Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

20. Electrochemistry

Cell Potential: The Nernst Equation

General Chemistry

20. Electrochemistry

Cell Potential: The Nernst Equation

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Multiple Choice

Using the Nernst equation, what is the concentration of Ag+ in the cathode half-cell if the cell potential is measured to be 0.70 V?

0.10 mol L^(-1)

0.001 mol L^(-1)

0.01 mol L^(-1)

1.0 mol L^(-1)

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Verified step by step guidance

Identify the half-reaction for the cathode. For silver, the reduction half-reaction is: Ag^+ + e^- → Ag.

Write the Nernst equation for the cell: E = E° - (RT/nF) * ln(Q), where E is the cell potential, E° is the standard cell potential, R is the gas constant, T is the temperature in Kelvin, n is the number of moles of electrons transferred, F is Faraday's constant, and Q is the reaction quotient.

Determine the standard cell potential (E°) for the Ag^+/Ag half-reaction. This value can be found in standard reduction potential tables.

Calculate the reaction quotient (Q), which for the half-reaction Ag^+ + e^- → Ag is [Ag^+]. Rearrange the Nernst equation to solve for [Ag^+]: [Ag^+] = exp((nF(E° - E))/(RT)).

Substitute the known values into the rearranged Nernst equation: E = 0.70 V, n = 1 (since one electron is transferred), and solve for [Ag^+].