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A solution contains 12.16g of chloroform (below: MW=119.38(g)/(m)ole ) and 9.58g of acetone (below: MW=58.08(g)/(m)ole ). If the vapor pressure of pure chloroform is 0.39atm
A solution contains
12.16g
of chloroform (below:
MW=119.38(g)/(m)ole
) and
9.58g
of acetone (below:
MW=58.08(g)/(m)ole
). If the vapor pressure of pure chloroform is
0.39atm
and that of pure acetone is
0.44atm
answer the following:\ a. Assuming ideal behavior what would the total vapor pressure be?\
x_(A)=x_(A)*P_(A)^(0)=x_(A)\\\\times 0.34atm=0.3818\\\\times 0.34=0.15\ P_(B)=x_(B)\\\\times P_(B)^(0)x_(B)\\\\times 0.44atm=0.6182\\\\times 0.14=0.27=0.42 toral \ P_(totul )=P_(1)+P_(2)
\ b. Based on molecular interactions between the species would you expect the actual vapor pressure to be above or below that calculated in a. Explain your answer.\ Acelone\ Chloratorm
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