The activation energy of a reaction is 50 kJ mol^-1 and the value of rate constant at 300 K is 2.5×10^-5 sec^-1. What is the value of the frequency factor, A?(a) 4228.53 s^-1(b) 3829.69 s^-1(c) 7596.45 s^-1(d) 6565.35 s^-1I had been asked this question in unit test.I want to ask this question from Chemical Kinetics in division Chemical Kinetics of Chemistry – Class 12

The activation energy of a reaction is 50 kJ mol^-1 and the value of r

1.	The activation energy of a reaction is 50 kJ mol^-1 and the value of rate constant at 300 K is 2.5×10^-5 sec^-1. What is the value of the frequency factor, A?(a) 4228.53 s^-1(b) 3829.69 s^-1(c) 7596.45 s^-1(d) 6565.35 s^-1I had been asked this question in unit test.I want to ask this question from Chemical Kinetics in division Chemical Kinetics of Chemistry – Class 12
Answer» The correct choice is (C) 7596.45 s^-1 Explanation: Given, EA = 50 kJ mol^-1 T = 300 K k = 1.5 × 10^-5 sec^-1 R = 8.314 J K^-1 mol^-1 log k = – Ea / (2.303 RT) + log A OR log A = log k + Ea / (2.303 RT) log A = log (1.5 × 10^-5) + 50000 / (2.303 × 8.314 × 300) log A = 3.88061 A = antilog (3.880611) A = 7596.45 s^-1.

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