One mole of an ideal gas at $300 \mathrm{K}$ in thermal contact with its surroundings expands isothermally from $1.0 \mathrm{L}$ to $2.0 \mathrm{L}$ against a constant pressure of $3.0 \mathrm{atm}$. In this process, the change in entropy of the surroundings $\left(∆{\mathrm{S}}_{\mathrm{s}\mathrm{u}\mathrm{r}\mathrm{r}}\right)$ in $\mathrm{J}\mathrm{ }{\mathrm{K}}^{-1}$ is:
$\left(1 \mathrm{L} \mathrm{atm} = 101.3 \mathrm{J}\right)$