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anonymous
 one year ago
A mixture of .150 moles of C is reacted with .117 moles of O2 in a sealed, 10.0 L vessel at 500K, producing a mixture of CO and CO2. The total pressure is .640 atm. What is the partial pressure of CO?
anonymous
 one year ago
A mixture of .150 moles of C is reacted with .117 moles of O2 in a sealed, 10.0 L vessel at 500K, producing a mixture of CO and CO2. The total pressure is .640 atm. What is the partial pressure of CO?

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anonymous
 one year ago
Best ResponseYou've already chosen the best response.0@dan815 can you help?

NathalyN
 one year ago
Best ResponseYou've already chosen the best response.0150 moles of C is reacted with .117 moles of O2 Let CO = moles CO formed and CO2 = moles CO2 formed CO + CO2 = .150, by conserving carbon atoms CO + 2CO2 = .117 x 2 = .234, by conserving oxygen atoms. Two linear equations in two unknowns you can solve. Once you know moles CO you just PV = nRT > P = nRT/V; just ignore CO2 as you want partial pressure of CO only Actually, this problem is overspecified, ie has more information than is required to precisely define it [and the problem can be that the data are not consistent] So by the above method use CO2 to find the partial pressure of CO2 and add it to that of CO and see if you get .640 atm; if you do not, then the data are inconsistent. CO and CO2 will be pretty ideal under those conditions.

NathalyN
 one year ago
Best ResponseYou've already chosen the best response.0does this answer yuor question

NathalyN
 one year ago
Best ResponseYou've already chosen the best response.0@onegirl does that answer your question

NathalyN
 one year ago
Best ResponseYou've already chosen the best response.0okay can you give me a medalplease
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