(a) What is the maximum electrical work obtainable from the reaction | 0,(g) + H,(g) = H,O(1) %3D under standard conditions (25°C and 1 atm pressure and specified amounts of reactants)? (b) What is the heat transferred if this maximum work is obtained? The standard free energy change for the reaction, AG°, is -237.18 kJ mol-'. The standard enthalpy change, AH°, is -285.85 kJ mol.

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Example 2.2
(a) What is the maximum electrical work obtainable from the reaction
| 02(g) + H,(g)
H2O(1)
%3D
under standard conditions (25°C and 1 atm pressure and specified
amounts of reactants)?
(b) What is the heat transferred if this maximum work is obtained?
The standard free energy change for the reaction, AG°, is -237.18 kJ mol.
The standard enthalpy change, AH°, is -285.85 kJ mol.
(a) According to equation 30, the maximum electrical work available under
reversible conditions (i.e., when T A,S = 0) is w' = -.
kJ mol'. (Two electrons are transferred per mole of the reaction. There-
fore the standard potential difference for the electrochemical reaction
is: -(-237,180) J/2 x 96,485 J/V =
AG° = 237.18
1.23 V.)
- 285.85 + 237.18
(b) The heat transferred is
-48.67 kJ mol-1. The system releases heat to the surroundings, but
much less than under irreversible conditions for this reaction.
AH° + w' =
(Note that here the system is the electrochemical reaction plus the external
electric circuit required to reversibly extract the free energy released.)
Transcribed Image Text:Example 2.2 (a) What is the maximum electrical work obtainable from the reaction | 02(g) + H,(g) H2O(1) %3D under standard conditions (25°C and 1 atm pressure and specified amounts of reactants)? (b) What is the heat transferred if this maximum work is obtained? The standard free energy change for the reaction, AG°, is -237.18 kJ mol. The standard enthalpy change, AH°, is -285.85 kJ mol. (a) According to equation 30, the maximum electrical work available under reversible conditions (i.e., when T A,S = 0) is w' = -. kJ mol'. (Two electrons are transferred per mole of the reaction. There- fore the standard potential difference for the electrochemical reaction is: -(-237,180) J/2 x 96,485 J/V = AG° = 237.18 1.23 V.) - 285.85 + 237.18 (b) The heat transferred is -48.67 kJ mol-1. The system releases heat to the surroundings, but much less than under irreversible conditions for this reaction. AH° + w' = (Note that here the system is the electrochemical reaction plus the external electric circuit required to reversibly extract the free energy released.)
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