Problem: A solution is prepared by mixing 0.0300 mole of CH2Cl2 and 0.0500 mole of CH2Br2 at 25°C. Assuming the solution is ideal, calculate the composition of the vapor (in terms of mole fractions) at 25°C. At 25°C, the vapor pressures of pure CH2Cl2 and pure CH2Br2 are 133 and 11.4 torr, respectively.

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FREE Expert Solution

Mole Fraction (X) relates the moles of each species in a mixture:

mole fraction (X)=mole of componenttotal moles


 Calculate the mole fraction.

0.0300 mole of CH2Cl2

0.0500 mole of CH2Br2 


mole fraction(X)=mole of componentTotal moleXCH2Cl2=mole CH2Cl2mole CH2Cl2 +mole CH2Br2 XCH2Cl2=0.030 mol0.030 mol +0.050 mol XCH2Cl2=0.030 mol0.080 mol 

XCH2Cl2 = 0.375


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Problem Details

A solution is prepared by mixing 0.0300 mole of CH2Cl2 and 0.0500 mole of CH2Br2 at 25°C. Assuming the solution is ideal, calculate the composition of the vapor (in terms of mole fractions) at 25°C. At 25°C, the vapor pressures of pure CH2Cl2 and pure CH2Br2 are 133 and 11.4 torr, respectively.