A 10.0 L balloon contains helium gas at a pressure of 655 torr. what is the new

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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