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

Effusion

General Chemistry

7. Gases

Effusion

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Multiple Choice

Which gas will have a faster rate of effusion according to Graham's law?

Helium (He)

Nitrogen (N2)

Carbon dioxide (CO2)

Oxygen (O2)

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Verified step by step guidance

Understand Graham's Law of Effusion, which states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass. Mathematically, this can be expressed as:

\frac{r}{r'} = \sqrt{\frac{M'}{M}}

, where r and r' are the rates of effusion of two gases, and M and M' are their molar masses.

Identify the molar masses of the gases in question: Helium (He) has a molar mass of approximately 4 g/mol, Nitrogen (N2) has a molar mass of approximately 28 g/mol, Carbon dioxide (CO2) has a molar mass of approximately 44 g/mol, and Oxygen (O2) has a molar mass of approximately 32 g/mol.

Apply Graham's Law to compare the rate of effusion of Helium with each of the other gases. Since the rate of effusion is inversely proportional to the square root of the molar mass, the gas with the smallest molar mass will effuse the fastest.

Calculate the square root of the molar masses for each gas to determine their relative rates of effusion. For example, for Helium, calculate

\sqrt{4}

, and compare it with

\sqrt{28}

for Nitrogen,

\sqrt{44}

for Carbon dioxide, and

\sqrt{32}

for Oxygen.

Conclude that the gas with the smallest square root of its molar mass will have the fastest rate of effusion. In this case, Helium, with the smallest molar mass, will effuse faster than Nitrogen, Carbon dioxide, and Oxygen.