When 36.0 g of a solute having the empirical formula CH₂O is dissolved in 1.20 kg of water the solution freezes at -0.93^oC. what is the molecular formula of the solute?
(K_f = 1.86^oC kg mol^-1)

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C₂H₄O₃

C₂H₄O

C₂H₄O2

C₂H₂O₂

answer is D.

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Detailed Solution

$\begin{aligned} {ΔT}_{f} = K_{f} \cdot m \Rightarrow 0 .93 = 1 .86 \times \frac{36}{M} \times \frac{1}{1 .2} \\ M = 60 and 30 \times n = 60; ∴ n = 2 \end{aligned}$
so compound is C₂H₄O₂.

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