The rate of reaction, A + B → P is 3.6 x 10 mol dm s when [A] = 0.2 mol dm and [B] = 0.1 mol dm. Calculate the Rate constant if the reaction is first order in A and second order in B.

The rate of the first order Ararr Products, is 7.5xx0^(-4) "mol" L^(-1)s^(-1) , when the concentration of A is 0.2 mol L^(-1) . The rate constant of the reaction is :

(a)In an experiment at 1000 K , the concentrations of different species are : [NH_3] = 0.105 mol dm^(-3), [N_2] =1.10 mol dm^(-3) and [H_2] =1.50 mol dm^(-3) Calculate the values of K_c and K_p for the reaction : N_2+3H_2 hArr 2NH_3 (b) What will be the K_c for the reaction : 2NH_3 hArr N_2+3H_2

In a first order reaction the concentration of the reactant is reduced from 0.6 "mol" L^(-1) to 0.2 "mol" L^(-1) in 5 minutes the rate constant of the reaction is

Pseudo first order rate for the reaction A + B rarr P when studied in 0.1 M of B is given by -(d[A])/(dt) = -k[A] where k = 1.85 xx 10^(4)s^(-1) . Calculate the value of second order rate constant.

In a first order reaction the concentration of reactant decreases from 800 mol/ dm^3 to 50 mol/dm3 in 2xx 10^4 s . The rate constant of reaction in s^(–1) is

The rate law equation for a reaction A rarr B is , r = k[A]^(0) If the initial concentration is 'a' mol "dm"^(-3) , the half of the reaction is

The rate first order reaction is 2.4 xx 10^(-3) mol L^(-1) s^(-1) , when the initial concentration is 0.2 mol L^(-1) . The rate constant is…………. .