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

The Ideal Gas Law: Density

General Chemistry

7. Gases

The Ideal Gas Law: Density

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Multiple Choice

Using the Ideal Gas Law, calculate the density of CO2 gas in g/L at 27°C and 0.50 atm pressure.

1.14 g/L

0.98 g/L

1.25 g/L

0.89 g/L

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Verified step by step guidance

Convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature: T(K) = 27 + 273.15.

Use the Ideal Gas Law in the form \( PV = nRT \) to find the molar volume. Rearrange it to \( V = \frac{nRT}{P} \), where \( R \) is the ideal gas constant (0.0821 L·atm/mol·K).

Calculate the molar mass of CO2. The molar mass of carbon (C) is 12.01 g/mol and oxygen (O) is 16.00 g/mol. Therefore, the molar mass of CO2 is \( 12.01 + 2 \times 16.00 \) g/mol.

Substitute the values into the rearranged Ideal Gas Law to find the volume of one mole of CO2 at the given conditions: \( V = \frac{(1 \text{ mol}) \times (0.0821 \text{ L·atm/mol·K}) \times T(K)}{0.50 \text{ atm}} \).

Calculate the density using the formula \( \text{Density} = \frac{\text{Molar Mass}}{\text{Molar Volume}} \). Substitute the molar mass of CO2 and the calculated molar volume to find the density in g/L.