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Heres the question:

A 6L flask containing carbon monoxide at 200kPa is connected by a closed stopcock to a 3L flask containing oxygen gas at 800kPa. If the stopcock is opened, calculate the pressure of the system, assuming constant temperature.

a) if no chemical reaction occurs

b) if a small amount of an appropriate catalyst is present

The balanced equation for this reaction is:

2 CO + O2 --> 2 CO2

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ok, i can do the first question. I found the partial pressures of each, and obtained an answer of 400kPa. Im stuck on the second question. Heres my working:

V(CO, 200kPa)=6L

[tex]\therefore[/tex] V(CO2, 200kPa)=6L

That working is according to gay-lussacs law. But that pressure of 200kPa is for 6L, and i need 9, so i did [tex]frac{200\times 6}{9}=133.33kPa[\tex], but that is incorrect. According to the book, the answer is 333.3kPa. Any help?

Thanks,

Dan.

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# Homework Help: Reacting Gases

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