Question

Calculate the resulting pressure if 4.50 liters of nitrogen at 35.0C and 790 torr and 3.7 liters of oxygen at 15.0C and 750 torr are pumped into a 1.00 liter container at 25.0C. Assume ideal gas behavior.

Answer 1

no of mole of N2 = PV/RT

     = (790/760)*4.5/(0.0821*308)

    = 0.185 mole

no of mole of O2 = PV/RT

     = (750/760)*3.7/(0.0821*288)

    = 0.154 mole

total no of mole of gas mixture = 0.154 + 0.185 = 0.339 mole

resulting pressure (P) = nRT/V

              = 0.339*0.0821*298/1

          = 8.29 atm