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

3. Chemical Reactions

Stoichiometry

General Chemistry

3. Chemical Reactions

Stoichiometry

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Multiple Choice

The volume of HCl gas required to react with excess Mg metal to produce 6.82 L of hydrogen gas at 2.19 atm and 35°C is ________ L. 2 HCl (g) + Mg (s) → MgCl2 (s) + H2 (g)

27.28 L

13.64 L

6.82 L

3.41 L

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Verified step by step guidance

Identify the balanced chemical equation: 2 HCl (g) + Mg (s) → MgCl2 (s) + H2 (g). This tells us that 2 moles of HCl produce 1 mole of H2.

Use the ideal gas law to find the number of moles of hydrogen gas produced. The ideal gas law is given by:

P V = n R T

, where P is pressure, V is volume, n is moles, R is the ideal gas constant, and T is temperature in Kelvin.

Convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature:

T =35+273.15

Rearrange the ideal gas law to solve for n (moles of H2):

n = \frac{P}{V} / R T

. Substitute the known values: P = 2.19 atm, V = 6.82 L, R = 0.0821 L atm/mol K, and T in Kelvin.

Use the stoichiometry from the balanced equation to find the moles of HCl needed. Since 2 moles of HCl produce 1 mole of H2, multiply the moles of H2 by 2 to find the moles of HCl. Then, use the ideal gas law again to find the volume of HCl gas required at the same conditions.