1. GAS LAWS
Quantitatively measure the relationship between
Pressure,Volume andTemperature.

2. PRESSURE:
is created by gas particles hitting a surface.

3. BOYLE’S LAW
pV = constant
p1V1=p2V2
Assumes temperature is constant
Pressure ↑,Volume↓
Pressure↓,Volume↑

4. PRACTICE PROBLEM:
Bacteria produce methane gas in sewage-treatment
plants.This gas is often captured or burned. If a bacterial
culture produces 60.0 mL of methane gas at 700.0 mm
Hg, what volume would be produced at 760.0 mm Hg?
p1V1=p2V2
700 mmHg x 60.0 mL = 760 mmHg xV2
= 55.3 mL of methane gas

5. PRACTICE PROBLEM
Hospitals buy 400-L cylinders of oxygen gas compressed
at 150 atm.They administer oxygen to patients at 3.0 atm
in a hyperbaric oxygen chamber.What volume of oxygen
can a cylinder supply at this pressure?
p1V1=p2V2
150 atm x 400 L mL = 3.0 atm xV2
= 20,000 L of oxygen

6. CHARLES’ LAW
V/T = constant
V1/T1 =V2/T2
Assumes pressure is constant.
Temp must be measured in Kelvin (K=˚C + 273)
V ↑ T↑
V↓ T↓

7. PRACTICE PROBLEM
A balloon is filled with 3.0 L of helium at 310 K.The
balloon is placed in an oven where the temperature
reaches 340 K.What is the new volume of the balloon?
V1/T1 =V2/T2
3.0L/310K =V2/340K
V2= 3.3 L

8. PRACTICE PROBLEM
A 25 L sample of nitrogen is heated from 110 ˚C to 260 ˚C.
What volume will the sample occupy at the higher
temperature?
K=˚C + 273
T1 = 110 ˚C + 273
T1 = 383 K
T2 = 260˚C + 273
T2 = 533 K
V1/T1 =V2/T2
25L/383K = V2/533K
V2= 35 L

9. COMBINED GAS LAW
PV/T = constant
P1V1/T1 = P2V2/T2

10. PRACTICE PROBLEM
A gas that has a volume of 28 L, a temperature of 45˚C, and an
unknown pressure has its volume increased to 34 L and its
temperature decreased to 35˚C. If I measure the pressure after
the change to be 2.0 atm, what was the original pressure of the
gas?
P1 = ?
V1 = 28L
T1 =45˚C + 273 = 318K
P2 = 2.0 atm
V2 = 34 L
T2 = 35˚C + 273 = 308 K
P1V1/T1 = P2V2/T2
(P1x 28L)/318K = (2.0atm
x 34L)/308K
P1 = 2.51 atm

11. PRACTICE PROBLEM
I have an unknown volume of gas at a pressure of 5.0 x 104 Pa and
a temperature of 325 K. If I raise the pressure to 1.2 x 105 Pa,
decrease the temperature to 320 K, and measure the final volume
to be 4.8 x 104 cm3, what was the initial volume of the gas?
P1V1/T1 = P2V2/T2
(5.0 x 104 Pa xV1)/325K =
(1.2 x 105 Pa x 4.8 x 104 cm3)/320K
V1 = 1.17x1013cm3