For an exothermic reaction,where the enthalpy | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(C) For any chemical reaction,the activation energy $(E_a)$ is the minimum energy required for the reactants to form the activated complex. In an exot

Vedclass · Accepted Answer

More than $\Delta H$

Vedclass · Answer

(C) For any chemical reaction,the activation energy $(E_a)$ is the minimum energy required for the reactants to form the activated complex. In an exothermic reaction,the energy of the products is lower than the energy of the reactants. The relationship between activation energy $(E_a)$,enthalpy of reaction $(\Delta H)$,and the activation energy of the reverse reaction $(E_{a,reverse})$ is given by: $E_a - E_{a,reverse} = \Delta H$. Since $E_{a,reverse}$ must always be a positive value,$E_a$ must be greater than $\Delta H$ (considering the magnitude of $\Delta H$ for an exothermic reaction). Therefore,the activation energy is always a positive value and is greater than the enthalpy change of the reaction.

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

Similar Questions

At $T \ K$,the following equation is obtained for a first order reaction: $\log \frac{k}{A} = -\frac{x}{T}$. The activation energy for this reaction is equal to $(R = \text{gas constant})$

For a first-order reaction,if the rate constant is $k_1$ at temperature $T_1$ and $k_2$ at temperature $T_2$,which of the following relations is correct? ($E_a$ = activation energy)

Which of the following plots is in accordance with the Arrhenius equation?

The rate constant of a reaction depends on

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

Vedclass Test Series

Exam Paper Generator

Online Exam Module