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

The rate law for elementary reaction A+2B to C +2D will be _.

Rate law for the reaction A + B to product is rate =K [A]^(2) [B]. What is the rate constant if the rate of the reaction at a given temperature is 0.22Ms^(-1) , when [A]=1 M and [B]=0.25 M?

Rate law for the reaction, 2 NO + Cl_2 rarr 2 NOCI is rate = k[NO]^2[Cl_2] . Thus of k would increase with

Write the rate law for the reaction, A+B rarrP from the following data:

Rate law for the reaction A + 2B rarrC is found to be 1 Rate =k [A][B] Concentration of reactant B is doubled,keeping the concentration of ‘A' constant, the value of rate constant will be

The rate of the first order reaction A rarr products, is 0.01 M sr1, when reactant concentration is 0.2 M. The rate constant for the reaction is-

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.