At room temperature, a dilute solution of urea is prepared by dissolving 0.60 g of urea in 360 g of water. If the…
Solutions · Class 12 · JEE Main Previous Year 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)
- a
0.028 mm Hg
- b
0.027 mm Hg
- c
0.031 mm Hg
- d✓
0.017 mm Hg
0.017 mm Hg
Strategy:\n> Lowering of vapour pressure () is given by Raoult's Law: . Calculate the mole fraction of urea in the water.\n\nStep 1: Calculate moles of solute and solvent\n- \n- \n\nStep 2: Determine the mole fraction ()\n\n\nStep 3: Calculate narrowing of vapour pressure\n\n\n\n
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