The volume of a gas with an initial pressure of 350 mmhg increases from 5.0 l to 8.0 l. what is the final pressure of the gas, in atm, assuming no change in moles or temperature? g

Question

Jakobe

Chemistry

13 July, 13:34

The volume of a gas with an initial pressure of 350 mmhg increases from 5.0 l to 8.0 l. what is the final pressure of the gas, in atm, assuming no change in moles or temperature? g

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Rhett Lewis · Answer 1

Use the ideal gas law for this problemP1V1 = n1RT1 (1) P2V2 = n2RT2 (2) Dividing equation (2) by equation (1), and note that n1 = n2, T1 = T2, you have the familiar Boyle's Law:

P1V1 = P2 V2whereP1 = 350 mmHgV1 = 5.0 LV2 = 8.0 L

350 (5) = P2 (8) 1750/8 = P2218.75 mmHg = P2

Divide the answer to 760.0 mm Hg because that represents 1 atm

So the final pressure P2 is 760 mmHg or 0.29 atm.