Study the scenario.

8 grams of C3H4 gas occupies a volume of 8.2 L at 300 K temperature. Assume ideal gas behavior. The ideal gas constant is 0.082 (L·atm)/(K·mol), and the molecular mass of C3H4 is 40 g/mol.

How much pressure is the gas applying to the walls of its container?

0.8 atm

0.4 atm

0.5 atm

0.6 atm

B?

2 answers

No. Are you using the ideal gas law. PV = nRT
Post your work and I'll find the error.
P = Pressure (atm) V = Volume (L) n = moles R = gas constant = 0.08

so its A?