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)

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

Tardigrade Admin · Accepted Answer

4=e(Ea/R) (1/300)-(1/310) In(4)=(Ea/R) (10/300×310) Ea=(0.693× 2× 8.314× 300× 310/10) =107165.79 J =107.165 KJ

Q. 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; $l n 2 = 0.693; R = 8.314 J$ $m o l^{- 1} K^{- 1}$ )

$107.2 k J m o l^{- 1}$

$53.6 k J m o l^{- 1}$

$26.8 k J m o l^{- 1}$

$214.4 k J m o l^{- 1}$

$4 = e^{\frac{E a}{R} {\frac{1}{300} - \frac{1}{310}}}$

In $(4) = \frac{E a}{R} {\frac{10}{300 \times 310}}$

$E a = \frac{0.693 \times 2 \times 8.314 \times 300 \times 310}{10}$

$= 107165.79 J = 107.165 K J$

Q. The rate of a reaction quadruples when the temperature changes from 300 to 310K. The activation energy of this reaction is : (Assume activation energy and pre-exponential factor are independent of temperature; ln2=0.693;R=8.314J mol−1K−1)

107.2kJmol−1

53.6kJmol−1

26.8kJmol−1

214.4kJmol−1