CIE Nov 2014 v1 Paper 4 Q1

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PMT Section A Answer all the questions in the spaces provided. (a) The oxidation of nitrogen(II) oxide is shown in the equation. 2NO(g) + O2(g)2NO2(g) The initial rate of this reaction was measured, starting with different concentrations of the two reactants. The following results were obtained. experiment number [NO] / mol dm3 [O2] / mol dm3 1 2 3 4 0.032 0.032 0.064 0.096 0.012 0.024 0.024 0.036 initial rate / mol dm3 s1 4.08103 8.15103 3.28102 (i) Use the data in the table to determine the order with respect to each reactant. Show your reasoning.(ii) Calculate the initial rate in experiment 4. Give your answer to two signi cantgures. initial rate =mol dm3 s1 (iii) Write the rate equation for this reaction.(iv) Use the results of experiment 1 to calculate the rate constant, k, for this reaction. Include the units of k. rate constant, k =units[6]UCLES 2014 9701/41/O/N/14<br /> (b) (i) On the following axesdraw two Boltzmann distribution curves, at two different temperatures, T1 and T2 (T2 > T1), label the curves and the axes. PMT (ii) State and explain, using your diagram, the effect of increasing temperature on the rate of reaction.[5] (c) The compound nitrosyluoride, NOF, can be formed by the following reaction. 2NO(g) + F2(g) 2NOF(g) The rate isrst order with respect to NO and F2. The reaction mechanism has two steps. Suggest equations for the two steps of this mechanism, stating which is the rate determining slower step.[2] [Total: 13]UCLES 2014 9701/41/O/N/14 [Turn over<br />

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