The rate constant of a reaction at 500K and 700K are `0.01s^-1` and `0.07s^-1` respectively. Calculate the value of activation energy for the reaction `(R = 8.314 JK^-1mol^-1).

The rate constants of a reaction at 500K and 700K are 0.02s^-1 and 0.07s^-1 respectively. Calculate value of activation energy for the reaction. (Given R = 8.314 JK^-1 mol^-1)

The rate constant of reaction is 1.5xx10^7s^-1 at 50^@C and 4.5xx10^7s^-1 at 100^@C . Calculate the value of activation energy for the energy for the reaction (R = 8.314 Jk^-1 mol^-1)

For a decomposition reaction, the values of rate constants at two different temperatures are given below: K_1 = 2.15xx10^-8 Lmol^-1s^-1 at 650k K_2 = 2.39xx10^-7 Lmol^-1s^-1 at 700k Calculate the value of activation energy for the reaction (R = 8.314 JK^-1 mol^-1 )

The rate constant of a reaction is 3xx10^2 min^-1 . What is the order of the reaction?

In a reaction 2A rarr P the Conc of A decreases from 0.5molL^(-1) to 0.4molL^(-1) in 10 sec. Calculate the rate of the reaction.

The rate constant for a chemical reaction at a given temperature is 2.3xx10^(-5)Lmol^(-1)s^(-1) . What is the order of the reaction

In general it is observed that the rate of a chemical reaction doubles with every 10^@ rise in temperature. If the generalisation holds for a reaction in the temperature range 295K to 305K, what would be the value of activation energy for the reaction?

Calculate the half-life of a first order reaction from their rate constants value as 200 s^-1

In a first order reaction, the concentration of the reactant is reduced from 0.6moll^(-1) to 0.2moll^(-1) in 5 minutes. Calculate the rate constant of the reaction.

The rate of reaction triples when temperature change from 20^@C to 50^@C . Calculate the energy of activation. (R = 8.314 Jmol^-1K^-1)