Question

An oxygen cylinder used in a hospital contains 35.4 L of oxygen gas at a pressure of 149.6 atm. How much volume would the oxygen occupy if it were transferred to a container that maintained a pressure of 1.00 atm if the temperature remains constant

Answer 1

Answer: 5296 L

Explanation:

To calculate the new volume, we use the equation given by Boyle's law. This law states that pressure is directly proportional to the volume of the gas at constant temperature.

The equation given by this law is:

$P_1V_1=P_2V_2$

where,

$P_1\text{ and }V_1$ are initial pressure and volume.

$P_2\text{ and }V_2$ are final pressure and volume.

We are given:

$P_1=149.6atm\\V_1=35.4L\\P_2=1.00atm\\V_2=?$

Putting values in above equation, we get:

$149.6\times 35.4L=1.00\times V_2\\\\V_2=5296L$

Thus volume occupied by oxygen if it were transferred to a container that maintained a pressure of 1.00 atm if the temperature remains constant is 5296 L