Question

The rate of a reaction quadruples when the temperature changes from $300$ to $310\, K$. The activation energy of this reaction is : (Assume activation energy and pre-exponential factor are independent of temperature; $ln\, 2 = 0.693; R=8.314 \,J$ $mol^{-1} \, K^{-1}$)

• A. $107.2 \, kJ \, mol^{-1}$
• B. $53.6 \, kJ \, mol^{-1}$
• C. $26.8 \, kJ \, mol^{-1}$
• D. $214.4 \, kJ \, mol^{-1}$

Answer 1

Answer: (A)

$107.2 \, kJ \, mol^{-1}$

Answer 2

4=e^{\frac{Ea}{R}\left\\{\frac{1}{300}-\frac{1}{310}\right\\}} In\left(4\right)=\frac{Ea}{R}\left\\{\frac{10}{300\times310}\right\\} $Ea=\frac{0.693\times 2\times 8.314\times 300\times 310}{10}$ $=107165.79 \,J =107.165\, KJ$