The reaction `F_2(g) + 2ClO_2(g)` is first order in each of the reactants. The rate of the reaction in each of the reactants. The rate of the reaction is `4.88xx10^(-4) M//s` when `[F_2] = 0.015M` and `[ClO_2] = 0.025 M`. Calculate the rate constant of the reaction.

The concentration of a reactant decreases from 0.2 M to 0.1 M in 10 minutes . The rate of the reaction is ______.

After how many seconds will the concentration of the reactant in a first order reaction be halved if the rate constant is 1.155xx10^(-3)s^(-1) ?

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-

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

Find the rate constant , at 298 K temperature of a chemical reaction with rate law, rate = k[X][Y]^2 . The rate of reaction is found to be 0.40 M//s and [X] = 0.6 M and [Y] = 0.39 M.

The rate of the reaction, A+B rarr P is 3.6xx10^(-2) mol dm^(-3) s^(-1) when [A] = 0.2 moles dm^(-3) and [B] = 0.1 moles dm^(-3) . Calculate the rate constant if the reaction is firsr order in A and second order in B.

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.

Consider the reaction 2A+2B rarr 2C +D . From the following data, calculate the order and rate constant of the reaction. Write the rate law of the reaction.