(C) For an endothermic reaction,the relationship between activation energies and the enthalpy change is given by: $\Delta H = E_{a(f)} - E_{a(b)}$.Her

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(C) For an endothermic reaction,the relationship between activation energies and the enthalpy change is given by: $\Delta H = E_{a(f)} - E_{a(b)}$.Here,$\Delta H = 5 \ kcal/mol$ and $E_{a(f)} = 15 \ kcal/mol$.Substituting the values: $5 = 15 - E_{a(b)}$.Therefore,$E_{a(b)} = 15 - 5 = 10 \ kcal/mol$.

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

Medium

An endothermic reaction $A \to B$ has an activation energy of $15 \ kcal/mol$ and an enthalpy change of reaction of $5 \ kcal/mol$. The activation energy of the reverse reaction $B \to A$ is ......... $kcal/mol$.

A
$20$
B
$15$
C
$10$
D
None of these

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Chemical Kinetics

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Collision theory, Energy of activation and Arrhenius equation

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An endothermic reaction $A \to B$ has an activation energy of $15 \ kcal/mol$ and an enthalpy change of reaction of $5 \ kcal/mol$. The activation energy of the reverse reaction $B \to A$ is ......... $kcal/mol$.

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Oxygen is available in plenty in air,yet fuels do not burn by themselves at room temperature. Explain.

The rate constant is given by the equation $k = p Z e^{-E_a/RT}$. Which factor should register a decrease for the reaction to proceed more rapidly?

For the reaction $A \to B$,$K_1 = 10^8 \, e^{-6000/8.34T}$ and for the reaction $P \to Q$,$K_2 = 10^{10} \, e^{-8000/8.34T}$. At what temperature $T$ will $K_1 = K_2$ (in $K$)?

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The reaction: $Cr_{2}O_{3} + 2 Al \rightarrow Al_{2}O_{3} + 2 Cr$ $\quad (\Delta_{r}G^{\Theta} = -421 \ kJ)$ is thermodynamically feasible as is apparent from the Gibbs energy value. Why does it not take place at room temperature?

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