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

7. Gases

Partial Pressure

General Chemistry

7. Gases

Partial Pressure

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Multiple Choice

A gas mixture contains 72.8% chlorine and 27.2% neon by mass. What is the partial pressure of neon in the mixture if the total pressure is recorded as 809 mmHg?

260 mmHg

289 mmHg

320 mmHg

392 mmHg

459 mmHg

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Verified step by step guidance

Step 1: Begin by understanding Dalton's Law of Partial Pressures, which states that the total pressure of a gas mixture is the sum of the partial pressures of each individual gas in the mixture.

Step 2: Calculate the mass of each gas in the mixture using the given percentages. Assume a total mass of 100 grams for simplicity. This means you have 72.8 grams of chlorine and 27.2 grams of neon.

Step 3: Convert the mass of each gas to moles using their molar masses. The molar mass of chlorine (Cl₂) is approximately 70.9 g/mol, and the molar mass of neon (Ne) is approximately 20.18 g/mol. Use the formula: \( \text{moles} = \frac{\text{mass}}{\text{molar mass}} \).

Step 4: Determine the mole fraction of neon in the mixture. The mole fraction is calculated using the formula: \( \text{mole fraction of Ne} = \frac{\text{moles of Ne}}{\text{total moles of gases}} \).

Step 5: Calculate the partial pressure of neon using its mole fraction and the total pressure. Use the formula: \( P_{\text{Ne}} = \text{mole fraction of Ne} \times \text{total pressure} \).