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(A) The Arrhenius equation describes the dependence of the rate constant $k$ on temperature $T$ and activation energy $E_a$. The equation is given by

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$k = A e^{-E_a / RT}$

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(A) The Arrhenius equation describes the dependence of the rate constant $k$ on temperature $T$ and activation energy $E_a$. The equation is given by $k = A e^{-E_a / RT}$,where $A$ is the Arrhenius factor (or frequency factor),$R$ is the universal gas constant,$T$ is the absolute temperature in Kelvin,and $E_a$ is the activation energy. This equation shows that the rate constant $k$ increases exponentially with an increase in temperature $T$ and decreases with an increase in activation energy $E_a$.

What is the relationship between the temperature $T$ and the activation energy $E_a$ in the Arrhenius equation?

Similar Questions

Define the following terms:
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For a chemical reaction,the rate constant,activation energy,and Arrhenius factor at $25 \, ^\circ C$ are $3.0 \times 10^{-4} \, s^{-1}$,$104.4 \, kJ \, mol^{-1}$,and $6.0 \times 10^{14} \, s^{-1}$ respectively. Find the value of the rate constant as $T \rightarrow \infty$.

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Consider the given plots for a reaction obeying the Arrhenius equation $(0\,^{\circ}C < T < 300\,^{\circ}C)$: ($k$ and $E_a$ are rate constant and activation energy respectively). Choose the correct option.

Which statement is incorrect according to the Arrhenius equation?

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