Question

The empirical formula and molecular mass of a compound are $C{H}_{2}O$ and $180\mu$ respectively. What will be the

• A. $C_9{H}_{18}O$
• B. $C{H}_{2}O$
• C. $C_2{H}_4{O}_2$
• D. $C_6{H}_{12}{O}_6$

Answer 1

The correct option is D $C_6{H}_{12}{O}_6$

Calculating empirical formula mass

Empirical formula = $C{H}_{2}O$

Empirical formula mass =

$=12+(1\times 2)+16$
$=12+2+16=30\mu$

Determining molecular formula

Given molecular mass = $180\mu$

Molecular formula = $(C{H}_{2}O{)}_n$

Where value of n = $\frac{Molecularmass}{empiricalmass}=\frac{180}{30}=6$

Thus, value of n = 6
Molecular formula = $(C{H}_{2}O{)}_6=C_6{H}_{12}{O}_6$

Thus, for empirical formula $C{H}_{2}O$ and molecular mass 180 $\mu$, molecular formula is $C_6{H}_{12}{O}_6$.