Explain boiling point of water at atmospheric pressure

Reference no: EM13548813

A solution consists of 360g of sucrose and 144g of water. Assume that the solution follows Raoult's law and that the vapor pressure of sucrose is negligible. The normal boiling point of water at atmospheric pressure is 100C. The molecular weight of sucrose is 180.

A) What is the mole fraction of water in solution?

B) What is the mole fraction of sucrose in solution?

C) If the solution is heated to 100C, what will be the vapor pressure of the water rising from the solution?

D) Will the solution boil at this temperature? (Hint: for a solution to boil at atmospheric pressure, the vapor pressure must be equal to 760 mm Hg). What does this tell you about the boiling point of a sucrose solution? Is it going to be higher or lower than 100C?

Reference no: EM13548813

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