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GreatEscapist
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Homework Statement
A gaseous mixture containing 0.190 mol fraction of carbon tetrachloride (CCl4) and 0.810 mol fraction of dry air is initially at 62.0°C and 1141 mmHg. If this mixture is cooled at a constant pressure, at what temperature does the CCl4 first start to condense? I already did this problem
At what temperature would 56.0% of the CCl4 condense?
Homework Equations
Partial pressure = p*(T)
log10(p*)= A + (B/(T+C))
I'm sure there are more I'm supposed to use
The Attempt at a Solution
After solving for the original problem, for the second, I know that I need to find how many moles are condensed...but I don't know how to do that. Or what to do after that, or with that information.