Question

A sample of nitrogen (N2) has a volume of 42.0 L at a pressure of 752 mmHg. What is the final volume, in liters, of the gas at each of the following pressures, if there is no change in temperature and amount of gas?

723mmHg=

3.0 atm=

0.580aatm=

880 torr=

Answer 1

1) P1V1 = P2V2

where, P1 = 752 mmHg = 0.989 atm

V1 = 42.0 L

P2 = 723 mmHg = 0.951 atm

V2 = ?

0.989 * 42.0 = 0.951 * V2

41.5 = 0.951 * V2

V2 = 41.5 / 0.951 = 43.6 L

Therefore, the final volume = 43.6 L

2) P1V1 = P2V2

where, P1 = 752 mmHg = 0.989 atm

V1 = 42.0 L

P2 = 3.0 atm

V2 = ?

0.989 * 42.0 = 3.0 * V2

41.5 = 3.0 * V2

V2 = 41.5 / 3.0 = 13.8 L

Therefore, the final volume = 13.8 L

3) P1V1 = P2V2

where, P1 = 752 mmHg = 0.989 atm

V1 = 42.0 L

P2 = 0.580 atm

V2 = ?

0.989 * 42.0 = 0.580 * V2

41.5 = 0.580 * V2

V2 = 41.5 / 0.580 = 71.6 L

Therefore, the final volume = 71.6 L

4) P1V1 = P2V2

where, P1 = 752 mmHg = 0.989 atm

V1 = 42.0 L

P2 = 880 torr = 1.16 atm

V2 = ?

0.989 * 42.0 = 1.16 * V2

41.5 = 1.16 * V2

V2 = 41.5 / 1.16 = 35.8 L

Therefore, the final volume = 35.8 L