Textbook Question
(a) What is the definition of the volt?
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20. Electrochemistry
Intro to Electrochemical Cells
Multiple Choice
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
Verified step by step guidance1
Identify the given cell notation: Cr | Cr^{3+} || Li^{+} | Li, and the cell potential E^{\(\text{cell}\)} = -2.63 \(\text{ V}\).
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.
Since E^{\(\text{cell}\)} is negative (-2.63 V), conclude that the cell cannot spontaneously convert chemical energy to electrical energy under standard conditions.
Understand that a galvanic cell operates spontaneously and has a positive cell potential; therefore, this cell is not a galvanic cell under standard conditions.
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.
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