dots and crosses) to show the bonding in methanol, CH 3 OH. You should show outer electrons only. (b) The Hess cycle below can be used to calculate the standard enthalpy change of combustion of methanol, using standard enthalpy changes of formation. (i) Complete the cycle by filling in the empty box. *(ii) Define the term standard enthalpy change of formation of a compound, making clear the meaning of standard in this context.
8 (iii) Use your cycle and the data below to calculate the standard enthalpy change of combustion of methanol, ΔH c. (c) An experiment was carried out, using the apparatus below, to estimate the standard enthalpy change of combustion of methanol. After burning the methanol for a few minutes, the temperature of water in the beaker had risen by 20.7 C and the mass of methanol burnt was g. (i) Calculate the amount of energy transferred to the water. Energy transferred (J) = mass of water 4.18 temperature change
9 (ii) Calculate the number of moles of methanol, CH 3 OH, burnt during the experiment. (iii) Use your answers to (c)(i) and (ii) to calculate the experimental value for the standard enthalpy change of combustion. Include a sign and units in your answer, which should be given to three significant figures. (iv) Compare your answers to (b)(iii) and (c)(iii) and give TWO reasons to explain any differences. (Total for question = 14 marks) Q7. The enthalpy change for the reaction to form hydrated sodium thiosulfate crystals cannot be measured directly. The following Hess cycle can be used. The enthalpy change for the reaction, ΔH r, is equal to A ΔH 1 + ΔH 2 B ΔH 1 ΔH 2 C ΔH 1 ΔH 2 D ΔH 1 + ΔH 2
10 Powered by TCPDF ( (Total for question = 1 mark)
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