1. A gas has a volume of 2.90 L, a pressure of 1.33 atm, and a temperature of 24

Question

1. A gas has a volume of 2.90 L, a pressure of 1.33 atm, and a temperature of 24.5 °C. Calculate the number of moles of gas present.

______ mol gas

2. A certain flexible weather balloon contains helium gas at a volume of 855 L. Initially, the balloon is at sea level where the temperature is 25°C and the barometric pressure is 726 torr. The balloon then rises to an altitude of 6000 ft, where the pressure is 605 torr and the temperature is 15°C. What is the change in volume of the balloon (in L) as it ascends from sea level to 6000 ft?

____________

3.

At what temperature will a 5.00 g sample of neon gas exert a pressure of 483 torr in a 7.00 L container?

________ K

Explanation / Answer

1.

V 2.9 L

P = 1.33 atm

T = 24.5°C = 297.5K

moles

PV = nRT

n = PV/(RT) = 1.33*2.9 / (0.082*297.5) = 0.15810 mol

2.

P1V1/T1 = P2V2/T2

726 * 855 / (25+273) = 605 * V/(15+273)

V = 726 * 855 / (25+273)*(15+273)/605

V = 991.570 L

3.

m = 5 g

MW = 20.1797

mol = mass/MW = 5/20.1797 = 0.2477

P = 483 torr = 483/760 = 0.6355 atm

V = 7 L

PV = nRT

T = PV/(RT) = 0.6355 * 7 / (0.082*0.2477) = 219.01493 K

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