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

General Chemistry

7. Gases

The Ideal Gas Law

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Multiple Choice

How many liters of HNO₃ gas, measured at 28.0 ºC and 780 torr, are required to prepare 2.30 L of 4.15 M solution of nitric acid?

56 L

62 L

189 L

230 L

262 L

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Verified step by step guidance

First, calculate the number of moles of HNO3 needed using the molarity formula: \( M = \frac{n}{V} \), where \( M \) is the molarity, \( n \) is the number of moles, and \( V \) is the volume in liters. Rearrange to find \( n = M \times V \). Substitute \( M = 4.15 \text{ M} \) and \( V = 2.30 \text{ L} \) to find \( n \).

Next, use the ideal gas law to find the volume of HNO3 gas required. The ideal gas law is \( PV = nRT \), where \( P \) is the pressure, \( V \) is the volume, \( n \) is the number of moles, \( R \) is the ideal gas constant, and \( T \) is the temperature in Kelvin.

Convert the given temperature from Celsius to Kelvin by using the formula \( T(K) = T(°C) + 273.15 \). For this problem, \( T = 28.0 + 273.15 \).

Convert the pressure from torr to atm, since the ideal gas constant \( R \) is typically given in terms of atm. Use the conversion factor \( 1 \text{ atm} = 760 \text{ torr} \). Therefore, \( P = \frac{780}{760} \text{ atm} \).

Rearrange the ideal gas law to solve for \( V \): \( V = \frac{nRT}{P} \). Substitute the values for \( n \), \( R = 0.0821 \text{ L atm K}^{-1} \text{ mol}^{-1} \), \( T \), and \( P \) to find the volume of HNO3 gas required.