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When \( 36.0 \mathrm{~g} \) of a solute having the empirical formula \( \mathrm{CH}_{2} \mathrm{O} \) is dissolved in \( 1.20 \mathrm{~kg} \) of water, the solution freezes at \( -0.93^{\circ} \mathrm{C} \). What is the molecular formula of the solute? \( \left(K_{f}=1.86^{\circ} \mathrm{C} \mathrm{kg}\right. \) \( \left.\operatorname{mol}^{-1}\right) \)
(a) \( \mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O} \)
(b) \( \mathrm{C}_{2} \mathrm{H}_{2} \mathrm{O}_{2} \)
(c) \( \mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}_{3} \)
(d) \( \mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}_{2} \)
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