1 .		What are the units of the rate constant for a reaction in solution that has an overall reaction order of two? (M is molarity, s is seconds.) Online Text [Hint]
2 .		For first-order reactions the rate constant, k, has the unit(s) Online Text [Hint]
3 .		The rate equation for the decomposition of H2O2 in the presence of I- is rate = k[H2O2][I-]. What are the units of the rate constant, k? Online Text [Hint]
4 .		In the reaction A --> products, the initial concentration of A is 1.56 M and the initial rate is 0.0190 M/sec. What is the value of the rate constant k in sec-1? Online Text [Hint]
5 .		The decomposition of N2O5 in carbon tetrachloride proceeds as follows: 2N2O5 --> 4NO2 + O2 The rate law is first-order in N2O5. At 45°C the rate constant is 6.08 x 10-4 s-1. What is the rate of the reaction when [N2O5] = 0.100 M, and what happens to the rate when the concentration of N2O5 is doubled to 0.200 M? Online Text [Hint]
6 .		The reaction 2NO + 2H2 --> N2 + 2H2O is first-order in H2 and second-order in NO. What happens to the rate when (i) [NO] is doubled, while [H2] is fixed (ii) [NO] is fixed, while [H2] is doubled (iii) both [NO] and [H2] are doubled? Online Text [Hint]
7 .		Consider the reaction in which nitric oxide is oxidized to nitrogen dioxide, 2 NO(g) + O2(g) ---> 2 NO2(g), for which the rate law is rate = k[NO]2[O2]. If this reaction takes place in a sealed vessel and the partial pressure of nitric oxide is doubled, what effect would this have on the rate of reaction? Online Text [Hint]
8 .		For the reaction 2NO2 + O3 --> N2O5 + O2 the following observations are made: Doubling the concentration of [NO2] doubles the rate, and doubling the concentration of [O3] doubles the rate. What is the rate law for the reaction? Online Text [Hint]
9 .		For a reaction of the type A + B + C going to products, the following observations are made: Doubling the concentration of A doubles the rate, doubling the concentration of B has no effect on the rate, and tripling the concentration of C increases the rate by a factor of 9. What is the rate law for the reaction? Online Text [Hint]
10 .		The decomposition of NOBr is monitored with the following results: Initial Rate Experiment Experiment Number [NOBr] (M) initial rate (M min-1) 1 0.0150 5.63 x 10-3 2 0.0225 1.27 x 10-2 3 0.0300 2.25 x 10-2 What is the rate law for the reaction and the value of the rate constant? Online Text [Hint]
11 .		The following data were collected for the rate of disappearance of NO in the reaction: 2NO(g) + O2 (g) --> 2NO2(g) Initial Rate Experiment Experiment Number [NO] (M) [O2] (M) initial rate (M/s) 1 0.0126 0.0125 1.41 x 10-2 2 0.0252 0.0250 1.13 x 10-1 3 0.0252 0.0125 5.64 x 10-2 What is the rate law for the reaction and the value of the rate constant? Online Text [Hint]
12 .		A kinetic study of the reaction 2A + 2B ----> products was conducted yielding the following results: Experiment [A], (M) [B], (M) Initial Rate, M/s-1 1 0.10 0.10 25 2 0.05 0.20 100 3 0.10 0.30 225 4 0.20 0.10 25 What is the rate law for the reaction? Online Text [Hint]
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