Name ____________________________________
Unit 8: Gas
8-1 Properties of Gas
1.
What are the properties of gasses? a.
Gas – i.
ii.
iii.
iv.
v.
vi.
b.
How do gasses exert a pressure on the sides of their containers? c.
What determines how much pressure a gas exerts?
2.
How do we quantify Gases? a.
There are 4 variables used to do gas calculations: i.
N – ii.
V- iii.
T-
1.
How do you convert between Kelvin and Celsius iv.
P-
1.
1atm = 101325Pa (Pascals)= 760mm Hg or torr= 14.7 lb/in 2 (psi)
Period ____________ b.
STP-
8-2 The Gas Laws
1.
What is the Combined Gas Law? a.
When is the combines gas law used?
Gas law animations can crush
1
1
1
2
2
2
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Sample Combined Gas Law Problems:
1.
72.0 mL of O
2
at 25 o C is at a pressure of 198 KPa. Determine the volume that the gas will occupy at STP.
2.
A sealed 1000L hot air balloon takes off at ground level (1atm) on a sunny day (25 o C). What will the volume of the balloon be at a altitude of 30,000 ft. where the pressure is 0.63atm and the temperature is 15 o C?
8-3 Avogadro’s Law
2.
What is Avogadro’s law?
3.
What volume will all gasses occupy at STP (1atm and 0 o C)
Sample mole gas conversations:
4.
How many L will 8 moles of CO
2 occupy at STP?
5.
How many moles of particles are in 44.8L?
6.
What is Dalton’s Law of Partial Pressures of gasses?
P
TOTAL
= P
A
+P
B
+ P
C . . . .
a.
In a mixture of gases, each individual gas exerts a portion of the total pressure of the mixture. The sum of the partial pressures of all the components in a gas mixture is equal to the total pressure of the gas mixture.
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Sample Daltons Law Problems:
1.
A flask contains a mixture of oxygen, argon, and carbon dioxide with partial pressures of 745 torr, 0.278 atm, and
391 mmHg respectively. What is the total pressure in the flask?
2.
The total pressure of a mixture of helium and neon is 498 mm Hg. If helium is 20.0 % of the mixture, what is the partial pressure of helium?
3.
What the air pressure in a greenhouse if a barometer reads 792mmHg the vapor pressure of water is measured to be 30mmHg?
8-4 The ideal gas Law
1.
What is an ideal gas? a.
What are the properties of an ideal gas? b.
Does an ideal gas exist? c.
What is the point of the ideal gas law?
2.
What is the ideal gas law? a.
The ideal gas law was determined by measuring a series of gasses (1mol of them) at the same pressure temperature and volume. i.
It was found that no matter what the gas was, when you multiply the pressure and volume, and the amount of a gas with the temperature, and divide the two together you always get the same number, R (the universal gas constant
R = 0.0821
𝑎𝑡𝑚 ∙𝐿 𝑚𝑜𝑙 ∙𝐾
or
𝑃𝑉
𝑁𝑇
= 0.0821
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ii.
However, because the units for P,V, N, and T can change R is unit specific iii.
In order to use 0.0821 as R you must have the following units:
P = atm
V =L n = number of moles
T = Kelven
Ideal Gas Law Problems:
1.
How many grams of carbon dioxide occupy a volume of 36.9 mL at 158 KPa and 72 o C?
2.
How much would a 20lb 8L SCUBA tank way at 22 o C if it were filled with oxygen gas until the pressure inside the tank was 200atm?
3.
What volume of gas would be produced if a 1Kg chunk of dry ice (solid CO
2
) turned completely to gas at sea level (1atm) and room temperature (22 o C)
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