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