The picture below shows two bulbs connected by a stopcock. The 6.00-L bulb contains nitric oxide at a pressure of 0.750 atm, and the 1.50-L bulb contains oxygen at a pressure of 2.50 atm.

After the stopcock is opened, the gases mix and react: 2NO(g) + O2 >>>> 2NO2(g)

Determine which gases remain after the reaction goes to completion and calculate their partial pressures. The temperature at the beginnning and the end of the experiment is 22 °C.

Which gases are present at the end of the experiment? (the answer is O2 and NO2)

Here is what I can't figure out:

What are the partial pressures of the gases? If the gas was consumed completely, put 0 for the answer.

P(NO)= 0, P(O2)=.2, so what does P(NO2) =?