1. G - L’s Law – Pressure vs. Temperature

2. Experiment to develop the relationship between the pressure and temperature of a gas.
Include: Gay-Lussac’s Law, Combined Gas Law, partial pressure
Additional KEY Terms

3. = P1V1 P2V2 BOYLE’S LAW – Pressure vs. Volume Pressure (kPa)
Volume (mL)

4. = V1 V2 T1 T2 CHARLES’S LAW – Temp vs. Volume Volume (mL)
Temperature (K)

5. Joseph Gay-Lussac ( )
Determined that temperature and pressure of a gas is a direct relationship (volume and amount of gas are held constant)

6. **As with Charles’ Law, temperature in Kelvin.= P1 P2 T1 T2

7. If a 12. 0 L sample of gas is found to have a pressure of 101
If a 12.0 L sample of gas is found to have a pressure of kPa at 0.0°C, calculate the new pressure at 128°C if the volume is held constant. P1 = P2 T1 T2
0.0°C = 273 K 128°C +273 = 401 K
101.3
149 kPa P2
(401) =
273

8. combined gas law P1 V1 = P2 V2 T1 T2 Boyle’s Law: Pressure α ___1___
volume
Charles’ Law: Volume α temperature
Gay-Lussac’s Law: Pressure α temperature P1 V1 = P2 V2 T1 T2
combined gas law

9. If a gas occupies a volume of 25. 0 L at 25. 0°C and 1
If a gas occupies a volume of 25.0 L at 25.0°C and 1.25 atm, calculate the volume at 128°C and atm. P1 V1 = P2 V2 T1 T2
25°C = 298 K 128°C +273 = 401 K
(1.25) 25 =
56.1 L V2
(401)
298 (0.750)

10. A gas has a volume of 125 L at 325 kPa and 58
A gas has a volume of 125 L at 325 kPa and 58.0°C, calculate the temperature in Celsius to produce a volume of 22.4 L at kPa P1 V1 = P2 V2 T1 T2
58°C = 331 K
18.5 K T2
(101.3)
22.4
(331) =
325 (125)
18.5 K = -254°C

11. A bag contains 145 L of air at the bottom of a lake, at a temperature of 5.20°C and a pressure of 6.00 atm. When the bag is released, it ascends to the surface where the pressure is 1.00 atm and 16.0°C.
Given:
P1 = 6.00 atm V1 = 145L T1 = 5.20°C
P2 = 1.00 atm T2 = 16.0°C
If the maximum volume of the lift bag is 750 L, will the bag burst at the surface?
Find: V2

12. Ptotal = P1 + P2 + P3 + P4 … Dalton’s Law of Partial Pressure:
Each gas in a mixture exerts pressure independently.
Total pressure = sum of the pressures of each gas (partial pressures)
Partial pressure depends on the number of gas particles present, the temperature and volume of container.
Ptotal = P1 + P2 + P3 + P4 …

13. 1.0 mol H2
2.0 mol He
3.0 mol gas

14. 2.0 L of O2 at an original pressure of 202.6 kPa
The following gases are placed in a litre container and held at a constant temperature:
2.0 L of O2 at an original pressure of kPa
3.00 L of Ne at an original pressure of kPa
What pressure is produced inside the container?
HINT: Each gas is will expand when put into the L container, so each will exert a partial pressure less than its original pressure.

15. P1V1 = P2V2
Oxygen: (202.6)(2.00) = P2 (10.00) P2 = 40.5 kPa
Neon: (303.9)(3.00) = P2 (10.00) P2 = 91.2 kPa
Total pressure = = kPa

17. CAN YOU / HAVE YOU?
Experiment to develop the relationship between the pressure and temperature of a gas.
Include: Gay-Lussac’s Law, Combined Gas Law, partial pressure
Additional KEY Terms