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(A) According to the Arrhenius equation, the rate constant $k$ is given by $k = A e^{-E_a/RT}$. Since the activation energy $E_a$ is always positive,

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Equilibrium constant may increase or decrease but rate constant always increases with temperature

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(A) According to the Arrhenius equation, the rate constant $k$ is given by $k = A e^{-E_a/RT}$. Since the activation energy $E_a$ is always positive, the rate constant $k$ always increases with an increase in temperature. According to the Van't Hoff equation, $\log \left(\frac{K_2}{K_1}\right) = \frac{\Delta H}{2.303 R} \left[\frac{1}{T_1} - \frac{1}{T_2}\right]$. If the reaction is endothermic $(\Delta H > 0)$, the equilibrium constant $K$ increases with temperature. If the reaction is exothermic $(\Delta H Therefore, the equilibrium constant may increase or decrease depending on the enthalpy change, while the rate constant always increases with temperature.

Which of the following statements is true about the equilibrium constant and rate constant of a single-step chemical reaction?

Similar Questions

$A$ graph plotted between $\log \,K$ vs $\frac{1}{T}$ for calculating activation energy is shown by:

Assertion : If the activation energy of a reaction is zero,temperature will have no effect on the rate constant.
Reason : Lower the activation energy,faster is the reaction.

Find True $(T)$ and False $(F)$ statements among the following:
$1.$ All collisions in a reaction result in the formation of products.
$2.$ All collisions in a reaction are effective.
$3.$ The number of collisions depends on the rate of reaction.

The rate constant of a reaction is increased $4$ times after the addition of a catalyst to the reaction mixture at the same temperature of $27^{\circ} C$. The change in the activation energy of this reaction is (Take $\ln(1/4) = -1.386, R = 8.314 \ J \ K^{-1} \ mol^{-1}$)

For $A + B \longrightarrow C + D$; $\Delta H = -20 \ kJ \ mol^{-1}$,the activation energy of the forward reaction is $85 \ kJ \ mol^{-1}$. The activation energy for the backward reaction is.....$kJ \ mol^{-1}$

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