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(C) The rate constant $k$ is given by the Arrhenius equation: $k = p Z e^{-E_a/RT}$.For the reaction to proceed more rapidly,the rate constant $k$ mus

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$E_a$

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(C) The rate constant $k$ is given by the Arrhenius equation: $k = p Z e^{-E_a/RT}$.For the reaction to proceed more rapidly,the rate constant $k$ must increase.In the expression $k = p Z e^{-E_a/RT}$,$p$ is the steric factor,$Z$ is the collision frequency,$E_a$ is the activation energy,$R$ is the gas constant,and $T$ is the temperature.To increase $k$,the value of the exponential term $e^{-E_a/RT}$ must increase.This occurs when the exponent $-E_a/RT$ becomes less negative,which happens if the activation energy $E_a$ decreases or the temperature $T$ increases.Therefore,a decrease in the activation energy $E_a$ will cause the reaction to proceed more rapidly.

The rate constant is given by the equation $k = p Z e^{-E_a/RT}$. Which factor should register a decrease for the reaction to proceed more rapidly?

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