For the reaction `A+B rarr C`. The following data were obtained. In the first experiment, when the initial concentrations of both `A` and `B` are `0.1 M`, the observed initial rate of formation of `C` is `1xx10^(-4) mol litre^(-1) minute^(-1)`. In the second experiment when the initial concentrations of `A` and `B` are `0.1 M` and `0.3 M`, the initial rate is `9.0xx10^(-4) mol liter^(-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.
(b) Calculate the value of specific rate constant for this reaction.

Explanation

To solve the problem step by step, we will first write the rate law for the reaction and then calculate the specific rate constant.

### Step 1: Write the Rate Law

The rate law for a reaction of the form \( A + B \rightarrow C \) can be expressed as:

\[
\text{Rate} = k [A]^m [B]^n
...