[confusedman27]

A mixture of 0.154 moles of C is reacted with 0.117 moles of O2 in a sealed, 10 L vessel at 500 K, producing a mixture of CO and CO2. The total pressure is 0.6907 atm. What is the partial pressure of CO?

any help would be awesome.

[Arkcon]

I'd like to welcome you, confusedman27: to the Chemical Forums.  According to the Forum Rules{click}, we want to see your attempt, so please click on that link, read the contents, and comply with our rules, so we can help you.

The first thing you should do is try to write a balanced equation, which will be tricky, given how open ended your products are.  At any rate, start with what would happen if you had an abundance of oxygen, and try to see how in this case, you  don't and try to come up with what you'll get.

any help would be awesome.

You wrote that, so I'm going to hold you to it

[confusedman27]

Sorry about that. Been trying this problem for like a hour and a half

3 C (s) + 2O₂ = 2 CO₂ + CO₂

Ive gone at it a couple different ways. Got the moles of each, found the limiting being carbon. , and i just kinda get lost from there. Ive found similar problems on the internet and have followed there steps, found the exact problem on one site that said the answer was .458 atm. I did it myself and thats what i got but my homework keeps saying its wrong

[sjb]

Can you say how many moles of gas there are, at the end?

[confusedman27]

.103 mole CO? sorry if thats wrong. Im real lost

[sjb]

Sounds a bit low. What equations do you know that describe the behaviour of gases?

[confusedman27]

Im really not sure. I got that by dviding what i was given by the moles of it I had, and then using molar ratio of CO. I really have no idea where to go from here. I know you guys are asking the questions out of good intentions, but i really kinda need a roadmap on how to solve this. I dont know how much help i can be.

[sjb]

OK, using pV=nRT, how many moles of gas are there at the end? Formed from how many moles of carbon?