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 Applications

General Chemistry

7. Gases

The Ideal Gas Law Applications

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Multiple Choice

Using the Ideal Gas Law, what is the pressure exerted by a 75.0 g sample of dinitrogen monoxide (N2O) gas in a 4.21 L vessel at 298 K?

1.50 atm

1.02 atm

0.85 atm

0.65 atm

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Verified step by step guidance

First, identify the variables given in the problem: the mass of N2O is 75.0 g, the volume of the vessel is 4.21 L, and the temperature is 298 K. We need to find the pressure exerted by the gas.

Convert the mass of N2O to moles using its molar mass. The molar mass of N2O is calculated by adding the atomic masses of nitrogen (14.01 g/mol) and oxygen (16.00 g/mol): Molar mass of N2O = 2(14.01) + 16.00 g/mol.

Use the Ideal Gas Law equation: \( PV = nRT \), 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.

Rearrange the Ideal Gas Law equation to solve for pressure (P): \( P = \frac{nRT}{V} \).

Substitute the values for n (moles of N2O), R (0.0821 L·atm/mol·K), T (298 K), and V (4.21 L) into the equation to calculate the pressure exerted by the gas.