For the reaction: $2A + B → A_2B$ the rate = k[A][B] 2 with k= 2.0 x 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 .

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The initial rate of the reaction is Rate = k [A][B] 2 Rate = (2.0 × 10 -6 mol -2 L 2 s -1 ) (0.1 mol L -1 ) (0.2 mol L -1 ) 2 Rate = 8.0 × 10 -9 mol -2 L 2 s -1 When [A] is reduced from 0.1 mol L -1 to 0.06 mol -1 , the concentration of A reacted = (0.1 - 0.06) mol L -1 = 0.04 mol L -1 Therefore, concentration of B reacted =  $\frac 12$  x 0.04 mol L -1 Then, concentration of B available, [B] = (0.2 - 0.02) mol L -1 [B]  = 0.18 mol L -1 After [A] is reduced to 0.06 mol L -1 , the rate of the reaction is given by Rate = k [A][B] 2 Rate = (2.0 × 10 -6 mol -2 L 2 s -1 ) (0.06 mol L -1 ) (0.18 mol L -1 ) 2 Rate = 3.89 mol L -1 s -1

For the reaction:
\(2A + B → A_2B\)
the rate = k[A][B]² with k= 2.0 x 10^-6 mol^-2L²s^-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.

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For the reaction:\(2A + B → A_2B\)the rate = k[A][B]2 with k= 2.0 x 10-6 mol-2L2s-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.