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