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A solution is prepared by mixing 0.0200 mol CH2Cl2 and 0.0300 mol 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.

2007-02-11 00:18:35 · 1 answers · asked by Anonymous in Science & Mathematics Chemistry

1 answers

I have already answered this question today, but I'll answer it again for you.

The total number of moles is 0.05, and so the moles fractions are .04 and 0.6 respectively.

Now all you have to do is to work out:

(0.4 x 133) + (0.6 x 11.4).

Over to you!

2007-02-11 01:22:28 · answer #1 · answered by Gervald F 7 · 0 0

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