Answer:
[tex]C_{6} H_{6}[/tex]
Explanation:
First, find the mass of empirical formula, CH. 12.01 g/mol is for carbon, and 1.008 g/mol is for hydrogen. 12.01+1.008=13.018 G/mol CH. Divide 78.110 G/mol by 13.018 g/mol. You get approximately 6. Multiply that by the subscript of each element. 6(CH)=
[tex]C_{6} H_{6}[/tex]
The molecular formula of the compound with an empirical formula of CH and a molar mass of 78.110g/mol is C₆H₆.
We want to determine the molecular formula of the compound with an empirical formula of CH and a molar mass of 78.110g/mol. First, we will calculate the molar mass of the empirical formula.
[tex]M(empirical\ formula) = M(C) + M(H) = 12.01 g/mol + 1.01 g/mol = 13.02g/mol[/tex]
Then, we will calculate the coefficient "n".
[tex]n = \frac{molar\ mass\ molecular\ formula }{molar\ mass\ empirical\ formula} = \frac{78.110g/mol}{13.02g/mol} \approx 6[/tex]
Finally, we will multiply the empirical formula by "n" to get the molecular formula.
[tex]CH \times 6 = C_6H_6[/tex]
The molecular formula of the compound with an empirical formula of CH and a molar mass of 78.110g/mol is C₆H₆.
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