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)`.

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 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 an elementary reaction : 2A + B rarr 3C the rate of appearance of C at time ‘t’ is 1.3 xx 10^(-4) mol l^(-1)s^(-1) . Calculate at this time : rate of disappearance of A.

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) .

Rate constant k=2.303 min^(-1) for a particular reaction. The initial concentration of the reactant is 1 mol // litre then rate of reaction after 1 minute is: