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

Electrolytic Cell

General Chemistry

20. Electrochemistry

Electrolytic Cell

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Multiple Choice

How many faradays of electricity are required to liberate 9g of aluminum in an electrolytic cell, given that the molar mass of aluminum is 27 g/mol?

1 faraday

3 faradays

2 faradays

4 faradays

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Verified step by step guidance

First, determine the number of moles of aluminum that correspond to 9 grams. Use the formula: \( \text{moles of Al} = \frac{\text{mass of Al}}{\text{molar mass of Al}} \). Given that the mass of aluminum is 9 g and the molar mass is 27 g/mol, calculate \( \text{moles of Al} = \frac{9}{27} \).

Next, consider the balanced chemical equation for the reduction of aluminum ions in an electrolytic cell: \( \text{Al}^{3+} + 3e^- \rightarrow \text{Al} \). This indicates that 3 moles of electrons are required to produce 1 mole of aluminum.

Calculate the total moles of electrons needed to produce the moles of aluminum calculated in step 1. Multiply the moles of aluminum by 3 (since 3 moles of electrons are needed per mole of aluminum): \( \text{moles of electrons} = \text{moles of Al} \times 3 \).

Recall that 1 faraday is equivalent to 1 mole of electrons. Therefore, the number of faradays required is equal to the number of moles of electrons calculated in step 3.

Finally, compare the calculated number of faradays to the options provided (1, 2, 3, or 4 faradays) to determine which is correct based on your calculations.