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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) =?
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The first-order decomposition of N2O5 proceeds as follows: 2 N2O5 (g) → 4 NO2 (g) + O2
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