(B) The activation energy $(E_a)$ for a reaction is defined as the difference between the energy of the transition state $(E_{TS})$ and the energy of

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(B) The activation energy $(E_a)$ for a reaction is defined as the difference between the energy of the transition state $(E_{TS})$ and the energy of the reactants $(E_R)$.$E_a = E_{TS} - E_R$Given:$E_{TS} = 170 \ kJ$$E_R = 50 \ kJ$Therefore,$E_a = 170 \ kJ - 50 \ kJ = 120 \ kJ$.Thus,the correct option is $B$.

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

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The graph for the process $R \rightarrow P$ is given below. Determine the activation energy $(E_a)$ for the forward reaction if the energy of the reactant is $50 \ kJ$ and the energy of the transition state is $170 \ kJ$. (in $kJ$)

GSEB 2023 All GSEB

A
$50$
B
$120$
C
$170$
D
$220$

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Class 12

Chemistry Questions

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Chemical Kinetics

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Collision theory, Energy of activation and Arrhenius equation

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The activation energy of a chemical reaction can be determined by:

MediumKCET 2016

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$A$ reaction having equal activation energies for forward and reverse reaction has:

Easy

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When the temperature of a reaction is increased from $300 \ K$ to $310 \ K$,the rate of the reaction increases by $2.5$ times. If the rate constant of the reaction at $300 \ K$ is $K$,what will be the rate constant at $310 \ K$?

Medium

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The rate constant for the first order decomposition of a certain reaction is described by the equation $\ln k (s^{-1}) = 14.34 - \frac{1.25 \times 10^{4} \ K}{T}$. The energy of activation for this reaction is

MediumAIIMS 2018

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The time taken for half of the initial amount of $N_2O_5$ to decompose is $12 \ min$ at $310 \ K$ and $2 \ hrs$ at $300 \ K$. The activation energy of the reaction in $kJ \ mol^{-1}$ is $\left(R=8.3 \ J \ K^{-1} \ mol^{-1}\right)$

EasyAP EAMCET 2019

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The graph for the process $R \rightarrow P$ is given below. Determine the activation energy $(E_a)$ for the forward reaction if the energy of the reactant is $50 \ kJ$ and the energy of the transition state is $170 \ kJ$. (in $kJ$)

Similar Questions

The activation energy of a chemical reaction can be determined by:

$A$ reaction having equal activation energies for forward and reverse reaction has:

When the temperature of a reaction is increased from $300 \ K$ to $310 \ K$,the rate of the reaction increases by $2.5$ times. If the rate constant of the reaction at $300 \ K$ is $K$,what will be the rate constant at $310 \ K$?

The rate constant for the first order decomposition of a certain reaction is described by the equation $\ln k (s^{-1}) = 14.34 - \frac{1.25 \times 10^{4} \ K}{T}$. The energy of activation for this reaction is

The time taken for half of the initial amount of $N_2O_5$ to decompose is $12 \ min$ at $310 \ K$ and $2 \ hrs$ at $300 \ K$. The activation energy of the reaction in $kJ \ mol^{-1}$ is $\left(R=8.3 \ J \ K^{-1} \ mol^{-1}\right)$

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