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

6. Chemical Quantities & Aqueous Reactions

Balancing Redox Reactions: Acidic Solutions

General Chemistry

6. Chemical Quantities & Aqueous Reactions

Balancing Redox Reactions: Acidic Solutions

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Multiple Choice

Which of the following is the correctly balanced redox reaction for Cr2O7^2-(aq) + I^-(aq) → Cr^3+(aq) + IO3^-(aq) in acidic solution?

Cr2O7^2- + 6I^- + 12H^+ → 2Cr^3+ + 3IO3^- + 6H2O

Cr2O7^2- + 6I^- + 8H^+ → 2Cr^3+ + 3IO3^- + 4H2O

Cr2O7^2- + 6I^- + 14H^+ → 2Cr^3+ + 6IO3^- + 7H2O

Cr2O7^2- + 6I^- + 10H^+ → 2Cr^3+ + 3IO3^- + 5H2O

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Verified step by step guidance

Identify the oxidation and reduction half-reactions. In this case, Cr2O7^2- is reduced to Cr^3+, and I^- is oxidized to IO3^-.

Balance the atoms in each half-reaction. For the reduction half-reaction, balance Cr atoms first, then balance oxygen atoms by adding H2O, and finally balance hydrogen atoms by adding H^+. For the oxidation half-reaction, balance iodine atoms first, then balance oxygen atoms by adding H2O, and finally balance hydrogen atoms by adding H^+.

Balance the charges in each half-reaction by adding electrons. For the reduction half-reaction, add electrons to the left side to balance the positive charge. For the oxidation half-reaction, add electrons to the right side to balance the negative charge.

Equalize the number of electrons transferred in both half-reactions by multiplying the half-reactions by appropriate coefficients.

Add the balanced half-reactions together, ensuring that electrons cancel out, and simplify the equation by combining like terms. Verify that the number of atoms and charges are balanced on both sides of the equation.