Question

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^-3

The 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 1

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.