For the reaction `2A+B to A, B,` the rate `=K[A] [B]^(2)` with `k= 2.0x 10^(-6)v 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).`

Explanation

i) Case I:
Rate `=k [A][B]^(2)`
`=[2.0xx10^(-6)mol ^(-2)L^(-2) s^(-1)]xx(0.1 mol L ^(-1))xx (0.2 mol L ^(-1)) ^(2)`
`=8.0 xx10^(-9) mol L^(-1)s^(-1).`
ii) Case II:
Concentratio of A at A at a prticular time `=0.06 mol L ^(-1)`
Amount of A reacted `=(0.1 -0.06)=0.04 mol L^(-1)`
Amount of B raacted `=1/2 xx0.04 mol L^(-1) =0.02 mol L^(-1)`
Concentration of B at a particular time `=[0.2 -0.02] mol L^(-1) =0.18 mol L^(-1)`
Rate `= [A][B]^(2)`
`=[2.0xx10^(-6)mol ^(-2)L^(-2) s^(-1)]xx(0.1 mol L ^(-1))xx (0.2 mol L ^(-1)) ^(2)`
`=8.0 xx10^(-9) mol L^(-1)s^(-1).`