For a reation: `A rarr` Product,
rate law is `-(d[A])/(dt)=K[A]_(0)`.
The concentration of `A` left after time `t` when `t=1/K` is:

For a reaction 2A + B rarr product, rate law is -(d[A])/(dt)=k[A] . At a time when t=(1)/(k) , concentration of the reactant is " (C_(0)="initial concentration")

The reaction A+OH^(-)rarr Products, obeys rate law expression as : (-d[A])/(dt)=k[A][OH^(-\)] If initial concentrations of [A] and [OH^(-)] are 0.02 M and 0.3 M respectively and if it takes 30 sec for 1% A to react at 25^(@)C , caclutate the rate constant for the reaction

Consider a certain reaction A rarr Products with k=2.0 xx 10^(-2) S^(-1) Calculate the concentration of A remaining after 100 s if the initial concentration of A is 1.0 mol L^(-1) .

For a first order reaction -(d[A])/(dt)=K[A]_(0) . The reaction is carried out by taking 100 mol//litre of A, then concentration of A decayed after time 1/K is:

Calculate the rate of reaction from rate law -d[A]//dt = K [A ][B ]^ (2) when the concentration of A and B are 0.01M and 0.02M respectively and K = 5.1×10^(-3) lit^(2) mol ^(- 2)s^(-1) .