20. Electrochemistry

Cell Potential and Gibbs Free Energy

Multiple Choice
What is the gibbs free energy change for the given reaction at 25ºC?
Au³⁺ (aq) + 3 Li (s) →. Au (s) + 3 Li⁺ (aq)
Given the following reduction potentials:
Au³⁺(aq) + 3 e^– →. Au(s) E°_red = + 1.50 Volts
Li⁺ (aq) + e^– →. Li (s) E°_red = – 3.04 Volts
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Multiple Choice
The reduction of chlorate is given by the equation:
ClO₃^– (aq) + 6 H₃O⁺ (aq) → Cl ^– (aq) + 9 H₂O (l)
If the standard cell potential is given as 1.373 V, how many electrons are transferred under standard conditions?
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Multiple Choice
In an electrochemical cell, if the Gibbs free energy change (ΔG) is positive, what can be said about the cell potential (E°cell)?
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Multiple Choice
Calculate the maximum obtainable work in kJ for the balanced redox reaction below at 25 °C. Given: 3 MnO4–(aq) + 4 H+(aq) + 5 NO(g) --> 3 Mn2+(aq) + 2 H2O(l) + 5 NO3–(aq), E°cell = 0.540 V. (HINT: 1 V = 1 J/C)
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Multiple Choice
Calculate the equilibrium constant (K) for an oxidation-reduction reaction (n = 2) with a cell potential of -0.51 V at 298 K.
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Multiple Choice
Given the reaction and standard cell potentials: Ni(s) + 2Ag⁺ (aq) ⇌ Ni²⁺ (aq) + 2Ag(s), where E°_Ag⁺/Ag = +0.80 V and E°_Ni²⁺/Ni = -0.26 V, calculate the standard free energy change (ΔG°) and the equilibrium constant (K) at 25°C for the reaction.
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Multiple Choice
What is ΔG° (in kJ/mol) for a redox reaction where two electrons are transferred with E°_cell = -0.273 V?
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Multiple Choice
For a large negative E°cell, what values of the equilibrium constant (K) and Gibbs free energy change (ΔG) are expected?
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Multiple Choice
What values of the equilibrium constant (K) and Gibbs free energy change (ΔG) are expected for a large positive standard cell potential (E°cell)?
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