Oxygen used in respiratory therapy is stored at room temperature under a pressure of 150 atm in a gas cylinder with a volume of 60.0 L. What volume would the oxygen occupy at 0.925 atm? Assume no temperature change.

9,729.73 L

Explanation: Based on Boyle's law when temperature is held constant then the volume of a fixed mass of a gas, V is inversely proportional to Pressure, P. That is; Pα 1/V Mathematically, P = k/V where k is a constant Therefore, when the volume of a gas and the pressure are altered, P1V1=P2V2 = k, where P1 and P2 are the initial and final pressure respectively while V1 and V2 are the initial and final pressure respectively.

In this case;

Initial Pressure, P1 = 150 atm

Initial volume, V1 = 60.0 L

Final pressure, P2 = 0.925 atm

we are required to calculate the final volume

But, P1V1 = P2V2

Rearranging the formula, V2 = P1V1 : P2

Thus;

V2 = (150 atm * 60.0 L) : 0.925 atm

= 9,729.73 L

The new volume will be 9,729.73 L