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A 2.6 liter container of nitrogen had a pressure of 3.2 atm. What volume will the gas occupy at a pressure of

1.5 atm?

User Narko
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1 Answer

6 votes

Final answer:

The volume the nitrogen gas will occupy at a pressure of 1.5 atm, using Boyle's Law, is calculated to be 5.44 liters.

Step-by-step explanation:

The student's question can be solved using Boyle's Law, which states that the pressure of a gas is inversely proportional to the volume when the temperature and the amount of gas are held constant. The formula for Boyle’s Law is P1 * V1 = P2 * V2, where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume respectively.

In this scenario:
P1 = 3.2 atm (initial pressure)
V1 = 2.6 liters (initial volume)
P2 = 1.5 atm (final pressure)
V2 = ? (final volume to be calculated)

Using the formula: 3.2 atm * 2.6 L = 1.5 atm * V2
So, V2 = (3.2 atm * 2.6 L) / 1.5 atm = 5.44 L. Therefore, the gas will occupy a volume of 5.44 liters at a pressure of 1.5 atm.

User KlingonJoe
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