| A compound has the empirical formula\[{{C}_{10}}{{H}_{8}}Fe\]. A solution of 0.26 g of the compound in 11.2 g of benzene \[({{C}_{6}}{{H}_{6}})\] boils at \[\text{8}0.\text{26}{}^\circ \text{C}\]. The boiling point of benzene is \[\text{8}0.\text{1}0{}^\circ \text{C}\] and \[{{K}_{b}}\] is \[\text{2}.\text{53}{}^\circ \text{C}/\text{molal}.\] |
| What is the molecular formula of the compound? |
A) \[{{C}_{30}}{{H}_{24}}F{{e}_{3}}\]
B) \[{{C}_{10}}{{H}_{8}}Fe\]
C) \[{{C}_{5}}{{H}_{4}}Fe\]
D) \[{{C}_{20}}{{H}_{16}}F{{e}_{2}}\]
Correct Answer: D
Solution :
| [d] \[\Delta {{T}_{b}}=80.26\] |
| \[0.16=2.53\times \frac{0.26/M}{11.20}\times 1000;\]\[M\approx 367\] |
| This is almost equal to molar mass of \[{{C}_{20}}{{H}_{16}}F{{e}_{2}}\]. |
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