SAMPLE EXERCISE 14.7 Using the Integrated First-Order Rate Law

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Presentation transcript:

SAMPLE EXERCISE 14.7 Using the Integrated First-Order Rate Law The decomposition of a certain insecticide in water follows first-order kinetics with a rate constant of 1.45 yr–1 at 12°C. A quantity of this insecticide is washed into a lake on June 1, leading to a concentration of 5.0  10–7 g/cm3. Assume that the average temperature of the lake is 12°C. (a) What is the concentration of the insecticide on June 1 of the following year? (b) How long will it take for the concentration of the insecticide to drop to 3.0  10–7 g/cm3?

SAMPLE EXERCISE 14.8 Determining Reaction Order from the Integrated Rate Law The following data were obtained for the gas-phase decomposition of nitrogen dioxide at 300°C, Is the reaction first or second order in NO2?

SAMPLE EXERCISE 14.9 Determining the Half-life of a First-Order Reaction The reaction of C4H9Cl with water is a first-order reaction. Figure 14.4 shows how the concentration of C4H9Cl changes with time at a particular temperature. (a) From that graph, estimate the half-life for this reaction. (b) Use the half-life from (a) to calculate the rate constant.

SAMPLE EXERCISE 14.12 Determining Molecularity and Identifying Intermediates It has been proposed that the conversion of ozone into O2 proceeds by a two-step mechanism: (a) Describe the molecularity of each elementary reaction in this mechanism. (b) Write the equation for the overall reaction. (c) Identify the intermediate(s).

SAMPLE EXERCISE 14.14 Determining the Rate Law for a Multistep Mechanism The decomposition of nitrous oxide, N2O, is believed to occur by a two-step mechanism: (a) Write the equation for the overall reaction. (b) Write the rate law for the overall reaction.