A galvanic cell converts :
Answer & explanation
Correct answer: option 2
The correct answer is Option (2) → Chemical energy to electrical energy
Electrochemical cells are of two kinds. In a galvanic (voltaic) cell a spontaneous redox reaction produces electricity: the Gibbs energy of the reaction is converted into electrical work. In an electrolytic cell electrical energy from outside drives a non-spontaneous reaction.
The Daniell cell is a galvanic cell:
\( \displaystyle \ce{Zn(s) + Cu^2+(aq) -> Zn^2+(aq) + Cu(s)} \qquad E^{\circ}_{\mathrm{cell}} = 1.1\ \mathrm{V} \)
So a galvanic cell converts chemical energy into electrical energy.
Why the other options are incorrect
Option (1) Electrical energy to chemical energy — Incorrect. This is what happens in an electrolytic cell (and in a secondary battery while it is being charged).
Option (3) Light energy to electrical energy — Incorrect. This is a photovoltaic (solar) cell; no redox reaction is used.
Option (4) Electrical energy to light energy — Incorrect. This is what a bulb or an LED does, not an electrochemical cell.
NCERT (2026-27 edition):
Galvanic Cells – “As mentioned earlier a galvanic cell is an electrochemical cell that converts the chemical energy of a spontaneous redox reaction into electrical energy. In this device the Gibbs energy of the spontaneous redox reaction is converted into electrical work which may be used for running a motor or other electrical gadgets like heater, fan, geyser, etc.”