For the reaction A_( g ) → B_( g ), the value of the equilibrium constant at 300 K and 1 atm is equal to 100.0. The value of Δ_r G for the reaction…

For the reaction $\displaystyle \mathrm{A}_{(\mathrm{g})} \rightarrow \mathrm{B}_{(\mathrm{g})}$, the value of the equilibrium constant at $\displaystyle 300$ K and $\displaystyle 1$ atm is equal to $\displaystyle 100.0$ . The value of $\displaystyle \Delta_{\mathrm{r}} \mathrm{G}$ for the reaction at $\displaystyle 300$ K and $\displaystyle 1$ atm in $\displaystyle \mathrm{J} \mathrm{mol}^{-1}$ is $\displaystyle -x \mathrm{R}$, where $\displaystyle x$ is \_\_\_\_. (Rounded off to the nearest integer) $\displaystyle \left[\mathrm{R}=8.31 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right.$ and $\displaystyle \ln 10=2.3$ )