1 .		Which concentration plot is linear for a first-order equation? (A is one of the reactants.) Online Text [Hint]
2 .		A reaction has a rate law: rate = k[A]2. What would you plot to have the concentration versus time data give a straight line? Online Text [Hint]
3 .		The decomposition of NOBr is second-order with respect to NOBr and second-order overall. If the initial concentration of NOBr is 0.102 M and the rate constant is 25 M-1 min-1, what is [NOBr] after 1.0 min? Online Text [Hint]
4 .		In a second-order reaction the rate constant is 4.0 x 10-4 M-1 s-1. What is the concentration of reactant after 10 min if the initial concentration is 0.800 M? Online Text [Hint]
5 .		The first-order rate constant for the decomposition of N2O5 to NO2 and O2 at 70°C is 6.82 x 10-3 s-1. Suppose we start with 0.300 mol of N2O5(g) in a 0.500-L container. How many moles of N2O5 will remain after 1.5 min? Online Text [Hint]
6 .		The thermal decomposition of N2O5(g) to form NO2(g) and O2(g) is a first-order reaction. The rate constant for the reaction is 5.1 x 10-4 s-1 at 318 K. What is the half-life of this process? Online Text [Hint]
7 .		The decomposition of NOBr is second-order with respect to NOBr and second-order overall. If the initial concentration of NOBr is 0.102 M and the rate constant is 25 M-1 min-1, what is the half-life of the reaction? Online Text [Hint]
8 .		The highly radioactive plutonium in nuclear waste undergoes first-order decay with a half-life of approximately 24,000 years. How many years must pass before the level of radioactivity due to the plutonium falls to 1/128th (about 1%) of its original potency? Online Text [Hint]
9 .		Which one of the following statements is incorrect? Online Text [Hint]
10 .		For the reaction: 2N2O5(g) --> 4NO2(g) + O2(g) the activation energy, Ea, and overall E are 100 kJ/mol and -23 kJ/mol, respectively. What is the activation energy for the reverse reaction? Online Text [Hint]
11 .		As the temperature of a reaction is increased, the rate of the reaction increases because the [Hint]
12 .		Assuming that collision factors are the same, rank the following in order of increasing rate constant: (i) Ea = 15 kJ/mol, E = -55 kJ/mol (ii) Ea = 25 kJ/mol, E = -50 kJ/mol (iii) Ea = 15 kJ/mol, E = -75 kJ/mol Online Text [Hint]
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