Medium
What is the effect of temperature on the rate constant of a reaction? How can this effect of temperature on rate constant be represented quantitatively?
(N/A) The rate constant of a chemical reaction generally increases with an increase in temperature. For many reactions,the rate constant is nearly doubled with a rise in temperature by $10^{\circ}C$.
The temperature effect on the rate constant is represented quantitatively by the Arrhenius equation:
$k = A e^{-E_a / RT}$
Where:
$k$ is the rate constant,
$A$ is the Arrhenius factor (or frequency factor),
$E_a$ is the activation energy for the reaction,
$R$ is the gas constant,
$T$ is the temperature in Kelvin.
The temperature effect on the rate constant is represented quantitatively by the Arrhenius equation:
$k = A e^{-E_a / RT}$
Where:
$k$ is the rate constant,
$A$ is the Arrhenius factor (or frequency factor),
$E_a$ is the activation energy for the reaction,
$R$ is the gas constant,
$T$ is the temperature in Kelvin.
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For the reaction $A_2 + B_2 \rightleftharpoons 2 AB$,the activation energies $(E_a)$ for the forward and backward reactions are $180 \ kJ \ mol^{-1}$ and $200 \ kJ \ mol^{-1}$ respectively. If a catalyst lowers the $E_a$ for both reactions by $100 \ kJ \ mol^{-1}$,which of the following statements is correct?
The slope of the Arrhenius plot $(\ln k \, vs \, \frac{1}{T})$ of a first-order reaction is $-5 \times 10^{3} \, K$. The value of $E_{a}$ of the reaction is: (in $kJ \, mol^{-1}$)
$[\text{Given } R = 8.314 \, J \, K^{-1} \, mol^{-1}]$
$[\text{Given } R = 8.314 \, J \, K^{-1} \, mol^{-1}]$
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