Statement I: A negative value of standard reduction potential means that reduction takes place on this electrode with reference to standard hydrogen electrode

Statement II: The standard electrode potential of a half-cell has fixed value

Statement I is false but Statement II is correct

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

Statement I is false. A negative value of standard reduction potential (\(E^\circ\)) does not necessarily mean that reduction takes place on this electrode with reference to the standard hydrogen electrode (SHE). The sign of the standard reduction potential only indicates the direction of the reaction concerning SHE. If the \(E^\circ\) value is positive, the half-cell reaction has a greater tendency to undergo reduction compared to the standard hydrogen electrode (SHE). If the \(E^\circ\) value is negative, it means the half-cell reaction has a greater tendency to undergo oxidation (lose electrons) compared to SHE.

Statement II is correct. The standard electrode potential (\(E^\circ\)) of a half-cell is indeed a fixed value under standard conditions (specified temperature, pressure, and ion concentrations). It is an intrinsic property of the half-cell reaction and represents the tendency of the reaction to undergo reduction (positive \(E^\circ\)) or oxidation (negative \(E^\circ\)).

In summary, Statement I is false because a negative \(E^\circ\) value indicates a greater tendency for the half-cell reaction to undergo oxidation, not reduction. However, Statement II is correct, as the standard electrode potential of a half-cell is indeed a fixed value under specific conditions.