What is the pressure of N2 (g) in Torr if 0.58 atm of O2 (g) and 1260 mmHg of He(g) are mixed with the nitrogen, and the total pressure is 2650 mmHg?

Answer 1

Just convert the oxygen pressure to torr, since torr = mmHg: (0.58 atm O₂) * (1 atm / 760 torr) = 441 torr O₂. Then partial pressure of N₂ = 2650 - 441 - 1260 = 949 torr N₂.