A100.0 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.

the answer is the first option

explanation:

just googled it m8. not that hard

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