Consider a certain reaction `ArarrProducts` with `k=2.0 xx 10^(-2) (s)^(-1)` .Calculate the concentration of A remaining after 100s if the initial concentration of `A` is 1.0 `molL^(-1)`

The time for half-life period of a certain reaction A rarr Products is 1 h. When the initial concentration of the reactant A, is 2.0 mol L^(-1) . How much time does it take for its concentration to come from 0.50 mol L^(-1) to 0.25 mol L^(-1) , if it is a zero-order reaction?

The rate constant of a reaction at 298 K is given by 3.2xx10^(-3)s^(-1) .Find the order of reaction?

The rate law expression of a reaction 2A+B rarr A_(2)B is rate = k[A][B]^(2) with rate constant k =0.65 mol^(-1) L s^(-1) calculate rate of reaction when concentration of A has been reduced to 1//4 and concentration of B has been reduced by 1//4