Given below is an expression for the rate constant of a first order reaction occurring at a certain temperature, T (K). k = 14.34 - 1.25 10^ 4 T The energy of activation in kcal mol^ -1 for the reaction is : (Given : k in s^ -1 , R = 1.987 cal mol^ -1 K^ -1 )
A. 24.84
The Arrhenius equation is given by: k = A - E_a RT The given equation is: k = 14.34 - 1.25 10^ 4 T Comparing the two equations: E_a R = 1.25 10^ 4 E_a = 1.25 10^ 4 R Substituting R = 1.987 cal mol^ -1 K^ -1 : E_a = 1.25 10^ 4 1.987 E_a = 24837.5 cal mol^ -1 E_a = 24.8375 kcal mol^ -1 24.84 kcal mol^ -1 Answer: 24.84
Related: Chemistry — Chemical Kinetics · All PYQ Banks