Asked by Summer

3.2 grams of CH4 gas applies 760 mmHg pressure at 273 K temperature. Assume ideal gas behavior. The ideal gas constant is 62.36 (L· mmHg)/(K·mol), and the molecular mass of CH4 is 16 g/mol.

How much volume does the gas occupy?
Answered by DrBob222
mols CH4 = n = grams/molar mass, then
PV = nRT and remember T must be in kelvin.
Answered by Summer
The answer would be 45.0, correct?
Answered by DrBob222
No. I'll look for the error if you post your work.
Answered by Damon
messed up a decimal point?
Answered by Summer
101325*V=16*62.36, this is the equation I came up with with the ideal gas law. I cannot seem to come up with the correct formula.
Answered by Summer
Could the answer be 4.5?
Answered by Damon
well, I just happen to think that a mol occupies about 22.4 liters at Standard temp and pressure which is about where you are at.
you have 3.2/16 mols
3.2/16 * 22..4 = 4.48 liters
Answered by Damon
760 * V = (3.2/16)(62.36)(73)
V = 4.48 sure enough :)
Answered by Damon typo
I typed 73 instead of 273
Answered by Summer
Thank you very much Damon and DrBob! I appreciate your help!
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