February 28, 2017

Homework Help: Chemistry

Posted by Mewtwo on Saturday, September 30, 2006 at 2:51pm.

A spherical glass container of unknown volume contains helium gas at 25C and 1.960 atm. When a portion of the helium is withdrawn and adjusted to 1.00 atm at 25C, it is found to have a volume of 1.75 cm^3. The fas remaining in the first container shows a pressure of 1.710 atm. Calculate the volume of the spherical container.

Use PV = nRT to calculate n for the gas removed.
Then substitute this n in PV = nRT for the shperical container using P = 1.960 - 1.710 and solve for V.
Post your work if you get stuck.

1 atm X 1.75 cm^3 = n X(.08206)X 298.15K

n = 0.0715?
For the container.

(1.960 - 1.710 atm) X Volume = 0.0715 X (0.08206) X 298.15K.

Volume = 0.1429 cm^3?

That small?

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