A 10.0 L balloon contains helium gas at a pressure of 655 torr. what is the new
ID: 1049718 • Letter: A
Question
A 10.0 L balloon contains helium gas at a pressure of 655 torr. what is the new pressure of the helium gas at a volume of 1500 ml if there is no change in temperature? P1V1 = P2V2 A sample of nitrogen gas has a volume of 50.0 L at a pressure of 760. torr. What is the new volume of the gas at a pressure of 0.500 atm? Charles' Law: A sample of neon initially has a volume of 2.50 L at 15 degree C. What is the new temperature in degree C when the volume is changed at constant pressure to 5.00L? V1/T1 = V2/T2 A balloon contains 2500 ml of helium gas at 75 degree C. What is the new volume of the gas when the temperature changes at constant pressure to -25 degree C?Explanation / Answer
1) 1.0 atm = 760 mmHg
0.866 atm = 658.16 mmHg
2) P1V1 = P2V2
P1 = 655 torr = 0.86 atm , V1 = 10.0 L
P2 = ? V2 = 1500 mL = 1.5 L
P2= (0.86 x 10) / 1.5
P2 = 5.73 atm = 4354.8 torr
3) P1V1 = P2V2
P1 = 760 torr = 1.0 atm , V1 =50 L
P2 = 0.5 atm , V2 = ?
V2 = (1.0 x 50) / 0.5
V2 = 100 L
4) V1/T1 = V2/T2
V1 = 2.50 L , T1 = 150C = 288 K
T2 = ? , V2 = 5.0 L
T2 = (5.0 x 288 / 2.50)
T2 = 576 K = 3030C
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