According to the Arrhenius equation,which of | vedclass

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

Question

(B) The Arrhenius equation is given by $K = Ae^{-\frac{E_a}{RT}}$.Statement $(A)$ is incorrect because a high activation energy $(E_a)$ implies a slow

Vedclass · Accepted Answer

$B, C, D$

Vedclass · Answer

(B) The Arrhenius equation is given by $K = Ae^{-\frac{E_a}{RT}}$.Statement $(A)$ is incorrect because a high activation energy $(E_a)$ implies a slow reaction,not a fast one.Statement $(B)$ is correct because as temperature $(T)$ increases,the fraction of molecules with energy greater than $E_a$ increases,leading to more effective collisions.Statement $(C)$ is correct because the term $e^{-\frac{E_a}{RT}}$ shows that the sensitivity of $K$ to temperature changes increases as $E_a$ increases.Statement $(D)$ is correct because the pre-exponential factor $(A)$ represents the frequency of collisions,which is independent of the energy threshold.Therefore,the correct statements are $(B)$,$(C)$,and $(D)$.

Similar Questions

Activation energy of any reaction depends on

For $N_2 + 3H_2 \rightarrow 2NH_3$,$\Delta H = -22 \ kcal$,and $E_a = 70 \ kcal$. Hence $E_a$ for $2NH_3 \rightarrow N_2 + 3H_2$ is $.....$ $kcal$.

$A$ reaction has an activation energy of $209 \, kJ \, mol^{-1}$. The rate increases $10$-fold when the temperature is increased from $27^{\circ} C$ to $X^{\circ} C$. The temperature $X$ is closest to
[Gas constant,$R = 8.314 \, J \, mol^{-1} \, K^{-1}$ ]

For a first order reaction,the rate constant is $0.04 \, \text{min}^{-1}$ at $27 \, ^\circ\text{C}$ and $0.08 \, \text{min}^{-1}$ at $37 \, ^\circ\text{C}.$ The activation energy of reaction is .......... $\text{kcal} / \text{mol}$ $(\ln \, 2 = 0.7)$

Vedclass Test Series

Exam Paper Generator

Online Exam Module