Question

A gas that exerts a pressure of 537 torr in a container with a volume of 5.30 L will exert a pressure of 255 torr when transferred to a container with a volume of ? L

Answer 1

11.2

Step-by-step explanation:

Use Boyle' s Law

Rearrange it

plug in the numbers

remember to have 3 sig figs

and an awesome day!!

Answer 2

Answer:- The gas needs to be transferred to a container with a volume of 11.2 L.

Solution:- From Boyle's law. "At constant temperature, Volume is inversely proportional to the pressure."

It means, the volume is decreased if the pressure is increased and vice versa.

Here, the Pressure is decreasing from 537 torr to 255 torr. So, the volume must increase and calculated by using the equation:

`P_1V_1=P_2V_2`

Where,
`P_1` is initial pressure and
`P_2` is final pressure. Similarly,
`V_1` is initial volume and
`V_2` is final volume.

Let's plug in the values in the equation:

(537 torr)(5.30 L) = (255 torr)(
`V_2`)

`V_2=((537 torr*5.30 L)/(255 torr))`

`V_2` = 11.2 L

So, the new volume of the container needs to be 11.2 L.