Chemical Kineti...

In the decomposition of oxalic acid following data were obtained.

For a reaction for which the activation energies of forward and reverse reactions are equal:

The rate constant for an isomerisation reaction, $$A\rightarrow B$$ is $$4.5\times 10^{-3} min ^{-1}$$. If the initial concentration of A is 1 M,  the rate of the reaction after 1 hr will be: 

The activation energy for a chemical reaction depends upon:

At room temperature, the reaction between $$NO$$ and $$O_2$$ to give $$NO_2$$ is fast, while that between $$CO$$ and $$O_2$$ is slow. It is due to:

For a first-order reaction, $$A\rightarrow Product$$, the initial concentration of A is 0.1M and after 40 minutes it becomes 0.025 M. Calculate the rate of reaction at reactant concentration of 0.01 M:

The maximum value of activation energy is equal to:

In a first order reaction the concentration of reactant decreases from 800 $$mol/dm^3$$ to $$50\ mol/dm^3$$ in $$2\times 10^4 sec$$. The rate constant of reaction in $$sec^{-1}$$ is:

Which of the following is not correct reason for the substantially lower rate of reaction than the collision frequency?