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1 mole of a non-volatile solid is dissolved in 200 moles of water. The solution in taken to a temperature \( T_{K} \) (lower than the freezing point of solution) to cause ice formation. After removal of ice, the remaining solution is taken to \( 373 \mathrm{~K} \) where vapour pressure is observed to be 740 \( \mathrm{mm} \) of \( \mathrm{Hg} \). Identify the correct option.
[Given data: \( \mathrm{K}_{\mathrm{f}}\left(\mathrm{H}_{2} \mathrm{O}\right)=2 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1} \) and normal boiling point of \( \mathrm{H}_{2} \mathrm{O}=373 \mathrm{~K} \).]
(a) 163 moles of ice will be formed.
(b) \( \mathrm{T}_{\mathrm{k}}=373-\frac{2000}{37 \times 18} \mathrm{~K} \).
(c) Freezing point of original solution should be \( -\frac{10}{18}{ }^{\circ} \mathrm{C} \).
(d) Relative lowering of vapour pressure of final solution will be \( \frac{1}{201} \).
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