(B) The enthalpy change of a reaction $(\Delta H)$ is defined as the difference between the activation energy of the forward reaction $(Ea_{(f)})$ and

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(B) The enthalpy change of a reaction $(\Delta H)$ is defined as the difference between the activation energy of the forward reaction $(Ea_{(f)})$ and the activation energy of the reverse reaction $(Ea_{(b)})$.$\Delta H = Ea_{(f)} - Ea_{(b)}$Given:$Ea_{(f)} = 150 \ kJ \ mol^{-1}$$Ea_{(b)} = 260 \ kJ \ mol^{-1}$Substituting the values:$\Delta H = 150 \ kJ \ mol^{-1} - 260 \ kJ \ mol^{-1}$$\Delta H = -110 \ kJ \ mol^{-1}$

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

Medium

The activation energy for the forward reaction is $150 \ kJ \ mol^{-1}$ and that of the reverse reaction is $260 \ kJ \ mol^{-1}$. The enthalpy change for the reaction is:

A
$410 \ kJ \ mol^{-1}$
B
$-110 \ kJ \ mol^{-1}$
C
$110 \ kJ \ mol^{-1}$
D
$-410 \ kJ \ mol^{-1}$

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Chemical Kinetics

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Collision theory, Energy of activation and Arrhenius equation

For an exothermic reaction,where the enthalpy of reaction is $\Delta H$ in $kJ/mol$,the minimum value for the activation energy will be:

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For a first-order reaction $A \rightarrow P$,the rate constant $k$ depends on temperature $(T)$ according to the equation $\log \, k = - \frac{2000}{T} + 0.6$. The pre-exponential factor $A$ and the activation energy $E_a$ are,respectively:

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Catalysts are used to increase the rate of a chemical reaction. Because it

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Assertion $(A)$ : $A$ catalyst increases the rate of a reaction.
Reason $(R)$ : In presence of a catalyst, the activation energy of the reaction increases.
The correct answer is

MediumAP EAMCET 2007

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For $N_2 + 3H_2 \rightarrow 2NH_3$,$\Delta H = -22 \ kcal$,and $E_a = 70 \ kcal$. Hence $E_a$ for $2NH_3 \rightarrow N_2 + 3H_2$ is $.....$ $kcal$.

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The activation energy for the forward reaction is $150 \ kJ \ mol^{-1}$ and that of the reverse reaction is $260 \ kJ \ mol^{-1}$. The enthalpy change for the reaction is:

Similar Questions

For an exothermic reaction,where the enthalpy of reaction is $\Delta H$ in $kJ/mol$,the minimum value for the activation energy will be:

For a first-order reaction $A \rightarrow P$,the rate constant $k$ depends on temperature $(T)$ according to the equation $\log \, k = - \frac{2000}{T} + 0.6$. The pre-exponential factor $A$ and the activation energy $E_a$ are,respectively:

Catalysts are used to increase the rate of a chemical reaction. Because it

Assertion $(A)$ : $A$ catalyst increases the rate of a reaction.Reason $(R)$ : In presence of a catalyst, the activation energy of the reaction increases.The correct answer is

For $N_2 + 3H_2 \rightarrow 2NH_3$,$\Delta H = -22 \ kcal$,and $E_a = 70 \ kcal$. Hence $E_a$ for $2NH_3 \rightarrow N_2 + 3H_2$ is $.....$ $kcal$.

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Assertion $(A)$ : $A$ catalyst increases the rate of a reaction.
Reason $(R)$ : In presence of a catalyst, the activation energy of the reaction increases.
The correct answer is