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

1.636 g of an unknown sulfur oxide gas, SO_x, is in a 0.5 L flask at 1 atm and 25.0 °C. Which is the most likely chemical formula of the compound?

SO2

S2O

SO3

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Verified step by step guidance

First, use the ideal gas law equation to find the number of moles of the gas. The ideal gas law is given by:

P V = n R T

, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature in Kelvin.

Convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature:

T =25.0+273.15

Rearrange the ideal gas law to solve for n (number of moles):

n = \frac{P V}{R T}

. Substitute the known values: P = 1 atm, V = 0.5 L, R = 0.0821 L·atm/mol·K, and T in Kelvin.

Calculate the molar mass of the unknown gas using the formula:

M = \frac{m}{n}

, where m is the mass of the gas (1.636 g) and n is the number of moles calculated in the previous step.

Compare the calculated molar mass with the molar masses of the given sulfur oxides (SO, SO2, S2O, SO3) to determine which formula matches the calculated molar mass. The closest match will be the most likely chemical formula of the compound.

4:09m

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Textbook Question

Which gas sample has the greatest pressure? Assume that all the samples are at the same temperature. Explain.

Textbook Question

Consider the apparatus shown in the following drawing. (a) When the valve between the two containers is opened and the gases are allowed to mix, how does the volume occupied by the N2 gas change?

Textbook Question

Imagine that you have two identical flasks, one containing chlorine gas and the other containing argon at the same temperature and pressure. How can you tell which is which without opening them?

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