Gas Law Problems

Gas Law Problems

2. If a gas at 25.0 °C occupies 3.60 liters at a pressure of 1.00 atm, what will be its volume at a pressure of 2.50 atm? (Use Boyle’s Law)

P1V1 = P2V2

P1=1.00 atm V1= 3.60 L P2= 2.5 atm V2=?

(1.00 atm) (3.60 L) = (2.5 atm) ( V2)

3.60 atm L = 2.5 atm V2

2.5 atm 2.5 atm

V2 = 1.44 L

3. A balloon is inflated to 5L at 20°C.What will be the new volume of the balloon if it is put in a freezer at 0°C? .(Use Charles’ Law)

V1 = V2

T1 = T2

V1= 5 L T1= 293 K V2= ? T2= 273 K

273 K 5L = V2 (273 K)

293 K 273 K

1365 L = V2 V2 = 4.66 L

293

4. A gas occupies 1.56 L at 1.00 atm. What will be the volume of this gas if the pressure becomes 3.00 atm? (Use Boyle’s Law)

P1V1 = P2V2

P1=1.00 atm V1= 1.56 L P2= 3 atm V2=?

(1.00 atm) (1.56 L) = (3 atm) ( V2)

1.56 atm L = 3 atm V2

3 atm 3 atm

V2 = 0.52 L

5. A cylinder of chlorine gas is stored in a concrete-lined room for safety. The cylinder is designed to withstand 50.0atm of pressure. The pressure gage reads 35.0 atm at 23.2°C. An accidental fire in the room next door causes the temperature in the storeroom to increase to 87.5°C. What will the pressure gage read at this temperature? (Use Gay-Lussac’s Law)

P1 / T1 = P2 / T2

P1 = 35 atm T1 = 23.2 C P2 = ? T2 = 87.5C

35 atm / 23.2*C = P2 / 87.5*C

(87.5*C) 35 atm / 23.2*C = P2 / 87.5*C (87.5*C)

3062.5 atm / 23.2 = P2

P2 = 132.00 atm

6. A gas occupies 11.2 liters at 0.860 atm. What is the pressure if the volume becomes 15.0 L? (Use Boyle’s Law)

P1V1 = P2V2

P1 = 0.86 atm V1 = 11.2 L P2 = ? V2= 15 L

(0.86 atm) (11.2 L) = (P2) ( 15 L)

15L 15 L

P2 = 0.642 atm

7. If you took a balloon outside that was originally at 20°C at 2 L in volume, and it heated up to 29°C, then what would its new volume be? (Use Charles’ Law)

V1 = V2

T1 = T2

V1= 2 L T1= 293 K V2= ? T2= 302 K

302 K 2L = V2 (302 K)

293 K 302 K

604 L = V2 V2 = 2.06 L

293

8. A 40.0 L tank of ammonia has a pressure of 1000 mmHg. Calculate the volume of the ammonia if its pressure is changed to 500 torr while its temperature remains constant.

P1V1 = P2V2

P1 = 1000 torr V1 = 40 L P2 = 500 torr V2= ?

(1000 torr) (40 L) = (V2) ( 500 torr)

500 torr 500 torr

40000 L = V2

500 V2 = 80 L

9. Chlorine gas occupies a volume of 1.2 liters at 720 torr pressure. What volume will it occupy at 1 atm pressure? (Use Boyle’s Law)

P1V1 = P2V2

P1 = 1 atm V1 = 1.2 L P2 = 0.95 atm V2= ?

(1 atm) (40 L) = (V2) ( 0.95 atm)

0.95 atm 0.95 atm

40 L = V2

0.95 V2 = 42.11 L

1 atm = 101.3 kPa = 101,325 Pa = 760 mm Hg = 760 torr

Use these conversion factors (dimensional analysis) to solve 8 and 9.