The rate of a reaction : `2A +B rarr A_2B` has the rate law : rate =`k[A]^2` with rate constant equal to 0.50 `mol L^-1 s^-1` . Calculate the rate of the reaction When [A] = 0.60 `mol L^-1` [B] = 0.05 `mol L^-1`

The rate of a reaction 2A+B rarr A_2B . has rate law : rate = k [A]^2 with the rate constant equal to 0.50 mol^(-1)" L sec"^(-1) . Calculate the rate of reaction when (i) [A] = 0.60 mol L^(-1) , [B] =-0.05 mol L^(-1) and (ii) When concentration of A and B have been reduced to 1/4 th

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) .

The rate of a reaction A to B has the rate law, rate = k [A] with the rate constant, = k = 0. 50 sec ^(-1) Q. What concentration of A would give a rate of 2. 4 xx 10 ^(-2) mol L ^(-1) sec ^(-1)?

The rate of a reaction is 1.209 xx10^-4L^2 mol^-2 s^-1 . The order of the reaction is :

For the reaction 2 A+B+C rarr A_2B+C The rate law has been found to be Rate = k[A] [B]^2 with k = 2.0 xx10^-6 mol^-2 L^2 s^-1 For this reaction, determine the initial rate of reaction with [A] = 0.1 mol L^-1, [B] = 0.2 mol L^-1, [C] = 0.8 mol L^-1 . Determine the rate after 0.04 mol L^-1 of A has been reacted.

The decomposition of hydrogen peroxide in the presence of iodide ion has been found to be first order with respect to H_2O_2 with rate constant k is 1.01 xx 10^(-2) min^(-1) . Calculate the rate of reaction when [H_2O_2] = 0.15 mol L^(-1)