A 100.0 ml flask contains 510. g of N2 at 0 degrees c. What is the pressure in atm, torr, psi

PV = nRT

We are solving for pressure. We are given the volume, which is 0.100 L (equivalent to 100 mL). The temperature is 273.15 K (equivalent to 0 Celsius). All we need to do is convert the grams to moles before we can solve for pressure.

N₂ has a molecular mass of 28.02. This means that 510 g N₂ * (1 mole N₂/28.02 g N₂) = 18.2 moles N₂

PV = nRT

P = nRT/V

R is the gas constant. R = 0.08206 atm*L / (K*mol)

P = (18.2 mol) * (0.08206 atm*L / (K*mol)) * (273.15 K) / (0.100 L)

P = 4.08 * 10^3 atm

The pressure is 4.08*10^3 atm.