Part A: A cylinder contains 29.5L of oxygen gas at a pressure of 1.7 atm and a t

Question

Part A:
A cylinder contains 29.5L of oxygen gas at a pressure of 1.7 atm and a temperature of 290K. How much gas (in moles) is in the cylinder? Express your answer using two significant figures.

Part B:
A weather balloon is inflated to a volume of 28.6L at a pressure of 730 mmHg and a temperature of 30.8°C. The balloon rises in the atmosphere to an altitude where the pressure is 400 mmHg and the temperature is -13.9° C. Assuming the balloon can freely expand, calculate the volume of the balloon at this altitude.

Explanation / Answer

Part A:-

Applying Ideal Gas Equation i.e, P*V = n*R*T ; we get

moles of the oxygen gas, n = (P*V)/(R*T) = (1.7*29.5)/(0.0821*290) = 2.106 moles

Part B:-

Since moles of the gas remains constant inside the balloon,

therefore , (P1*V1)/T1 = (P2*V2)/T2

where P1 = 730 mm of Hg ; P2 = 400 mm of Hg ; V1 = 28.6 litres , V2 = ? ; T1 = 303.8 K & T2 = 259.1 K

Thus, V2 = 44.515 litres

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