(Solved): The equilibrium constant for the equation Ag+(aq)+2NH3(aq)Ag(NH3)2+(aq) is K=2.5 ...

The equilibrium constant for the equation ${\mathrm{Ag}}^{+}(\mathrm{aq})+2{\mathrm{NH}}_3(\mathrm{aq})?{?\mathrm{Ag}{\left({\mathrm{NH}}_3\right)}_2?}^{+}(\mathrm{aq})$ is $K=2.5\times 10^3$ at $25.0^{?}\mathrm{C}$. Calculate the value of $?G_{\mathrm{rin}}^{?}$ at $25.0^{?}\mathrm{C}$. $?G_{\text{tin }}^{+}=\mathrm{kJ}/\mathrm{mol}$ Is the reaction spontaneous under standard conditions? Calculate the value of $?G_{\mathrm{rnn}}$ at $25.0^{?}\mathrm{C}$ when $?{\mathrm{Ag}}^{†}?=0.00387\mathrm{M},[{\mathrm{NH}}_3?=0.521\mathrm{M}$, and $\left[{?{\mathrm{Ag}}^{?}{\left({\mathrm{NH}}_3\right)}_2?}^{†}\right]=0.00930\mathrm{M}$. $?G_{\mathrm{nn}}=\mathrm{kJ}/\mathrm{mol}$ Is the reaction spontancous under these conditions? yes no