For the electrochemical cell represented by Cr | Cr^{3+} || Li^+ | Li, E^ext{cell} = -2.63ext{ V}. This cell:

• A. will spontaneously convert chemical energy to electrical energy under standard conditions
• B. is a galvanic cell operating under standard conditions
• C. cannot produce electrical energy spontaneously under standard conditions
• D. has a positive cell potential, indicating a spontaneous reaction

Answer: (C)

Verified step by step guidance

1. Identify the given cell notation: Cr | Cr^{3+} || Li^{+} | Li, and the cell potential E^{\text{cell}} = -2.63 \text{ V}.
2. Recall that the sign of the cell potential (E^{\text{cell}}) indicates spontaneity: a positive E^{\text{cell}} means the reaction is spontaneous, while a negative E^{\text{cell}} means it is non-spontaneous under standard conditions.
3. Since E^{\text{cell}} is negative (-2.63 V), conclude that the cell cannot spontaneously convert chemical energy to electrical energy under standard conditions.
4. Understand that a galvanic cell operates spontaneously and has a positive cell potential; therefore, this cell is not a galvanic cell under standard conditions.
5. Summarize that the negative cell potential means the reaction is non-spontaneous, so the cell cannot produce electrical energy spontaneously, and the statement about a positive cell potential is incorrect.