For the reaction, A+B to C, the following dara were obtained. In the first experiment, when the initial concentrations of both A and B are 0.1M the observed initial rate of formation of C is 1xx10^(-4)mol "lt"^(-1)minute^(-1). In second experiment when the initial concentrations of (A) and (B) are 0.1M and 0.3M, the initial rate is 9.0xx10^(-4) mol litre^(-1)minute^(-1). In the third experiment, when the initial concentrations of both A and B are 0.3M, the initial rate is 2.7xx10^(-3)mol litre^(-1) minute^(-1). (a) Write rate law for this reaction. (ii) Calculate the value of specific rate constant for this reaction.

For the reaction, A+B to C, the following dara were obtained. In the f

1.	For the reaction, A+B to C, the following dara were obtained. In the first experiment, when the initial concentrations of both A and B are 0.1M the observed initial rate of formation of C is 1xx10^(-4)mol "lt"^(-1)minute^(-1). In second experiment when the initial concentrations of (A) and (B) are 0.1M and 0.3M, the initial rate is 9.0xx10^(-4) mol litre^(-1)minute^(-1). In the third experiment, when the initial concentrations of both A and B are 0.3M, the initial rate is 2.7xx10^(-3)mol litre^(-1) minute^(-1). (a) Write rate law for this reaction. (ii) Calculate the value of specific rate constant for this reaction.
Answer» Solution :Let Rate `-k[A]^(x)[B]^(y)` `r_(1)=1xx10^(-4)=k(0.1)^(x)(0.1)^(y)` …………`(1)` `r_(2)=9xx10^(-4)=k(0.1)^(x)(0.3)^(y)`………..`(2)` `r_(3)=2.7xx10^(-3)=k(0.3)^(x)(0.3)^(y)`…………`(3)` By Eqs. `(1)` and `(2)`, `(r_(1))/(r_(2))=(1xx10^(-4))/(9xx10^(-4))=((1)/(3))^(y) :. y=1` By Eqs. `(2)` and `(3)` `(r_(2))/(r_(3))=(9xx10^(-4))/(27xx10^(-4))=((1)/(3))^(x) :. x=1` `:.` Rate `=k[A]^(1)[B]^(2)` ALSO, `1xx10^(-4)=k(0.1)^(1)(0.1)^(2)` `:. k=10^(-1)=0.1Lt^(2)MOL^(-1)min^(-1)`