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The standard reduction potentials of the Fe3+/Fe2+ and Fe2+/Fe couples are 0.77 and –0.44 V, respectively. The standard reduction potential (in V) for the Fe3+/Fe couple is _______
Correct answer is '-0.03'. Can you explain this answer?
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The standard reduction potentials of the Fe3+/Fe2+ and Fe2+/Fe couples...
Given information:
- Standard reduction potentials of Fe3 /Fe2 and Fe2 /Fe couples are 0.77 and 0.44 V, respectively.
To find:
- Standard reduction potential for the Fe3 /Fe couple.
Solution:
The standard reduction potential for a half-reaction is defined as the potential difference between the standard hydrogen electrode (SHE) and the electrode in question, when both are in their standard states and the electron transfer occurs under standard conditions (298 K, 1 atm pressure, and 1 M concentration).
The half-reactions for the Fe3 /Fe2 and Fe2 /Fe couples are as follows:
Fe3+ + e- → Fe2+ E° = 0.77 V
Fe2+ + 2e- → Fe(s) E° = 0.44 V
To find the standard reduction potential for the Fe3 /Fe couple, we need to use the Nernst equation:
E = E° - (RT/nF) ln Q
Where,
- E is the cell potential under non-standard conditions
- E° is the standard reduction potential
- R is the gas constant (8.314 J/mol K)
- T is the temperature in Kelvin
- n is the number of electrons transferred in the half-reaction
- F is the Faraday constant (96,485 C/mol)
- Q is the reaction quotient
For the Fe3 /Fe2 half-reaction, the number of electrons transferred is 1. Therefore, we can use the Nernst equation as follows:
E = 0.77 - (8.314 x 298/1 x 96485) ln ([Fe2+]/[Fe3+])
At equilibrium, [Fe2+]/[Fe3+] = 10^(E°/0.0592)
Substituting the given values, we get:
E = 0.77 - (8.314 x 298/1 x 96485) ln (10^(0.77/0.0592))
E = -0.03 V
Therefore, the standard reduction potential for the Fe3 /Fe couple is -0.03 V.
Conclusion:
The standard reduction potential for the Fe3 /Fe couple is -0.03 V.
- Standard reduction potentials of Fe3 /Fe2 and Fe2 /Fe couples are 0.77 and 0.44 V, respectively.
To find:
- Standard reduction potential for the Fe3 /Fe couple.
Solution:
The standard reduction potential for a half-reaction is defined as the potential difference between the standard hydrogen electrode (SHE) and the electrode in question, when both are in their standard states and the electron transfer occurs under standard conditions (298 K, 1 atm pressure, and 1 M concentration).
The half-reactions for the Fe3 /Fe2 and Fe2 /Fe couples are as follows:
Fe3+ + e- → Fe2+ E° = 0.77 V
Fe2+ + 2e- → Fe(s) E° = 0.44 V
To find the standard reduction potential for the Fe3 /Fe couple, we need to use the Nernst equation:
E = E° - (RT/nF) ln Q
Where,
- E is the cell potential under non-standard conditions
- E° is the standard reduction potential
- R is the gas constant (8.314 J/mol K)
- T is the temperature in Kelvin
- n is the number of electrons transferred in the half-reaction
- F is the Faraday constant (96,485 C/mol)
- Q is the reaction quotient
For the Fe3 /Fe2 half-reaction, the number of electrons transferred is 1. Therefore, we can use the Nernst equation as follows:
E = 0.77 - (8.314 x 298/1 x 96485) ln ([Fe2+]/[Fe3+])
At equilibrium, [Fe2+]/[Fe3+] = 10^(E°/0.0592)
Substituting the given values, we get:
E = 0.77 - (8.314 x 298/1 x 96485) ln (10^(0.77/0.0592))
E = -0.03 V
Therefore, the standard reduction potential for the Fe3 /Fe couple is -0.03 V.
Conclusion:
The standard reduction potential for the Fe3 /Fe couple is -0.03 V.
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