(C) catalyst provides an alternative reaction pathway with a lower activation energy. In a reversible reaction,it lowers the activation energy for bot

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Decreases the activation energy of both,forward and backward reaction

(C) catalyst provides an alternative reaction pathway with a lower activation energy. In a reversible reaction,it lowers the activation energy for both the forward and backward reactions equally,thereby increasing the rate of both reactions without affecting the equilibrium constant.

Class 12 Chemistry Chemical Kinetics Collision theory, Energy of activation and Arrhenius equation

Easy

In a reversible reaction,the catalyst

A
Increases the activation energy of the backward reaction
B
Increases the activation energy of the forward reaction
C
Decreases the activation energy of both,forward and backward reaction
D
Decreases the activation energy of forward reaction

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Chemical Kinetics

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Collision theory, Energy of activation and Arrhenius equation

The rate constant of a reaction depends on ................

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For two reactions,the values of the pre-exponential factor are the same. However,the difference between their activation energy values is $24.9 \, kJ \, mol^{-1}$. The ratio of their rate constants at $300 \, K$ is ....

Medium

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The rate of a reaction quadruples when temperature changes from $27^{\circ} C$ to $57^{\circ} C$. Calculate the energy of activation.
Given $R=8.314 \ J \ K^{-1} \ mol^{-1}, \log 4=0.6021$

MediumNEET 2024

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For the reaction $A \rightarrow B$,the rate constant $k$ (in $s^{-1}$) is given by $\log_{10} k = 20.35 - \frac{2.47 \times 10^{3}}{T}$. The energy of activation in $kJ \, mol^{-1}$ is ..... . (Nearest integer) [Given: $R = 8.314 \, J \, K^{-1} \, mol^{-1}$]

DifficultJEE MAIN 2021

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In the given graph,$E_{a}$ for the reverse reaction will be (in $kJ$)

EasyKCET 2025

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In a reversible reaction,the catalyst

Similar Questions

The rate constant of a reaction depends on ................

For two reactions,the values of the pre-exponential factor are the same. However,the difference between their activation energy values is $24.9 \, kJ \, mol^{-1}$. The ratio of their rate constants at $300 \, K$ is ....

The rate of a reaction quadruples when temperature changes from $27^{\circ} C$ to $57^{\circ} C$. Calculate the energy of activation.Given $R=8.314 \ J \ K^{-1} \ mol^{-1}, \log 4=0.6021$

For the reaction $A \rightarrow B$,the rate constant $k$ (in $s^{-1}$) is given by $\log_{10} k = 20.35 - \frac{2.47 \times 10^{3}}{T}$. The energy of activation in $kJ \, mol^{-1}$ is ..... . (Nearest integer) [Given: $R = 8.314 \, J \, K^{-1} \, mol^{-1}$]

In the given graph,$E_{a}$ for the reverse reaction will be (in $kJ$)

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The rate of a reaction quadruples when temperature changes from $27^{\circ} C$ to $57^{\circ} C$. Calculate the energy of activation.
Given $R=8.314 \ J \ K^{-1} \ mol^{-1}, \log 4=0.6021$