For the reaction, `2A + B+C rarr A_(2)B+C`
The rate `= k[A][B]^(2)` with `K = 2.0 xx 10^(-6) M^(-2) s^(-1)`. Calculate the initial rate of the reaction when `[A] = 0.1M, [B] = 0.2M` and `[C] = 0.8M`. IF the rate of reverse reaction is negligible then calculate the rate of reaction after `[A]` is reduced to `0.06M`.

For the reaction : 2A+B rarr A_(2)B the rate =k[A][B]^(2) with k=2.0xx10^(-6)mol^(-2)L^(2)s^(-1) . Calculate the initial rate of the reaction when [A]=0.1 mol L^(c-),[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 to A_(2)B , the reaction rate = k[A][B]^(2) with k = 2.0 xx 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) . Also calculate the reaction rate when [a] is reduced to 0.06 mol L^(-1) .

For the following reaction: 2A + B +C rarr A_(2)B + C The rate law has been determined to be Rate = k[A][B]^(2) with k = 2.0 xx 10^(-6) mol^(-2) L^(2) s^(-1) For this reaction, determine the initial rate of the reaction with [A] = 0.1 mol L^(-1), [B] = 0.2 mol L^(-1), C = 0.8 mo, L^(-1) . Determine the rate after 0.04 mol L^(-1) of A has reacted.

For the reaction : 2A + B to A_2B , the rate = K[A][B]^2 with K = 2.0 xx 10^(-6) mol^(-1) lit^(2) sec^(-1) . Initial concentration of A and B are 0.2 mol/lt and 0.4 mol/lit respectively. Calculate the rate of reaction after [A] is reduced to 0.12 mol/lit

In the reaction, A + 2B to 6C + 2D , if the initial rate -(d[A])/(dt) at t = 0 is 2.6 xx 10^(-2) m sec^(-1) , what will be the value of -(d[B])/(dt)" at " t = 0 ?