Gas Law Problem!! HELP!!

What mass (in grams) of N2 gas is present in a 25.0 L container at 100 K at 5.0 atm N2 pressure if the gas is ideal?

PV = nRT = gRT / MM
g = PV * MM / RT = 5.0 * 25.0 * 28.0 / (0.08206 * 100) = 427 g

use ideal gas law PV=nRT

P = pressure in atm
V = volume in liters
n = moles of gas
R = ideal gas constant (0.0821 L*atm/mol*K)
T = temperature in kelvin (K)

n = PV/RT

(5 atm)(25.0L) / (0.0821)(100K) = moles

convert moles to grams : n (moles) = g/molar mass