In a reaction, `2A rarr Products`, the concentration of A decreases from 0.5 mol L^(-1) to `0.4 molL^-1` in 10 minutes. Calculate the rate during this interval?

For a first order reaction, (A) rarr Products, the concentration of A changes from 0.1 M to 0.025 M in 40 minutes The rate of reaction when the concentration of A is 0.01 M is

For the reaction R rarr P , the concentration of a reactant changes from 0.03M to 0.02M in 25 minutes. Calculate the average rate of reaction using units of time both in minutes and seconds.

In a first order reaction, the concentration of the reactant decreases from 800 mol/ dm^3 to 50 mol/ dm^3 in 2 xx 10^4 sec. The rate constant of the reaction in sec^-1 is

In a first order reaction, the concentration of the reactant decreases from 0.6 M to 0.3 M in 30 minutes. The time taken for the concentration to change from 0.1 M to 0.025 M is

The reaction 2 N _(2) O _(5) (g) to NO _(2) (g) + O _(2) (g) takes place in a closed contaner. It is found that the concentration of NO _(2) increases by 1. 6 xx 10 ^(-2) mol L ^(-1) in four seconds . Calculate the rate of change of concentration of N _(2) O _(5).

The rate law for the reaction A+B to Product, is given by the expression k [A] [B] . If the concentration of B is increased from 0.1 to 0.3 mol/L, keeping the value of A at 0.1 mol/L, the rate constant will be:

The time for half life period of a certain reaction A rarr Products is 1 hour. When the initial concentration of the reactant ‘A’ is 2.0 mol L^-1 , how much time does it take for its concentration to come from 0.50 to 0.25 mol L^-1 ? if it is a zero order reaction?

For a first-order reaction, it takes 5 minutes for the initial concentration of 0.6 mol L^-1 to become 0.4 mol L^-1 . How long will it take for the initial concentration to become 0.3 mol L^-1 ?

Decomposition of H_2O_2 follows a first order reaction. In fifty minutes the concentration of H_2O_2 decreases from 0.5 to 0.125 M in one such decomposition. When the concentration of H_2O_2 reaches 0.05 M, the rate of formation of O_2 will be

The rate of formation of a dimer in a second order reaction is 9.5xx10^-5 mol L^-1 s^-1 at 0.01 mol L^-1 monomer concentration. Calculate the rate constant.