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

In the following reaction identify the oxidizing agent and the reducing agent:
Cr₂O₇^2- + 6 Fe²⁺ + 14 H⁺→ 2 Cr³⁺ + 6 Fe³⁺ + 7 H₂O

Oxidizing Agent:Fe, Reducing Agent:H

Oxidizing Agent:Fe, Reducing Agent:Cr

Oxidizing Agent:Cr, Reducing Agent:Fe

Oxidizing Agent:H, Reducing Agent:Fe

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Verified step by step guidance

Understand the concept of oxidation and reduction: Oxidation involves the loss of electrons, while reduction involves the gain of electrons. An oxidizing agent is a substance that gains electrons and is reduced, whereas a reducing agent is a substance that loses electrons and is oxidized.

Examine the oxidation states of the elements involved in the reaction. For example, in the dichromate ion \( \text{Cr}_2\text{O}_7^{2-} \), chromium typically has an oxidation state of +6. In \( \text{Cr}^{3+} \), chromium has an oxidation state of +3.

Determine the change in oxidation states for each element. Chromium goes from +6 in \( \text{Cr}_2\text{O}_7^{2-} \) to +3 in \( \text{Cr}^{3+} \), indicating a reduction. Iron goes from +2 in \( \text{Fe}^{2+} \) to +3 in \( \text{Fe}^{3+} \), indicating oxidation.

Identify the oxidizing and reducing agents based on the changes in oxidation states. The substance that is reduced (gains electrons) is the oxidizing agent, and the substance that is oxidized (loses electrons) is the reducing agent.

Conclude that in this reaction, \( \text{Cr}_2\text{O}_7^{2-} \) is the oxidizing agent because it is reduced to \( \text{Cr}^{3+} \), and \( \text{Fe}^{2+} \) is the reducing agent because it is oxidized to \( \text{Fe}^{3+} \).