1. The problem statement, all variables and given/known data 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? 2. Relevant equations Partial pressure = p*(T) log10(p*)= A + (B/(T+C)) I'm sure there are more I'm supposed to use 3. 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.