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

The minimum energy a molecule should possess in order to enter into a fruitful collision is known as

For a reaction,the temperature increases from $10\,^\circ\text{C}$ to $50\,^\circ\text{C}$. The rate of the reaction will increase by a factor of ........

Which of the following options is incorrect?

The rate of a reaction decreased by $3.555$ times when the temperature was changed from $40^{\circ} C$ to $30^{\circ} C$. The activation energy of the reaction is.........$kJ \, mol^{-1}$.
[Take; $R = 8.314 \, J \, mol^{-1} \, K^{-1}$,$\ln(3.555) = 1.268$]

The rate constant,$k$ for a first order reaction,$C_2H_5I_{(g)} \rightarrow C_2H_{4(g)} + HI_{(g)}$ is $x \ s^{-1}$ at $600 \ K$ and $4x \ s^{-1}$ at $700 \ K$. The energy of activation of the reaction (in $kJ \ mol^{-1}$) is (in $.16$)

Vedclass Test Series

Exam Paper Generator

Online Exam Module