For a certain reaction the values of Arrhenius factor and Activation energy are 4 x 10^13 collision/sec and 98.6KJ/mol at 303K. Calculate the rate constant if reaction is 1^st order?( R=8.341mol^-1K^-1)(a) 6.07 x 10^-3(b) 3.02 x 10^-5(c) 4.07 x 10^-4(d) 7.42 x 10^-3The question was posed to me by my college professor while I was bunking the class.I would like to ask this question from Chemical Kinetics topic in division Chemical Kinetics of Chemistry – Class 12

For a certain reaction the values of Arrhenius factor and Activation e

1.	For a certain reaction the values of Arrhenius factor and Activation energy are 4 x 10^13 collision/sec and 98.6KJ/mol at 303K. Calculate the rate constant if reaction is 1^st order?( R=8.341mol^-1K^-1)(a) 6.07 x 10^-3(b) 3.02 x 10^-5(c) 4.07 x 10^-4(d) 7.42 x 10^-3The question was posed to me by my college professor while I was bunking the class.I would like to ask this question from Chemical Kinetics topic in division Chemical Kinetics of Chemistry – Class 12
Answer» Right ANSWER is (c) 4.07 x 10^-4 Easy EXPLANATION: Given, Arrhenius factor(A) = 4 x 10^13 collisions/sec Activation energy (Ea)=98.6KJ/mol=98.6 x 10^3J/mol, T=303 K log K = log A – (Ea/2.303RT) log K = log (4 x 10^13) – (98.6 x 10^3)/(2.303 x 8.314 x 303) log K = 13.6020 – (98.6 x 10^3/5801.584) log k = -3.39 K = 10^-3.39 K = 4.07 x 10^-4.

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