Calculating Pressure Using Boyle's Law

A sample of carbon dioxide occupies a volume of 3.50 L at 125 kPa

What pressure would the gas exert if the volume was decreased to 2.00 L but the temperature was held constant?

Question: A sample of carbon dioxide occupies a volume of 3.50 L at 125 kPa. What pressure would the gas exert if the volume was decreased to 2.00 L but the temperature was held constant? Answer: Using Boyle's Law, the final pressure exerted by a sample of carbon dioxide gas that has its volume decreased from 3.50 L to 2.00 L at constant temperature is 218.75 kPa.

Explanation:

The question involves applying Boyle's Law, which states that for a given mass of gas at constant temperature, the volume of the gas is inversely proportional to its pressure.

According to Boyle's Law (P1V1 = P2V2), where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume, the pressure exerted by the gas can be calculated if the volume is decreased and temperature remains constant.

In this case, for a sample of carbon dioxide gas that has an initial volume (V1) of 3.50 L at an initial pressure (P1) of 125 kPa, and the volume is decreased to 2.00 L (V2), the final pressure (P2) can be calculated using:

P2 = (P1 * V1) / V2

= (125 kPa * 3.50 L) / 2.00 L

= 218.75 kPa (final pressure with volume decreased to 2.00 L)

← What gas is used in a flame ionization detector Chemical properties of phosphoric acid →

More Posts: