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For a first-order reaction, the plot of k against 1/T is a straight line with a slope of -12028 K. The activation energy for the reaction is ____ kJ mol ⁻¹ . (Nearest integer) [Given: R = 8.314 J K ⁻¹ mol ⁻¹ ]

Correct answer

100

Step-by-step solution

The Arrhenius equation is given by: k = A e^ -E_a/RT Taking the natural logarithm on both sides: k = A - E_a RT Comparing this with the equation of a straight line y = mx + c , the slope m of the plot of k vs 1/T is: m = - E_a R Given that the slope is -12028 K: - E_a R = -12028 E_a = 12028 8.314 E_a = 100000.792 J mol ⁻¹ Converting to kJ mol ⁻¹ : E_a 100 kJ mol ⁻¹ Answer: 100

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