Question

A 1.0 L container was filled by pumping into it 1.0 L of N2 at 20.0cm Hg, 1.00 L of O2 at 155 torr, and 1.0 L of He at 0.450 atm. All volumes and pressures were measured at the same temperature. What was the total pressure inside the container after the mixture was made? For some reason my book lists this as a difficult problem but I got the answer 697 torr. My question is what implications does contant temperature have to do with the mixture. If it had a different temperature for every gas would you use the ideal gas law?

Answer 1

Answer: According to the question here first we have to write the balanced equation :

  N2 (g) + O2 (g) --> 2 NO (g)

And we know that 1 cm Hg = 10 torr so , 20 cm hg = 200 torr

Now the Ptotal = Pa + Pb

P of N2 = 200 / 0.5 = 400 torr

P of O2 = 155 / 0.5 = 310 torr

Basically , here you have to use the henry's law . and there is no effect of the inert gas .

hence the total pressure is found to be 710 torr . So , it is all about the given question .

Thank you :)