HW #7 - Chemistry 132, Winter 2008 Solutions to Homework...

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Chemistry 132, Winter 2008 Solutions to Homework No. 7 Problem 1. See Levine problem 17.1. (a) False. Only reactions whose rate law has a particular form (Levine eq. 17.5) can be said to have an order. Other reactions do not have an overall order. For example, reaction (1) in Levine eq. 17.6 does not have an order. (b) False. The dimensions of a rate constant must be such that when the rate constant is multiplied by the appropriate powers of the concentrations of the relevant species (Levine eq. 17.5) the units of the result, which is a reaction rate, are those of concentration divided by time (Levine eq. 17.4). Therefore, the units of k are (dm 3 / mol) n - 1 s - 1 (Levine p. 530), where n is the overall order of the reaction. Since n depends on the particular reaction, the units of k are not the same for all reactions. (c) True. The rate of a homogeneous reaction (Levine eq. 17.1) is the derivative of a concentration with respect to time (Levine eq. 17.4). Therefore, homogeneous reaction rates have units of concentration divided by time. (d) False. Partial orders can be fractional, as in reaction (5) of Levine eq. 17.6. (e) True. The rate constant k is experimentally found to be a function of temperature and pressure (Levine p. 530). (f) False. Partial orders can be negative, as in reaction (8) of Levine eq. 17.6. (g) True. The rate of conversion J (Levine eq. 17.2) is defined to be positive or zero (Levine p. 529). Thus, the rate of reaction r J/V (Levine eq. 17.3) must be positive or zero, because volume cannot be negative. Then, the rate constant k = r/ ([ A ] α [ B ] β ··· [ L ] λ ) (Levine eq 17.5) must non-negative, because concentrations cannot be negative. (h) False. A catalyst is neither a reactant nor a product, but may appear in a rate law, as does NO in reaction (6) of Levine eq. 17.6. Problem 4. See Levine problem 17.10, but use the mechanism given in
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HW #7 - Chemistry 132, Winter 2008 Solutions to Homework...

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