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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20. Electrochemistry
Cell Potential and Gibbs Free Energy
Back20. Electrochemistry
Cell Potential and Gibbs Free Energy
- Multiple ChoiceIn an electrochemical cell, if the Gibbs free energy change (ΔG) is positive, what can be said about the cell potential (E°cell)?1views
- Multiple ChoiceWhat values of the equilibrium constant (K) and Gibbs free energy change (ΔG) are expected for a large positive standard cell potential (E°cell)?
- Multiple ChoiceCalculate 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)1views
- Multiple ChoiceFor a large negative E°cell, what values of the equilibrium constant (K) and Gibbs free energy change (ΔG) are expected?
- 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
- 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?
- Multiple ChoiceWhat is ΔG° (in kJ/mol) for a redox reaction where two electrons are transferred with E°_cell = -0.273 V?
- Multiple ChoiceGiven 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.1views