A sample of a gas at room temperature occupies a volume of 18.0 L at a pressure of 902 torr . If the pressure changes to 4510 torr , with no change in the temperature or moles of gas, what is the new volume, V2

The correct answer is 3.6 L

Explanation:

According to the gases Boyle's law, the relation between the volume and  the pressure of a gas at constant temperature is given by the following mathematical expression:

Pi x Vi = Pf x Vf

Where Pi and Vi are the initial pressure and volume of the gas whereas Pf and Vf are the final pressure and volume, respectively.

In this problem we have:

Vi = 18.0 L

Pi= 902 Torr

Pf= 4510 Torr

The final volume (Vf) will be:

Vf = (Pi x Vi)/Pf = (902 Torr x 18.0 L)/4510 Torr= 3.6 L

From the result, we can see that if the pressure increases, the volume of the gas decreases.

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