Question

A gas that exerts a pressure of ? bar in a container with a volume of 0.5650 L will exert a pressure of 715.1 bar when transferred to a container with a volum of 1.204 L

Answer 1

Robert Boyle, the 17th century British chemist, first noticed that the volume of a given amount of gas is inversely proportional to its pressure when kept at a constant temperature. When working with ideal gases we use PV = nRT, but remember n, R, and T are all constant. Therefore we have:

PV(before) = PV(after)

P(0.5650) = (715.1)(1.204)

Answer 2

Answer:

The pressure is 1,523.86 bar

Explanation:

Pressure and volume are related by Boyle's law, which says:

"The volume occupied by a given gas mass at constant temperature is inversely proportional to the pressure"

Boyle's law is expressed mathematically as:

Pressure * Volume = constant

o P * V = k

You have a certain volume of gas V1 that is at a pressure P1 at the beginning of the experiment. If you vary the gas volume to a new value V2, then the pressure will change to P2, and it will be true:

P1 * V1 = P2 * V2

In this case, you know:

• P1= ?
• V1= 0.5650 L
• P2= 715. 1 bar
• V2= 1.204 L

Replacing:

P1* 0.5650 L= 715.1 bar* 1.204 L

Solving:

$P1=\frac{715.1 bar*1.204 L}{0.5650 L}$

P1= 1,523.86 bar

The pressure is 1,523.86 bar