Gas Law Review Chemistry Study Guide
1. STP: standard temperature and pressure
2. Standard Pressure: 1 atm, 760 torr/mmHg, 101.3 kPa (sea level)
3. Standard Temperature: 0ºC, 273K
4. kelvin: unit of temperature to be used with gas law equations
5. 20ºC-25ºC: room temperature
6. enclosed gas: fixed number of particles
7. Boyle's Law: pressure of an enclosed gas at CONSTANT TEMP is INVERSELY proportional to the volume of
the gas
8. increase pressure, decrease volume/ decrease pressure, increase volume: -
pressure and volume are inversely proportional
9. boyle's law equation: P1(V1) = P2(V2)
10. What is the resulting volume of 6.2L of gas at STP as the pressure is
increased to 2.6 atm?: identify P1: 1 atm P2: 2.6 atm V1: 6.2L V2: x
| solve: 1 atm(6.2L)= 2.6atm(V2)
| answer 2.4 L = V2
11. Charles' Law: volume of an enclosed gas at constant pressure is DIRECTLY proportional to the Kelvin
temp of the gas
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, 12. Charles' Law Equation: V1/T1 = V2/T2
13. 575 mL of a gas at 23ºC is heated to 77ºC. What is the resulting volume?:
identify: V1: 575mL, T1: 23ºC+273K, V2: x, T2: 77ºC + 273K
| solve: (575ml/296K) = (V2/350K)
| answer: 680mL
14. Gay-Lussac's Law: pressures of an enclosed gas at constant volume is directly proportional to the
kelvin temperature of the gas
15. Gay-Lussac's Equation: P1/T1=P2/T2
16. A 2.5L container at 25ºC and 255kPa is heated to 250ºC. What is the
resulting pressure?: identify: P1: 255kPa, T1: 298K, P2: x, T2: 523K (2.5L is constant)
| solve: (255kPa/298K) = (x/523K) cross multiply
| answer: 448 kPa
17. combined gas law: where pressure, volume and temperature all change
18. combined gas law equation: P1(V1)/T1 = P2(V2)/T2
19. A 30.0 L weather balloon at sea level and 17ºC rises in the atmosphere
to an altitude where the temperature is -32ºC and pressure is .31 atm. what is
the volume of the balloon?: identify: P1: sea level (1 atm), V1: 30.0L, T1: 290K, P2: .31atm, V2: x, T2: 241K
| solve: 1(30.0)/290 = .31 x/241
| answer: V2 = 80.42L
20. dalton's law of partial pressures: the sum of partial pressures of all gases in a mixture
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1. STP: standard temperature and pressure
2. Standard Pressure: 1 atm, 760 torr/mmHg, 101.3 kPa (sea level)
3. Standard Temperature: 0ºC, 273K
4. kelvin: unit of temperature to be used with gas law equations
5. 20ºC-25ºC: room temperature
6. enclosed gas: fixed number of particles
7. Boyle's Law: pressure of an enclosed gas at CONSTANT TEMP is INVERSELY proportional to the volume of
the gas
8. increase pressure, decrease volume/ decrease pressure, increase volume: -
pressure and volume are inversely proportional
9. boyle's law equation: P1(V1) = P2(V2)
10. What is the resulting volume of 6.2L of gas at STP as the pressure is
increased to 2.6 atm?: identify P1: 1 atm P2: 2.6 atm V1: 6.2L V2: x
| solve: 1 atm(6.2L)= 2.6atm(V2)
| answer 2.4 L = V2
11. Charles' Law: volume of an enclosed gas at constant pressure is DIRECTLY proportional to the Kelvin
temp of the gas
1/
5
, 12. Charles' Law Equation: V1/T1 = V2/T2
13. 575 mL of a gas at 23ºC is heated to 77ºC. What is the resulting volume?:
identify: V1: 575mL, T1: 23ºC+273K, V2: x, T2: 77ºC + 273K
| solve: (575ml/296K) = (V2/350K)
| answer: 680mL
14. Gay-Lussac's Law: pressures of an enclosed gas at constant volume is directly proportional to the
kelvin temperature of the gas
15. Gay-Lussac's Equation: P1/T1=P2/T2
16. A 2.5L container at 25ºC and 255kPa is heated to 250ºC. What is the
resulting pressure?: identify: P1: 255kPa, T1: 298K, P2: x, T2: 523K (2.5L is constant)
| solve: (255kPa/298K) = (x/523K) cross multiply
| answer: 448 kPa
17. combined gas law: where pressure, volume and temperature all change
18. combined gas law equation: P1(V1)/T1 = P2(V2)/T2
19. A 30.0 L weather balloon at sea level and 17ºC rises in the atmosphere
to an altitude where the temperature is -32ºC and pressure is .31 atm. what is
the volume of the balloon?: identify: P1: sea level (1 atm), V1: 30.0L, T1: 290K, P2: .31atm, V2: x, T2: 241K
| solve: 1(30.0)/290 = .31 x/241
| answer: V2 = 80.42L
20. dalton's law of partial pressures: the sum of partial pressures of all gases in a mixture
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