For a gaseous reaction 2A+B_(2)to2AB, the following rate data were obtained at 300 K {:("Rate of disappearance of "B_(2),,,"""Concentration",,,),("(""mol lit"^(-1)"min"^(-1)")",,,[A],,,[B_(2)]),((i)1.8xx10^(-3),,,0.015,,,0.15),((ii)1.08xx10^(-2),,,0.09,,,0.15),((iii)5.4xx10^(-3),,,0.015,,,0.45):} Calculate the rate constant for the reaction and rate of formation of AB when [A] is 0.02 and [B_(2)] is 0.04 "mol lit"^(-1)" at 300 K".

For a gaseous reaction 2A+B_(2)to2AB, the following rate data were obt

1.	For a gaseous reaction 2A+B_(2)to2AB, the following rate data were obtained at 300 K {:("Rate of disappearance of "B_(2),,,"""Concentration",,,),("(""mol lit"^(-1)"min"^(-1)")",,,[A],,,[B_(2)]),((i)1.8xx10^(-3),,,0.015,,,0.15),((ii)1.08xx10^(-2),,,0.09,,,0.15),((iii)5.4xx10^(-3),,,0.015,,,0.45):} Calculate the rate constant for the reaction and rate of formation of AB when [A] is 0.02 and [B_(2)] is 0.04 "mol lit"^(-1)" at 300 K".
Answer» Solution :From (i) and (II), when `[B_(2)]` is KEPT constant and [A] is made 6 times, the rate also six times. Thous, Rate `prop[A].` Further, from (i) and (iii), when [A] is kept constant and `[B_(2)]` is made three times, rale also becomes three times. Thus, Rate `prop[B_(2)]`. Hence, rate `=k[A][B_(2)].` PUT the values of [A] and `[B_(2)]` and calculate k. It comes out to be 0.8 LITRE `"mol"^(-1)min^(-1)`. When [A] = 0.02 M and `B_(2)=0.04" M",` Rate of formation of `AB=2xx" Rate of disappearance of "B_(2)`