For the following reaction : $K=1.7\times {10}^7$  at ${25}^{0}C$

$A{g}_{\left(aq\right)}^{+}+2N{H}_{3\left(aq\right)}\rightleftharpoons {\left[Ag{\left(N{H}_3\right)}_2\right]}^{\oplus }$  then $\Delta G^0$  in $KJ$  is

$\Delta G^0=-2.303RT\log K_c$

$=-2.303\times 8.314\times {10}^{-3}\times 298\times \log \left(1.7\times {10}^7\right)KJ/mole$

$=-2.030\times 8.314\times 0.298\times 7.2304KJ/mole$

$=-41.25KJ/mole$