The activation energy of a reaction is 155326 J/ mol. The rate constant of the reaction at and 300K as a function of rate constant at 400K, obtained by the Collision theory is ____(a) k1 = 1.5 × 10^-7k2(b) k1 = 1.2 × 10^-6 k2(c) k1 = 1.5 × 10^-6 k2(d) k1 = 1.2 × 10^-7 k2This question was addressed to me at a job interview.I need to ask this question from Kinetics of Homogeneous Reactions in section Kinetics of Homogeneous Reactions of Chemical Reaction Engineering

The activation energy of a reaction is 155326 J/ mol. The rate constan

1.	The activation energy of a reaction is 155326 J/ mol. The rate constant of the reaction at and 300K as a function of rate constant at 400K, obtained by the Collision theory is ____(a) k1 = 1.5 × 10^-7k2(b) k1 = 1.2 × 10^-6 k2(c) k1 = 1.5 × 10^-6 k2(d) k1 = 1.2 × 10^-7 k2This question was addressed to me at a job interview.I need to ask this question from Kinetics of Homogeneous Reactions in section Kinetics of Homogeneous Reactions of Chemical Reaction Engineering
Answer» Right choice is (a) K1 = 1.5 × 10^-7k2 The explanation: By COLLISION THEORY, ln(\(\frac{k_2}{k_1}) = -\frac{E}{R} (\frac{1}{T_2} – \frac{1}{T_1}) + 0.5ln(\frac{T_2}{T_1}) \) ln(\(\frac{k_2}{k_1}) = -\frac{155326}{8.314}(\frac{1}{400} – \frac{1}{300}) + 0.5ln(\frac{400}{300}) \) Hence, k1 = 1.5 × 10^-7k2.

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