For a reversible reaction A rightleftharpoons | vedclass

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

Question

(C) From the given energy profile diagram:$E_a$ = activation energy of forward reaction$E_a^{\prime}$ = activation energy of backward reaction$E_t$ =

Vedclass · Accepted Answer

The threshold energy is less than that of activation energy

Vedclass · Answer

(C) From the given energy profile diagram:$E_a$ = activation energy of forward reaction$E_a^{\prime}$ = activation energy of backward reaction$E_t$ = threshold energy$1$. Since the energy level of product $B$ is higher than reactant $A$,the reaction is endothermic.$2$. The activation energy of the forward reaction $(E_a)$ is the difference between threshold energy $(E_t)$ and energy of reactant $(E_R)$.$3$. The activation energy of the backward reaction $(E_a^{\prime})$ is the difference between threshold energy $(E_t)$ and energy of product $(E_p)$.$4$. From the diagram,$E_a > E_a^{\prime}$.$5$. The relationship is $E_a = E_a^{\prime} + \Delta E$,where $\Delta E$ is the heat of reaction.$6$. The threshold energy $(E_t)$ is always greater than or equal to the activation energy ($E_a$ or $E_a^{\prime}$),as it represents the minimum energy required for the reaction to occur. Therefore,the statement that 'threshold energy is less than that of activation energy' is incorrect.

For a reversible reaction $A \rightleftharpoons B$,which one of the following statements is wrong from the given energy profile diagram?

Similar Questions

Consider the following graph of the kinetic energy distribution among molecules at temperature $T$. If the temperature is increased,how would the resulting graph differ from the one above?

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?

The activation energy for the reaction $X \rightarrow Y$ is $150 \text{ kJ mol}^{-1}$. The change in enthalpy for the above reaction is $-135 \text{ kJ mol}^{-1}$. What is the activation energy for the reverse reaction $Y \rightarrow X$?

Which of the following graphs of $\log \, K \rightarrow 1/T$ can be used to calculate the activation energy?

Vedclass Test Series

Exam Paper Generator

Online Exam Module