For a reaction,$A \rightarrow B$,the average energies of $A$ and $B$ are $30 \ kcal/mol$ and $60 \ kcal/mol$ respectively. The energy of activation for the backward reaction is $93 \ kcal/mol$. The energy of activation for the forward reaction is:
- A$30 \ kcal/mol$
- B$123 \ kcal/mol$
- C$153 \ kcal/mol$
- D$90 \ kcal/mol$
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Similar Questions
The rate of a reaction can be expressed by the Arrhenius equation as:
$k = A e^{-E_a / RT}$
In this equation,$E_a$ represents:
$k = A e^{-E_a / RT}$
In this equation,$E_a$ represents:
The decomposition of a hydrocarbon follows the equation $k = (4.5 \times 10^{11} \ s^{-1}) e^{-28000 \ K / T}$. Calculate the activation energy $E_a$.
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View SolutionFor a reaction,the rate constants $K_1$ and $K_2$ are given by $10^{16} \cdot e^{-2000/T}$ and $10^{15} \cdot e^{-1000/T}$ respectively. At what temperature will $K_1 = K_2$?
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View SolutionFor a certain gaseous reaction,the temperature is increased by $10\,^{\circ}C$ from $25\,^{\circ}C$ to $35\,^{\circ}C$. If the rate of the reaction doubles,what will be the value of the activation energy $(E_a)$?
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View SolutionFor the reaction $A \rightleftharpoons B$,if $E_a$ is the activation energy of the forward reaction,then the activation energy of the backward reaction is:
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