2. (a) You study the effect of temperature on the rate of two reactions and graph the natural logarithm (ln) of the rate constant for each reaction as a function of 1 ? . Explain, with the aid of diagrams and equations, how the two graphs compare if (i) The activation energy of the second reaction is higher than the activation energy of the first reaction but the two reactions have the same frequency factor. (ii) The frequency factor of the second reaction is higher than the frequency factor of the first reaction but the two reactions have the same activation energy.
2. (a) You study the effect of temperature on the
(i) The activation energy of the second reaction is higher than the activation energy of the first reaction but the two reactions have the same frequency factor.
(ii) The frequency factor of the second reaction is higher than the frequency factor of the first reaction but the two reactions have the same activation energy.
(b) The rate equation for the reaction: A + B → C has been determined to be d[C]/dt = k [A][B] k = 10-3 mol-1 dm3 s -1
(i) What is the overall order of the reaction and what is the constant k called in the above equation?
(ii) When a 25 cm3 of a 0.3 M solution of A is mixed with 150 cm3 of a 0.2 M solution of B, what is the initial rate of formation of product?
(c) Urea (NH2CONH2), which is the end product in protein
The reaction is first order in urea and first order overall. When [NH2CONH2] = 0.200 M, the rate at 61 °C is 8.56 x 10-5 M s -1 .
(i) What is the value of the rate constant?
(ii) What is the concentration of urea in this solution after 1 hour if the starting concentration is 0.500 M?
(iii) How long does it take for the initial concentration of urea to decrease to half its value at 61 °C?
(iv) What is the proportion of starting material that remains after three (3) half-lives?
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