Ethylene obeys the truncated virial equation-of-state
\[
\frac{P V}{R T}=1+\frac{B P}{R T}
\]
where $P$ is the pressure, $V$ is the molar volume, $T$ is the absolute temperature and $B$ is the second virial coefficient. The universal gas constant $R=83.14 \mathrm{bar} \mathrm{cm}^{3} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$. At $340 \mathrm{~K}$, the slope of the compressibility factor vs. pressure curve is $-3.538 \times 10^{-3} \mathrm{bar}^{-1}$. Let $G^{R}$ denote the molar residual Gibbs free energy. At these conditions, the value of $\left(\frac{\partial G^{R}}{\partial P}\right)_{T}$, in $\mathrm{cm}^{3} \mathrm{~mol}^{-1}$, rounded off to $1$ decimal place, is $\_\_\_\_\_\_\_\_$