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Q.

A compound has the empirical formula $C_{10} H_{8} F e$ . A solution of 0.26 g of the compound in 11.2 g of benzene $(C_{6} H_{6})$ boils at ${80.26}^{\circ} C$ . The boiling point of benzene is ${80.10}^{\circ} C$ ; the $K_{b}$ of benzene is ${2.53}^{\circ} C / m o l a l$ . What is the molecular formula of the compound? (Atomic mass of Fe: 56)

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a

$C_{10} H_{8} F e$

b

$C_{20} H_{16} F e_{2}$

c

$C_{30} H_{24} F e_{3}$

d

$C_{5} H_{4} F e$

answer is D.

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Detailed Solution

$T_{b} = 80.26, Δ T_{b} = 0.16 0.16 = 2.53 \times \frac{0.26 / M}{11.20} \times 1000; M \approx 367$

That is almost molar mass of $C_{20} H_{16} F e_{2}$

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A compound has the empirical formula C10H8Fe. A solution of 0.26 g of the compound in 11.2 g of benzene (C6H6) boils at 80.26∘C. The boiling point of benzene is 80.10∘C; the Kb of benzene is 2.53∘C/molal. What is the molecular formula of the compound? (Atomic mass of Fe: 56)