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?
mols CH4 = n = grams/molar mass, then
PV = nRT and remember T must be in kelvin.
The answer would be 45.0, correct?
messed up a decimal point?
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.
Could the answer be 4.5?
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
760 * V = (3.2/16)(62.36)(73)
V = 4.48 sure enough :)