At $300\,\mathrm{K}$, a certain reaction has an equilibrium constant equal to 10. The value of $\Delta G^\circ$ for this reaction (in $\mathrm{kJ\,mol^{-1}}$) is:}
\[
(R=8.314\,\mathrm{J\,K^{-1}mol^{-1}})
\]
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Remember:
\[
\Delta G^\circ=-RT\ln K.
\]
If $K>1$, then $\Delta G^\circ$ is negative.