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Sahay Sir > Question Answers > JEE Adv and Mains Chemistry 41 Years Solved Video Solutions 1979 - 2019 > Chemistry > Chapter 17 - Chemical Kinetics > Two reactions R1 and R2 have identical pre-exponential factors. Activation energy of R1 exceeds that of R2 by 10 kJ mol^–1. If k1 and k2 are rate constants for reactions R1 and R2 respectively at 300 K, then ln(k2/k1) is equal to- (R = 8.314 J mol^–1K^–1)

Two reactions R1 and R2 have identical pre-exponential factors. Activation energy of R1 exceeds that of R2 by 10 kJ mol^–1. If k1 and k2 are rate constants for reactions R1 and R2 respectively at 300 K, then ln(k2/k1) is equal to- (R = 8.314 J mol^–1K^–1)

A2 k1⇔k-1 2A For an elementary chemical reaction the expression for d[A]/dt is.