AQA Jun 2017 Paper 2 Q3

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0 3 A series of experiments is carried out with compounds C and D. Using the data obtained, the rate equation for the reaction between the two compounds is deduced to be rate = k [C][D] 0 3 . 1 In one experiment at 25 C, the initial rate of reaction is 3.1103 mol dm3 s1 when the initial concentration of C is 0.48 mol dm3 and the initial concentration of D is 0.23 mol dm3 Calculate a value for the rate constant at this temperature and give its units. [3 marks] Rate constant Units *06* IB/M/Jun17/7405/2<br /> 0 3 . 2 An equation that relates the rate constant, k, to the activation energy, Ea, and the temperature, T, is ln k = Ea RT + ln A Use this equation and your answer from Question 3.1 to calculate a value, in kJ mol1, for the activation energy of this reaction at 25 C. For this reaction ln A = 16.9 The gas constant R = 8.31 J K1 mol1 (If you were unable to complete Question 3.1 you should use the value of 3.2103 for the rate constant. This is not the correct value.) [4 marks] Activation energy kJ mol1 *07* Turn overIB/M/Jun17/7405/2<br />

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