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A compound has an empirical formula $C_2H_4O$.An independent analysis gave a value of 132.16 for its molecular mass.What is the correct molecular formula ?

$\begin{array}{1 1}(a)\;C_4H_4O_5&(b)\;C_{10}H_{12}\\(c)\;C_7O_3&(d)\;C_6H_{12}O_3\end{array}$

Can you answer this question?

Empirical formula mass=$2\times 12+4+16$
$\qquad\qquad\qquad\qquad=44$
Molecular formula=$(C_2H_4O)_n$
$n=\large\frac{Mol.mass}{Emp.mass}$
$\;\;=\large\frac{132.16}{44}$
$\;\;=3$(approx)
$\therefore$ Molecular formula =$(C_2H_4O)_3=C_6H_{12}O_3$
Hence (d) is the correct answer.
answered Oct 24, 2013