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

🧠 Dilute Urea Solution — Direct Raoult Lowering Calculation

Read the question. Urea is non-electrolyte (). Dilute solution (small amount of solute), so use Raoult's dilute approximation:

Find  and , then compute .

🗺️ Working It Out

Moles of urea: .

Moles of water: .

Relative lowering:

Absolute lowering:

Matches option (d).

⚡ The Smart Move

For "dilute solution VP lowering" questions, the compact formula:

Plug in: . One line.

The dilute approximation is valid here because  —

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