What is change in free energy for an electrolytic cell?

ΔG > 0

The correct answer is option 1. ΔG > 0.

In an electrolytic cell, the process is non-spontaneous, meaning energy is required to drive the reaction forward. This is in contrast to a galvanic cell, where the process is spontaneous and energy is released. The relationship between the change in free energy (\(\Delta G\)) and the cell potential (\(E\)) is given by:

\(\Delta G = -nFE\)

Where:

\(n\) is the number of moles of electrons transferred in the reaction,

\(F\) is Faraday's constant (\( 96485 \, \text{C/mol} \)),

\(E\) is the cell potential (in volts).

For an electrolytic cell, where \(E\) is typically negative (since the reaction is non-spontaneous), \(\Delta G\) will be positive. This is because the negative value of \(E\) causes \(\Delta G\) to be positive, indicating that energy is required for the reaction to occur.

Therefore, the correct answer is: \( \Delta G > 0 \)