Aleksza Honors Chemistrty 2013-14
Crash Course Chemistry: Episode #12 – The Ideal Gas Law
( http://www.youtube.com/watch?v=BxUS1K7xu30&index=13&list=PL8dPuuaLjXtPHzzYuWy6fYEaX9 mQQ8oGr# )
Name:______________________________________________________MOD:________
1.
What is Boyles’ Law?
2.
What is Charles’ Law?
3.
What is Avogadro’s Law?
4. What is the Ideal Gas Law Equation and what do the symbols mean?
5. Identify the different units of pressure.
6. What is the universal gas constant?
7. What are the 2 special cases where the gas law no longer applies? (Think about the equation.)
8. Describe how and when you are able to use the Ideal Gas Law. Provide basic examples of how your would use this equation to solve for Pressure, Volume, Temperature and number of moles.
9. Define the following terms:
STP:
Absolute Zero

Aleksza Honors Chemistrty 2013-14
Crash Course Chemistry: Episode #13 – The Ideal Gas Law Problems http://www.youtube.com/watch?v=8SRAkXMu3d0&list=PL8dPuuaLjXtPHzzYuWy6fYEaX9mQQ8oGr
Name:______________________________________________________MOD:________
1. Describe why large size and attraction to others = trouble for gases?
2. How did Mendeleev rescue the Ideal Gas Law?
3. Under what three conditions does the Ideal Gas Law no longer apply?
4. Which temperature scale is used in Gas Laws? ________________________________
5. What is the relationship between volume and 1 mol of a gas at STP? (dimensional analysis ratio)

Aleksza Honors Chemistrty
Crash Course Chemistry: Episode #14 – Real Gases
2013-14 http://www.youtube.com/watch?annotation_id=annotation_5563&feature=iv&src_vid=8SRAkXMu3d0
&v=GIPrsWuSkQc
Name:______________________________________________________MOD:________
1. Describe the van Der Waals Equation. (ID all variables)
2. Solve the following problem using the van Der Waals Equation:
If 1.00 mol of an ideal gas were confined to 22.4 L at 0.0
°C, it would exert a pressure of 1.00 atm.
Use van der Waals equation and the constants below, to estimate the pressure exerted by 1.00 mol of Cl
2(g) in 22.41 L at 0.0 °C.
R = 0.08206 L-atm/mol-K, a = 6.49 L 2 -atms/mol 2 and b = 0.0563 L/mol

Aleksza Honors Chemistrty 2013-14
Crash Course Chemistry: Episode #15 – Partial Pressures & Vapor Pressure http://www.youtube.com/watch?v=JbqtqCunYzA
Name:______________________________________________________MOD:________
1.
Describe Dalton’s law of Partial Pressures. (ID all variables)
2. Describe a mole fraction. (ID all variables)
3. Describe the process of collecting a gas over a column of water.
4. Define vapor pressure.

Aleksza Honors Chemistrty 2013-14
Crash Course Chemistry: Episode #15 – Partial Pressures & Vapor Pressure http://www.youtube.com/watch?v=JbqtqCunYzA
Name:______________________________________________________MOD:________
1. Explain Net velocity vs Average velocity:
2. Define Effusion and the Rate of Effusion:
3. Explain Graham’s Law of Effusion and identify all the variables involved.
4. Define Diffusion
5. Define Concentration Gradients
6. Describe the Precipitation RXN with gases and compare that to the precipitation reaction of aqueous solutions.