Consider a certain reaction `A rarr Products` with `k = 2.0x10^-2 s^-1.Calculate the concentration of A after 100s if the initial concentration of A is 1.0 mol L^-1.

For the reaction: 2A + B rarr A_2B the rate = k[A][B]^2 with k = 2.0xx10^-6 mol^-2 L^2 s^-1 . Calculate the initial rate of the reaction when [A] = 0.1 mol L^-1 , [b] = 0.2 mol L^-1 . Calculate the rate of reaction after [A] is reduced to 0.06 mol L^-1 .

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

A reaction is second order with respect to a reacant. How is the rate of reaction affected if the concentration of the reactant is reduced to 1/2?

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 of a reaction is 1.2xx10^-3 L mol^-1 s^-1 . What is the order of the reaction?

For a chemical reaction variation in concentraction, ln[R] vs. time (min) plot is shown below : If initial concentration of the reactant is half of the original concentration, how will t_(1//2) change?

If NaCl is doped with 10^-3 mol % of SrCl_2 , what is the concentration of cation vacancies?

In the reaction A + 2B rarr 3C + 2D , the rate of diappearance of B is 1xx10^-2 mol L^-1s^-1 . What will be the rate of the reaction and rate of change of concentration of A and C?