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A solution contains 82.0 g of glucose (C6H12O6) in 322 g water. Calculate the vapor pressure lowering at 25oC. The vapor pressure of pure water at 25o is 23.76 mmHg.
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I calculated that there is 41/90 mol glucose and 92/3 mol water. Then I calculated the molar fraction of solvent in the solution, which I found to be .985. Next I multiplied the .985 by 23.76 mmHg and came up with 23.4 mmHg. To find the "lowering," I subtracted this from 23.76 coming up with a final answer of
.348 mmHg.
Assuming I didn't make any arithmetic errors, is my process correct?
Thank you.
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