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Ch.13 - Fundamentals of ElectrochemistryWorksheetSee all chapters

# Nernst Equation

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Sections
Basic Concepts
Electrochemical Cells
Standard Potentials
Nernst Equation
Standard Cell Potential & the Equilibrium Constant
###### Nernst Equation

Concept #1: The Nernst Equation reveals the quantitative connection between the concentrations of compounds and cell potential.

###### Nernst Equation Calculations

Example #1: Determine the cell potentials of the following concentration cells:

Ag | Ag+ (aq, 0.0010 M) || Cu2+ (aq, 1.0 M) | Cu

EAnode = 0.799 V         ECathode = 0.339 V

Example #2: Consider the following electrochemical cell for the question:

Pt  |  KBr(aq, 0.01 M), Br2(l)  ||  FeBr2(aq, 1.0M)  |  Fe

EAnode = 1.078 V         ECathode = - 0.440 V

Determine the spontaneity and cell potential based on the given cell notation.

Example #3: Consider a standard voltaic cell based on the reaction:

2 H+ (aq) + Sn (s) ⇌ Sn2+ (aq) + H2 (g)

Which of the following actions would change the emf of the cell?

a) Increasing the pH at the cathode

b) Lowering the pH at the cathode

c) Increasing [Sn2+] at the anode

d) Increasing the hydrogen gas pressure at the cathode

e) All of the above changes will alter the cell potential

Example #4: Consider the following half cell reaction at T = 25. °C

Ni2+(aq) + 2 e –    Ni(s)      E° = – 0.260 V

What will be the value for E°, the half cell potential for standard conditions, for the reaction

2 Ni(s)    2 Ni2+ (aq) + 4 e

a) + 0.52 V          b) + 0.26 V          c) – 0.26 V          d) – 0.52 V