The picture below shows two bulbs connected by a stopcock. The 6.00-L bulb conta

Question

The picture below shows two bulbs connected by a stopcock. The 6.00-L bulb contains nitric oxide at a pressure of 0.50o 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(g) -> 2NO2(g)

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

Which gases are present at the end of the experiment?

What are the partial pressures of the gases?

If the gas was consumed completely, put 0 for the answer.

Pno ? Po2?? Pno2?

The picture below shows two bulbs connected by a stopcock. The 6.00-L bulb contains nitric oxide at a pressure of 0.50o 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(g) -> 2NO2(g) Determine which gases remain after the reaction goes to completion and calculate their partial pressures. The temperature at the beginning and the end of the experiment is 22 ½C. Which gases are present at the end of the experiment? What are the partial pressures of the gases? If the gas was consumed completely, put 0 for the answer. Pno ? Po2?? Pno2?

Explanation / Answer

To determine partial pressures in a reaction of these reactive gases in an isolated system (bulbs) reacting the following compounds where:

2NO + O2> 2NO2

Facts:no. mol 2NO= 2 mol
no. mol O2= 1 mol
no. mol 2NO2= 2 mol
R= 0.082 atm.L/k.mol
T= 22

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