Answer:- Under standard state conditions, the electrical work done in a galvanic cell can be expressed as: \[\Delta G^\circ = -nF E^\circ_{\text{cell}}\] where: - \(\Delta G^\circ\) is an extensive property because its value depends on the amount of substance. - \(n\) is the number of moles of electrons transferred. - \(F\) is the Faraday constant. - \(E^\circ_{\text{cell}}\) is the standard cell potential. If the stoichiometric equation of the redox reaction is multiplied by 2, meaning that the number of substances oxidized and reduced is doubled, both \(\Delta G^\circ\) and the moles of electrons transferred (\(n\)) also double. The ratio, \[E^\circ_{\text{cell}} = -\frac{\Delta G^\circ}{nF}\] then becomes, \[E^\circ_{\text{cell}} = -\frac{2\Delta G^\circ}{2nF} = \frac{\Delta G^\circ}{nF}\] Thus, \(E^\circ_{\text{cell}}\) remains the same when multiplying the redox reaction by 2. This implies that \(E^\circ_{\text{cell}}\) is independent of the amount of substance and is considered an intensive property.