For the reaction : 2A + B → A 2 B the Rate = k[A][B] 2 with k = 2.0 × 10 -6 mol -2 L 2 sec -1 . Calculate the initial rate of the reaction when [A] = 0.1 mol L -1 and [B] = 0.2 mol L -1 . Calculate the rate of reaction after [A] is reduced to 0.06 mol L -1 .

Question

Philoid · Accepted Answer

a) Rate = k[A][B]², Rate = 2.0 × 10^-6[0.1][0.2]²

Rate = 8 × 10^-9 mol L^-1sec^-1

b)

Situation when A is remained 0.06 mol L^-1

Now, According to rate law, Rate = k[A][B]²

Rate = 2 × 10^-6[0.06][0.18]²

i.e. Rate = 3.888 × 10^-9 mol L^-1sec^-1

Initial rate of reaction is 8 × 10^-9 mol L^-1sec^-1. and rate when concentration of A is 0.06 mol L^-1 is 3.888 × 10^-9 mol L^-1sec^-1.

For the reaction :2A + B → A2Bthe Rate = k[A][B]2 with k = 2.0 × 10-6 mol-2 L2 sec-1. Calculate the initial rate of the reaction when [A] = 0.1 mol L-1 and [B] = 0.2 mol L-1. Calculate the rate of reaction after [A] is reduced to 0.06 mol L-1.

For the reaction :
2A + B → A₂B

the Rate = k[A][B]² with k = 2.0 × 10^-6 mol^-2 L² sec^-1. Calculate the initial rate of the reaction when [A] = 0.1 mol L^-1 and [B] = 0.2 mol L^-1. Calculate the rate of reaction after [A] is reduced to 0.06 mol L^-1.