SolutionHard
Question
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°C. What is the molecular formula of the solute? (Kf = 1.86°C kg mol−1)
Options
A.C6H12O6
B.C3H6O3
C.CH2O
D.C2H4O2
Solution
$\Delta T_{f} = K_{f}.m \Rightarrow 0.93 = 1.86 \times \frac{36/M}{1.2} \Rightarrow M = 60$
If the molecular formula is CxH2xOx, then
12x + 2x + 16x = 60 ⇒ x = 2
∴ Molecular formula = C2H4O2
Create a free account to view solution
View Solution FreeMore Solution Questions
An ideal solution is obtained by dissolving n moles of non-volatile, non-electrolyte solute in N moles of solvent. If th...A mixture of liquids ‘A’ and ‘B’ in the molar ratio 1: 2 forms a maximum boiling azeotrope. Identify the incorrect state...The vapour pressure of a dilute aqueous solution of glucose is 750 mm of mercury at 373 K. The mole fraction of solute i...The vapour pressure of pure liquid solvent A is 0.80 atm. When a non-volatile substance B is added to the solvent, its v...Which statement about the triple point of a substance is/are incorrect...