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

Standard Reduction Potentials

General Chemistry

20. Electrochemistry

Standard Reduction Potentials

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Multiple Choice

Use the table of standard reduction potentials to calculate the equilibrium constant at standard temperature (25 °C) for the reaction: Fe(s) + Ni²⁺(aq) → Fe²⁺(aq) + Ni(s). Which of the following is the correct equilibrium constant (K)?

K = 1.0 x 10^1

K = 1.0 x 10^3

K = 1.0 x 10^2

K = 1.0 x 10^5

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Verified step by step guidance

Identify the half-reactions involved in the given redox reaction. The oxidation half-reaction is Fe(s) → Fe²⁺(aq) + 2e⁻, and the reduction half-reaction is Ni²⁺(aq) + 2e⁻ → Ni(s).

Look up the standard reduction potentials (E°) for each half-reaction from the table of standard reduction potentials. The standard reduction potential for Ni²⁺(aq) + 2e⁻ → Ni(s) is typically given, as well as for Fe²⁺(aq) + 2e⁻ → Fe(s).

Calculate the standard cell potential (E°cell) using the formula: E°cell = E°(reduction) - E°(oxidation). Substitute the values from the table to find E°cell.

Use the Nernst equation to relate the standard cell potential to the equilibrium constant (K). The equation is: ln(K) = (nF * E°cell) / (RT), where n is the number of moles of electrons transferred, F is Faraday's constant (96485 C/mol), R is the universal gas constant (8.314 J/mol·K), and T is the temperature in Kelvin (298 K for standard conditions).

Solve for K by rearranging the Nernst equation to K = e^((nF * E°cell) / (RT)). Calculate the exponent using the values for n, F, E°cell, R, and T, and then find K by taking the exponential of the result.