(Solved): Calculate the standard reaction free energy \( \left(\Delta G^{0}\right) \) for the following unba ...

Calculate the standard reaction free energy \( \left(\Delta G^{0}\right) \) for the following unbalanced redox reaction in acidic conditions. (HINT: You need to balance) \[ \mathrm{NO}(\mathrm{g})+\mathrm{Cu}^{2+}(\mathrm{aq}) \rightarrow \mathrm{HNO}_{2}(\mathrm{aq})+\mathrm{Cu}^{+}(\mathrm{aq}) \] The potential for the oxidation of \( \mathrm{NO}(\mathrm{g}) \) to \( \mathrm{HNO}_{2}(\mathrm{aq}) \) is \( -0.983 \mathrm{~V} \). The potential for the reduction of \( \mathrm{Cu}^{2+}(\mathrm{aq}) \) to \( \mathrm{Cu}^{+}(\mathrm{aq}) \) is \( 0.153 \mathrm{~V} \). The standard cell potential \( \left(E_{\text {cell }}^{0}\right) \) for the reaction above is V. There are of electrons transferred during this reaction. The standard reaction free energy \( \left(\Delta \mathrm{G}^{0}\right) \) for this redox reaction is kJ. This redox reaction at \( 25^{\circ} \mathrm{C} \).