The kinetics of the hydrolysis of methyl methanoate, CH₃COOCH₃, in aqueous solution were investigated by measuring the concentration of the ester after different time intervals. The reaction was found to be first order in the concentration of the ester. Use the data below to determine the rate constant for the reaction.
$\begin{array}{lllllll}\text { time, } & 0 & 1800 & 3600 & 5400 & 7200 & 9000 \\t / \mathrm{s} & & & & & & \\\text { concentration, } & 0.300 & 0.191 & 0.135 & 0.081 & 0.055 & 0.035 \\c /\left(\mathrm{mol} d \mathrm{~m}^{-3}\right) & & & & &\end{array}$

Question

The kinetics of the hydrolysis of methyl methanoate, CH₃COOCH₃, in aqueous solution were investigated by measuring the concentration of the ester after different time intervals. The reaction was found to be first order in the concentration of the ester. Use the data below to determine the rate constant for the reaction.

\begin{array}{lllllll}\text { time, } & 0 & 1800 & 3600 & 5400 & 7200 & 9000 \\t / \mathrm{s} & & & & & & \\\text { concentration, } & 0.300 & 0.191 & 0.135 & 0.081 & 0.055 & 0.035 \\c /\left(\mathrm{mol} d \mathrm{~m}^{-3}\right) & & & & &\end{array}

Quizplus · Accepted Answer

The rate constant for a first-order reaction is given by the equation:$$k = \frac{1}{t} \ln \frac{[A]_0}{[A]_t}$$where:* k is the rate constant* t is the time* [A]_0 is the initial concentration of the reactant* [A]_t is the concentration of the reactant at time tUsing the data in the table, we can calculate the rate constant as follows:$$k = \frac{1}{9000 s} \ln \frac{0.300 mol dm^{-3}}{0.035 mol dm^{-3}} = 7.87 	imes 10^{-4} s^{-1}$$Therefore, the correct answer is B.

The Kinetics of the Hydrolysis of Methyl Methanoate, CH3COOCH3, in Aqueous

The Kinetics of the Hydrolysis of Methyl Methanoate, CH₃COOCH₃, in Aqueous