At room temperature, a dilute solution of urea is prepared by dissolving 0.60 g of urea in 360 g of water. If the vapour pressure of pure water at this temperature is 35 mm Hg, lowering of vapour pres

Question

At room temperature, a dilute solution of urea is prepared by dissolving 0.60 g of urea in 360 g of water. If the vapour pressure of pure water at this temperature is 35 mm Hg, lowering of vapour pressure will be:

(molar mass of urea = 60 g mol⁻¹)

Canvas Classes · Accepted Answer

Strategy:
 Lowering of vapour pressure () is given by Raoult's Law: . Calculate the mole fraction of urea in the water.

Step 1: Calculate moles of solute and solvent
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Step 2: Determine the mole fraction ()

Step 3: Calculate narrowing of vapour pressure

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