For two reactions : R-I and R-II the rate constants at 300 K and 320 K are 0.1 sec1 and 0.3 sec1 respectively (for R-I) and 0.2 sec1 and 0.8 sec1 (for R-II}. Which of the options regarding activation energy is correct?

see full answer

High-Paying Jobs That Even AI Can’t Replace — Through JEE/NEET

🎯 Hear from the experts why preparing for JEE/NEET today sets you up for future-proof, high-income careers tomorrow.

An Intiative by Sri Chaitanya

Activation energies for both the reactions is same.

Activation energy for second reaction is $\frac{4}{3}$ times as that of first reaction.

Activation energy for first reaction is more.

Activation energy for second reaction is more.

answer is C.

(Unlock A.I Detailed Solution for FREE)

JEE

NEET

Foundation JEE

Foundation NEET

CBSE

Detailed Solution

$\ln (\frac{k_{2}}{k_{1}}) = \frac{E_{a}}{R} [\frac{1}{T_{1}} - \frac{1}{T_{2}}]$

$\frac{\ln (\frac{k_{2}}{k_{1}})}{\ln (\frac{k_{2}^{'}}{k_{1}^{'}})} = \frac{E_{a}}{E_{a}^{'}}$

$\Rightarrow E_{a}^{'} > E_{a}$

So, we can says that Activation energy for second reaction is more.

Watch 3-min video & get full concept clarity

Ready to Test Your Skills?

Check your Performance Today with our Free Mock Test used by Toppers!

Take Free Test