(a) We’re being asked to determine the standard cell potential (E°cell) of the reaction occurring in an electrochemical cell. To calculate for the standard cell potential, use the following equation:
Determine the anode and cathode by comparing their E° values.
• ↓ E° → oxidation → anode
• ↑ E° → reduction → cathode
Nickel and aluminum electrodes are used to build a galvanic cell. The standard reduction potential for the nickel(II) ion is -0.26 V and that of the aluminum(III) ion is -1.66 V.
a. What is the theoretical cell potential assuming standard conditions?
b. Which metal is the cathode?
c. Which statement is true?
- Electrons flow from Ni to Al.
- Electrons flow from Al to Ni.
- The nickel electrode loses mass.
- The aluminum electrode gains mass.
d. Type the shorthand notation for this cell. Do not include concentrations.
For example, in shorthand notation your answer might look like Cu|Cu + | |Pd2+|Pd
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