Statement I: If standard reduction potential for the reaction \(Ag^+ + e^− \rightarrow Ag\) is 0.80 V. Then for the reaction \(2Ag^+ + 2e^− \rightarrow 2Ag\), it will be 1.60 V

Statement II:  If the concentration of Ag+ ions is doubled, the electrode potential will not be doubled

Statement I is false but Statement II is correct

The answer is 4. Statement I is false but Statement II is correct.

Statement I: If standard reduction potential for the reaction \(Ag^+ + e^− \rightarrow Ag\) is 0.80 V. Then for the reaction \(2Ag^+ + 2e^− \rightarrow 2Ag\), it will be 1.60 V.

This is false. The standard reduction potential for a reaction is the potential difference between the electrode where the reduction reaction occurs and a standard hydrogen electrode. The standard reduction potential for a reaction does not depend on the stoichiometry of the reaction.

In the reaction \(2Ag^+ + 2e^− \rightarrow 2Ag\), the standard reduction potential is still 0.80 V. This is because the same number of electrons are transferred in both reactions.

Statement II: If the concentration of Ag⁺ ions is doubled, the electrode potential will not be doubled

This is true. The Nernst equation describes the relationship between the electrode potential and the concentration of the ions in the solution. The Nernst equation shows that the electrode potential is proportional to the logarithm of the concentration of the ions in the solution. If the concentration of the ions is doubled, the electrode potential will increase by a factor of 0.3010.