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

Pressure Units

General Chemistry

7. Gases

Pressure Units

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Multiple Choice

What is the pressure of a 75.0 g sample of N2O in a 4.12 L vessel at 25°C, assuming ideal gas behavior?

3.67 atm

0.98 atm

1.12 atm

2.45 atm

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Verified step by step guidance

First, convert the mass of N2O to moles. Use the molar mass of N2O, which is approximately 44.01 g/mol. The formula to convert grams to moles is: \( \text{moles} = \frac{\text{mass}}{\text{molar mass}} \).

Next, use the Ideal Gas Law to find the pressure. The Ideal Gas Law is given by \( PV = nRT \), where \( P \) is the pressure, \( V \) is the volume, \( n \) is the number of moles, \( R \) is the ideal gas constant (0.0821 L·atm/mol·K), and \( T \) is the temperature in Kelvin.

Convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature. So, \( T = 25 + 273.15 \).

Rearrange the Ideal Gas Law to solve for pressure: \( P = \frac{nRT}{V} \). Substitute the values for \( n \), \( R \), \( T \), and \( V \) into the equation.

Calculate the pressure using the rearranged equation. Ensure all units are consistent, particularly the volume in liters and the temperature in Kelvin.