1. Review for Test 5
Gas Laws

2. Charles Law V1 = V2 P constant T1 T2 Boyles Law P1V1 = P2V2 T constant Gay-Lussac’s Law P1 = P2 V constant T1 T2 Combined P1V1 = P2V2 T1 T2 Ideal Gas Law PV = nRT
Whatever is held constant is not in the equation.
Gay-Lussac: warm tires increase in pressure

3. Dalton’s Law of Partial Pressure
The sum of the individual gas pressures equals the overall pressure of the mixture of gases.
P1 + P2 + P = Ptotal
The gases would be the same temperature and have the same volume. The difference in their volumes is due only to the numbers of their molecules.

4. A sample of gas occupies 2. 97 L at 72˚C
A sample of gas occupies 2.97 L at 72˚C. What volume would it take up at 502K? V1 = V2 T1 T2 Volume should increase! 2.97L x 502K = 4.32 L 345K

5. A gas-filled bottle is heated from 25°C to 89°C
A gas-filled bottle is heated from 25°C to 89°C. If the original pressure was 760 torr, what would be the new pressure ? T1 = =298K T2 = =362K 760 = P P2 = 923 torr

6. A gas at 98. 2 kPa has a volume of 39L. What is its volume at 120
A gas at 98.2 kPa has a volume of 39L. What is its volume at 120.5kPa and constant temperature? P1V1 = P2V2 Volume should decrease. 39L x 98.2 kPa = 31.8L kPa

7. At STP, the volume of a gas is 325 mL. What volume does it occupy at 20.0°C and 93.3kPa? P1V1 = P2V2 T1 T2 325 mL x 293K x kPa = 379 mL 273K 93.3 kPa

8. P= nRT V = .00306mol x 8.31 L∙kPa x 282K .0259 L mol∙K = 277kPa
What pressure is exerted by mole of gas in a 25.9 cm3 container at 9˚C?
P= nRT V
= mol x 8.31 L∙kPa x 282K
.0259 L mol∙K
= 277kPa

9. A 35. 0L tank contains 7. 00 mol of compressed air
A 35.0L tank contains 7.00 mol of compressed air. If the pressure inside the tank is kPa, what is the temperature of the compressed gas? T = PV nR T = 500.0kPa x 35.0L 7.00mol x 8.31 = 301 K

10. A gaseous mixture containing argon, nitrogen, and oxygen is in a vessel. If the total pressure is 98.5 kPa, and the partial pressures of nitrogen and argon are 22.0 kPa and 50.0 kPa respectively, what is the partial pressure of oxygen? Ptot = PAr + PN + PO 98.5 kPa = Po PO = 26.5 kPa