Under the same reaction conditions, initial concentration of 1 . 386 mol dm - 3 of a substance becomes half in 40 s and 20 s through first order and zero order kinetics, respectively. Ratio k 1 k 0 of the rate of constants for first order k 1 and zero order k 0 of the reaction is

Step-by-step solution

Given that, Under the same reaction conditions, initial concentration of 1 . 386   mol   dm - 3 of a substance becomes half in 40   s and 20   s for first order and zero order kinetics, respectively. For first order reaction, t 1 / 2 = ln 2 k 1 = 40   s . . . i For zero order reaction, t 1 / 2 = A 0 2 k 0 = 20   s . . . . ii Divide eqn. (i) by (ii), we get 1 2 = [ A ] 0 2 k 0 × k 1 ln 2 k 1 k 0 = ln 2 [ A ] 0 = 0 . 693 1 . 386 = 0 . 5   mol - 1 dm 3