MHT CET 202621 AprilEvening Shift
- Exam
- MHT CET
- Year
- 2026
- Date
- 21 April
- Shift
- Evening Shift
- Subject
- Chemistry
- Chapter
- Electrochemistry
MHT CET 2026 · 21 April · Evening Shift · Chemistry · Electrochemistry
Calculate the standard Gibbs energy for the following cell...
Calculate the standard Gibbs energy for the following cell reaction,
, if E^{}^{\circ}_{cell} is .
, if E^{}^{\circ}_{cell} is .
Options
- A
- B
- C
- D
Correct answer
D.
Step-by-step solution
The given cell reaction is .
The number of electrons transferred in the reaction is .
The standard Gibbs free energy change is given by the equation:
\Delta G^{}^{\circ} = -n F E^{}^{\circ}_{cell}
Substituting the given values ( and E^{}^{\circ}_{cell} = 0.556\ \text{V}):
\Delta G^{}^{\circ} = -2 \times 96500 \times 0.556
\Delta G^{}^{\circ} = -107308\ \text{J mol}^{-1}
\Delta G^{}^{\circ} \approx -107.31\ \text{kJ mol}^{-1}
Answer:
The number of electrons transferred in the reaction is .
The standard Gibbs free energy change is given by the equation:
\Delta G^{}^{\circ} = -n F E^{}^{\circ}_{cell}
Substituting the given values ( and E^{}^{\circ}_{cell} = 0.556\ \text{V}):
\Delta G^{}^{\circ} = -2 \times 96500 \times 0.556
\Delta G^{}^{\circ} = -107308\ \text{J mol}^{-1}
\Delta G^{}^{\circ} \approx -107.31\ \text{kJ mol}^{-1}
Answer: