Consider a certain reaction A `rarr` Products with k=2.0 xx 10^(-2)`S^(-1)` Calculate the concentration of A remaining after 100 s if the initial concentration of A is 1.0 mol L^(-1)`.

For a first order reaction, k = 2.5xx10^-4 s^-1 , what is the rate of reaction, when the initial concentration of the reactant is 0.1 mol L^-1 ?

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

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?

The rate constant of the reaction A rarr B is 0.6 xx10^-3 mole per second. If the concentration of A is 5 M, then concentration of B after 20 minutes is:

For the reaction: 2A + B rarr A2B the rate = k[A][B]^2 with k = 2.0 × 10^(-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) .

Consider the reaction, 2A + B rarr Products When concentration of B alone was doubled, the half-life did not change. When the concentration of A alone was doubled, the rate increased by two times. The units of rate constant for this reaction are -

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, 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 ?

The rate of a first order reaction is : 1.5 xx 10^-2 mol L^-1 mi n^-1 at 0.5 M concentration of the reactant. The half life of the reaction is :