What is the pressure, in mm Hg, of 2.50 moles of an ideal gas if it has a volume of 50.0 liters when the temperature is 27.0° C?

Use the ideal gas law:

PV=nRT

p = pressure

v = volume

n = number of moles of sample

R = ideal gas constant = ~0.08206 (l*atm) / (K*mole)

T = Temp in Kelvin

Now we substitute while simultaneously solving for P (pressure)

P = (nRT) / V

P = (2.50 * 0.08206 * (27+273.15)) / 50

P = Now it's your turn.