Consider the following single step reaction in gas phase at constant temperature. 2 A_( g ) + B_( g ) → C_( g ) The initial rate of the reaction is…

Consider the following single step reaction in gas phase at constant temperature. $$2 \mathrm{~A}_{(\mathrm{g})}+\mathrm{B}_{(\mathrm{g})} \rightarrow \mathrm{C}_{(\mathrm{g})} $$ The initial rate of the reaction is recorded as $\displaystyle \mathrm{r}_1$ when the reaction starts with $\displaystyle 1.5$ atm pressure of A and $\displaystyle 0.7$ atm pressure of B . After some time, the rate $\displaystyle \mathrm{r}_2$ is recorded when the pressure of C becomes $\displaystyle 0.5$ atm . The ratio $\displaystyle \mathrm{r}_1: \mathrm{r}_2$ is $\displaystyle \_\_\_\_$ $\displaystyle \times 10^{-1}$. (Nearest integer)