if a compound has a molar mass of 180 g/mol and its empirical formula is ch₂o, what is its molecular…

Answer:

C. $C_6H_{12}O_6$

Explanation:

Step1: Calculate empirical formula mass

The empirical formula is $CH_2O$. The atomic masses of $C = 12\ g/mol$, $H= 1\ g/mol$, $O = 16\ g/mol$. So the empirical - formula mass $M_{empirical}=(12\times1)+(1\times2)+(16\times1)=30\ g/mol$.

Step2: Find the ratio $n$

The molar mass of the compound $M_{molecular}=180\ g/mol$. The ratio $n=\frac{M_{molecular}}{M_{empirical}}=\frac{180\ g/mol}{30\ g/mol}=6$.

Step3: Determine molecular formula

Multiply the sub - scripts in the empirical formula by $n$. The empirical formula is $CH_2O$, so the molecular formula is $(CH_2O)6 = C_6H{12}O_6$.