Question

A gas occupies 525 mL at a pressure of 45.0 kPa. What would the volume of the gas be at a pressure of 65.0 kPa

Answer 1

Answer:

The volume of the gas at a pressure of 65.0 kPa would be 363 mL

Explanation:

Boyle's Law is a gas law that relates the pressure and volume of a certain amount of gas, without temperature variation, that is, at constant temperature.

Boyle's law states that the pressure of a gas in a closed container is inversely proportional to the volume of the container, when the temperature is constant. In other words, the product P · V remains constant at the same temperature:

P*V=k

Being P1 and V1 the pressure and volume in state 1 and P2 and V2 the pressure and volume in state 2 are fulfilled:

P1*V1=P2*V2

In this case:

• P1= 45 kPa= 45,000 Pa (being 1 kPa=1,000 Pa)
• V1= 525 mL= 0.525 L (being 1 L=1,000 mL)
• P2= 65 kPa= 65,000 Pa
• V2= ?

Replacing:

45,000 Pa* 0.525 L= 65,000 Pa*V2

Solving:

$V2=\frac{45,000 Pa* 0.525 L}{65,000 Pa}$

V2=0.363 L=363 mL

The volume of the gas at a pressure of 65.0 kPa would be 363 mL