Inside
Outside



First label letters and numbers very very very freakishly small
Second outline the boxes all ten
Third in box 5, write Block 7, Nature of Gases, Name, period and Picture of gas in action
Picture of Gas
in action
Vocabulary box 1
1. Charles Law- Temp change
Volume change
2. Boyles Law- PV=KT, where K
and T are constant
3. Gay-Lussac’s LawV1 / V2 = Whole number
4. Amonton’s Law- T increase
means Kinetic Energy increase, P
increase
5. Combined Gas Law- Charles
and Boyles together PV/T =K
6. Ideal Gas Law- P units pascals,
V units m3 T in kelvin, K = rn,
r = 8.314J/Kmol n moles PV = nrT
Box 8
Standards Chemistry



Box B
𝑃1
𝑉2
Box A
Charles law
A gas is collected and found to fill 2.85 L
at 25.0°C. What will be its volume at
standard temperature?
 Convert 25.0°C to Kelvin and you
get 298 K.
 Standard temperature is 273 K
 Plug into equation
2.85 L = V2
V2 = ??
298 K
273 K
Box C
Gay Lussac’s Law
ΣVRi / ΣVPi = K
Add all volumes divide by all
volumes = constant
2 volumes of Hydrogen + 1 volume of
Oxygen = 1 volumes of gaseous water
Box E
Combined Gas Law
Chance has a boyle on his face. The
boyle exerts a pressure of 2 atm, when
it is at a volume of 3 cm3 when he is in
the oozarks his boyle is at a volume of
2 cm3, with a pressure of 1 atm. Find
the temperature. Oozarks -73c is 200 K
(2)(3) = (1)(2)
6(200)= 2T1
T1
200
T1 = ??
4b- random motion of
molecules explains the
diffusion of gases.
4a–random motion of
molecules and their
collisions with a surface
create the observable
pressure on that surface.
4c- apply the gas laws to
relations between the
pressure, temperature, and
volume of an ideal gas or
any mixture of ideal gases.
=
𝑃2
𝑉1
Boyles Law
𝑃1
𝑉
= 𝑉2
P1V1 = P2V2
𝑃
2
1
4.40 L of a gas is collected at 100mmHg.
What will be its volume after increasing
pressure to 200atm?
 Convert 100mmHg
(1atm/760mmHg) = 0.13 atm
 Plug in values
(0.13 atm)(4.4L) = (200 atm) V2
V2 = ???
Box D
𝑃1
𝑃2
Amonton Law
𝑇
= 1
P1T2 = P2T1
𝑇2
A Basketball has a pressure of 31 atm
at a temperature of 298K. If Oscar is
shooting lights out, he’s on fire, and
the ball has a temp. of 325 K find the
pressure of the ball.
31 = 298
P2
325
298(P2) = 31(325)
Box F
Ideal Gas Law
PV = nRT
Solve for P, V = 2.5 L, n = 3mol
R = 8.314 T = 300
P(2.5) = 3(8.314)(300)
P = 7482.6 / 2.5 = 2993.04
Box G Copy Questions only
Answers in box H
1. Why is a gas easy to compress?
2. List three factors that can affect gas pressure.
3. Why does a collision with an air bag cause less
damage than a collision with a steering wheel?
4. How does a decrease in temperature affect the
pressure of a contained gas?
5. If the temperature is constant, what change in
volume would cause the pressure of an
enclosed gas to be reduced to one quarter of its
original value?
6. Assuming the gas in a container remains at a
constant temperature, how could you increase
the gas pressure in the container a
hundredfold?
Box K Copy Questions only
Answers in Box L
14. Briefly describe the assumptions of kinetic
theory as applied to gases.
15. Use kinetic theory to explain what causes gas
pressure.
16. How is the Kelvin temperature of a substance
related to the average kinetic energy of its
particles?
17. Convert the following pressures to
kilopascals.
18. a. 0.95 arm
b. 45 mm Hg
19. A cylinder of oxygen gas is cooled from 300 K
(27°C) to 150 K (-123°Q. By what factor does
the average kinetic energy of the oxygen
molecules in the cylinder decrease?
Box I Copy Questions only
Answers in Box J
7. How are the pressure and volume of a gas
related at constant temperature?
8. If pressure is constant, how does a change
in temperature affect the volume of a gas?
9. What is the relationship between the
temperature and pressure of a contained
gas at constant volume?
10. Write the mathematical equation for
Boyle's law and explain the symbols.
11. A given mass of air has a volume of 6.00 L
at 101 kPa. What volume will it occupy at
25.0 kPa if the temperature does not
change?
12. Explain how Charles's law can be derived
from the combined gas law.
13. The volume of a weather balloon increases
as the balloon rises in the atmosphere.
Why doesn't the drop in temperature at
higher altitudes cause the volume to
decrease?