Question

A gas sample occupies 6.2 L at a pressure of 201 kPa. What volume will it occupy if the pressure is increased to 335 kPa? The temperature remains the same.

Answer 1

The volume will be 3.72 L.

Step-by-step explanation:

We can find the new volume by using the Ideal Gas Law:

`PV = nRT`

Where:

P: is the pressure

V: is the volume

n: is the number of moles

R: is the gas constant

T: is the temperature

Initially, we have:

`P_(1)V_(1) = nRT` (1)

with V₁ = 6.2 L, P₁ = 201 kPa and nRT = constant

When the pressure is increased we have:

`P_(2)V_(2) = nRT` (2)

with V₂ =?, P₂ = 335 kPa and nRT = constant

By equating (1) and (2) we have:

`P_(1)V_(1) = P_(2)V_(2)`

`V_(2) = (P_(1)V_(1))/(P_(2)) = (201 kPa*6.2 L)/(335 kPa) = 3.72 L`

Therefore, the pressure is increased to 335 kPa the volume will be 3.72 L.

I hope it helps you!

Answer 2

Answer: The volume of the gas at the increased pressure will decrease to 3.72L.

Step-by-step explanation:

Boyle's law states that the volume occupied by a fixed mass of gas is inversely proportional to the pressure, provided temperature is kept constant. That is,

PV=K

P1V1 =P2V2

P1= 201 kpa

V1 = 6.2L

P2= 335kpa

V2= ?

Making V2 the subject of formula,

V2= P1V1/P2

V2= 201× 6.2/335

V2= 1246.2/336

V2= 3.72L

Thus, the volume of the gas decreases as the pressure increases. Hope this helps, thanks