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.

Question

How much volume does the gas occupy?

Answer 1

mols CH4 = n = grams/molar mass, then
PV = nRT and remember T must be in kelvin.

Answer 2

The answer would be 45.0, correct?

Answer 3

No. I'll look for the error if you post your work.

Answer 4

messed up a decimal point?

Answer 5

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.

Answer 6

Could the answer be 4.5?

Answer 7

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

Answer 8

760 * V = (3.2/16)(62.36)(73)
V = 4.48 sure enough :)

Answer 9

I typed 73 instead of 273

Answer 10

Thank you very much Damon and DrBob! I appreciate your help!