A gas sample with a constant number of gas molecules and at a constant temperature has a volume of 5.0 L at 50 mmHg pressure. The volume of the container can be varied. What would the gas sample volume be (in Liters) if the pressure of the gas increased to 500 mmHg?

.5 L

Explanation:

- Start with the Ideal Gas Law. This equation will be P1V1T2=P2V2T1

- Next, take out temperature because that is not given and therefore constant.

- Rearrange the equation. You should get V2=V1P1/P2

- Fill in with variables. You should get V2=((5.)(50))/500

- Solve and you will get .5L

- Lastly, you can check this by knowing that P and V at constant T have an inverse relationship. Hence, volume went down, while pressure went up.

the formula would be mgso4

mgso[subscript]4