A sample of a gas at room temperature occupies a volume of 29.0 L at a pressure of 562 torr . If the pressure changes to 2810 torr , with no change in the temperature or moles of gas, what is the new volume, V2?

The new volume will be 5.80 L

Explanation:

Step 1: Data given

The initial volume = 29.0 L

The initial pressure = 562 torr = 562 /760 atm = 0.739474 atm

The pressure changes to 2810 torr = 2810 /760 atm = 3.697368 atm

The temperature and number of moles will not change

Step 2: Calculate the new volume

P1*V1 = P2*V2

⇒With P1 = the initial pressure = 0.739474 atm

⇒with V1 = the initial volume = 29.0 L

⇒with P2 = the increased pressure = 3.697368 atm

⇒with V2 = The new volume = TO BE DETERMINED

0.739474 atm * 29.0 L = 3.697368 atm * V2

V2 = 5.80 L

OR

562 torr * 29.0 L = 2810 torr * V2

V2 = 5.80 L

The new volume will be 5.80 L

it takes on an electronical energy