a sample of a compound contains 60.0 g c and 5.05 g h. its molar mass is 78.12 g/mol. what is the compounds…

Explanation:

Step1: Calculate moles of C

Moles of C = $\frac{\text{mass of C}}{\text{molar - mass of C}}=\frac{60.0\ g}{12.01\ g/mol}\approx5.0\ mol$

Step2: Calculate moles of H

Moles of H = $\frac{\text{mass of H}}{\text{molar - mass of H}}=\frac{5.05\ g}{1.01\ g/mol}\approx5.0\ mol$

Step3: Find the empirical - formula ratio

The ratio of C to H is $\frac{5.0\ mol}{5.0\ mol}=1:1$, so the empirical formula is CH.

Step4: Calculate the empirical - formula mass

Empirical - formula mass of CH = $12.01\ g/mol+1.01\ g/mol = 13.02\ g/mol$

Step5: Find the multiple (n)

$n=\frac{\text{molar mass}}{\text{empirical - formula mass}}=\frac{78.12\ g/mol}{13.02\ g/mol}=6$

Step6: Determine the molecular formula

Molecular formula = (Empirical formula)$_n$=(CH)$_6$ = C$_6$H$_6$

Answer:

C₆H₆