The molecular formula for [tex]CH_{2}[/tex] carrying a molar mass of 112 g/mol would be:
- [tex]C_{8} H_{16}[/tex]
Given that,
Empirical Formula of the compound [tex]=[/tex] [tex]CH_{2}[/tex]
The molar mass of the compound [tex]= 112 g/mol[/tex]
As we know,
Empirical Mass = [tex]12 + 2[/tex]
[tex]= 14[/tex]
It is known that,
Molar mass [tex]= n[/tex] × [tex]empirical mass[/tex]
∵ [tex]n = molar mass/empirical mass[/tex]
[tex]= 112/14[/tex]
[tex]= 8[/tex]
∵ The Molecular Formula of the compound would be determined by multiplying n into the empirical formula,
so,
Molecular Formula = [tex]n[/tex] × [tex]emprical formula[/tex]
[tex]=[/tex] ([tex]CH_{2}[/tex]) × [tex]8[/tex]
= [tex]C_{8} H_{16}[/tex]
Thus, [tex]C_{8} H_{16}[/tex] is the correct answer.
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