For a reaction `A+2B rarr C`, the rate law is, rate= `kxx[A]xx[B]^2`. If the rate constant of the reaction is `3.74xx10^(-2) M^(-2)s^(-1)`, calculate the rate of the reaction when the concentrations of A and B are 0.126 M and 0.142 M respectively.

The rate constant of a reaction is 2.1 xx 10^(-2) litre mol^(-1)s^(-1) . The order of reaction is

The rate law for the reaction A+B rarr C is found to be rate = k [A]^2 [B] . The rate constant of the reaction at 25^@C is 6.25 M^(-2)S^(-1) . What is the rate of reaction, When [A] = 0.1 mol.dm^(-3) and [B] = 0.2 mol.dm^(-3) ?

The rate constant of a certain first order reaction is 3.12xx10^(-3) min^(-1) What is the molarity of the reactant after 1.5 hours , If initial concentration is 0.045 M ?

For the reaction 2A + B rarr products, find the rate law from the following data What is the rate constant and order of the reaction?

For a reaction 2A +B rarr C+D , the active mass of B is kept constant but tht of A is tripled. The rate of reaction will

The rate law for the reaction C_2H_4Br_2+3I^- rarr C_2H_4+2Br^-+I_3^- is rate = k[C_2H_4Br_2] [I^-] . The rate of the reaction is found to be 1.1xx10^(-4)M//s when the concentrations of C_2H_4Br_2 and I^- are 0.12M and 0.18M respectively. Calculate the rate constant of the reaction.