Which of the following statements is true abo | vedclass

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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?

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