/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 116 The rate of a chemical reaction ... [FREE SOLUTION] | 91影视

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Chapter 13: Problem 116

The rate of a chemical reaction is too slow to measure at room temperature. We could either raise the temperature or add a catalyst. Which would be a better solution for making an accurate determination of the rate constant?

Short Answer

Expert verified
Answer: Adding a catalyst is a better solution for making an accurate determination of the rate constant in this case, as it can increase the rate of the reaction without increasing the number of side reactions.

Step by step solution

01

Effects of Temperature on Rate Constant

Increasing the temperature typically increases the rate of a chemical reaction. According to the Arrhenius Equation: \(k = Ae^{(-Ea/RT)}\), where \(k\) is the rate constant, \(A\) is the pre-exponential factor, \(Ea\) is the activation energy, \(R\) is the gas constant, and \(T\) is the temperature in Kelvin. As the temperature increases, the exponent term becomes larger and the rate constant increases. However, increasing temperature can lead to an increase in the number of side reactions, which can potentially cause inaccuracies in the determination of the rate constant.
02

Effects of Catalysts on Rate Constant

A catalyst is a substance that increases the rate of a chemical reaction without being consumed in the reaction. Catalysts work by lowering the activation energy of the reaction, which increases the rate constant according to the Arrhenius Equation. Unlike increasing temperature, adding a catalyst does not increase the number of side reactions.
03

Comparing Temperature and Catalyst Effects on Rate Constant Determination

Both increasing temperature and adding a catalyst can increase the rate constant; however, they have different effects on the reaction. Increasing the temperature can cause an increase in side reactions, potentially leading to inaccuracies in determining the rate constant. On the other hand, adding a catalyst lowers the activation energy, making the reaction faster without increasing side reactions.
04

Conclusion

It can be concluded that adding a catalyst would be a better solution for making an accurate determination of the rate constant in this case. A catalyst can increase the rate of the reaction without increasing the number of side reactions, which allows for a more accurate determination of the rate constant.

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Most popular questions from this chapter

Tropospheric Ozone Tropospheric (lower atmosphere) ozone is rapidly consumed in many reactions, including $$\mathrm{O}_{3}(g)+\mathrm{NO}(g) \rightarrow \mathrm{NO}_{2}(g)+\mathrm{O}_{2}(g)$$ Use the following data to calculate the instantaneous rate of the reaction at \(t=0.000 \mathrm{s}\) and \(t=0.052 \mathrm{s}\) $$\begin{array}{cc}\text { Time (s) } & {[\mathrm{NO}](\mathrm{M})} \\\0.000 & 2.0 \times 10^{-8} \\\\\hline 0.011 & 1.8 \times 10^{-8} \\\\\hline 0.027 & 1.6 \times 10^{-8} \\\\\hline 0.052 & 1.4 \times 10^{-8} \\\\\hline 0.102 & 1.2 \times 10^{-8} \\\\\hline\end{array}$$

Two reactions in which there is a single reactant have nearly the same magnitude rate constant. One is first order; the other is second order. a. If the initial concentrations of the reactants are both \(1.0 \mathrm{mM},\) which reaction will proceed at the higher rate? b. If the initial concentrations of the reactants are both 2.0 \(M,\) which reaction will proceed at the higher rate?

The kinetics of the reaction between chlorine dioxide and ozone are relevant to the study of atmospheric ozone destruction. The value of the rate constant for the reaction between chlorine dioxide and ozone was measured at four temperatures between 193 and \(208 \mathrm{K}\). The results were as follows: $$\begin{array}{cc}T(\mathrm{K}) & k\left(M^{-1} \mathrm{s}^{-1}\right) \\\193 & 34.0 \\\\\hline 198 & 62.8 \\\\\hline 203 & 112.8 \\\\\hline 208 & 196.7 \\\\\hline\end{array}$$ a. Calculate the values of the activation energy and the frequency factor for the reaction. b. What is the value of the rate constant higher in the stratosphere where \(T=245 \mathrm{K} ?\)

On the basis of the frequency factors and activation energy values of the following two reactions, determine which one will have the larger rate constant at room temperature \((298 \mathrm{K})\). \(\mathrm{O}_{3}(g)+\mathrm{O}(g) \rightarrow \mathrm{O}_{2}(g)+\mathrm{O}_{2}(g)\) \(A=8.0 \times 10^{-12} \mathrm{cm}^{3} /(\text { molecules } \cdot \mathrm{s}) \quad E_{\mathrm{a}}=17.1 \mathrm{kJ} / \mathrm{mol}\) \(\mathrm{O}_{3}(g)+\mathrm{Cl}(g) \rightarrow \mathrm{ClO}(g)+\mathrm{O}_{2}(g)\) \(A=2.9 \times 10^{-11} \mathrm{cm}^{3} /(\text { molecules } \cdot \mathrm{s}) \quad E_{\mathrm{a}}=2.16 \mathrm{kJ} / \mathrm{mol}\)

The dimerization of ClO, $$2 \mathrm{ClO}(g) \rightarrow \mathrm{Cl}_{2} \mathrm{O}_{2}(g)$$ is second order in ClO. a. Use the following data to determine the value of \(k\) at \(298 \mathrm{K}\) $$\begin{array}{cc} \text { Time (s) } & \text { [ClO] (molecules/cm }^{3} \text { ) } \\ 0 & 2.60 \times 10^{11} \\ \hline 1.00 & 1.08 \times 10^{11} \\ \hline 2.00 & 6.83 \times 10^{10} \\ \hline 3.00 & 4.99 \times 10^{10} \\ \hline 4.00 & 3.93 \times 10^{10} \\ \hline \end{array}$$ b. Determine the half-life for the dimerization of C1O.
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