JEE Main 2017 · 9 Apr · Shift 1 · Chemistry Q39

ChemistrySingle correct+4 / -1Question 39 of 90

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 $^{-1}$ )

107.2 kJ mol

^{-1}

53.6 kJ mol

^{-1}

26.8 kJ mol

^{-1}

214.4 kJ mol

^{-1}

Answer and worked solution

Official answer: A

$\ln4=\frac{E_a}R\left(\frac1{300}-\frac1{310}\right)\implies E_a=\frac{1.386\times8.314\times300\times310}{10}\approx107.2\text{ kJ mol}^{-1}.$

JEE Main 2017 · 9 Apr · Shift 1, Chemistry question 39