Question

163.26 g/mol, c₁₁h₁₇n
express your answer as a chemical formula.
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part b
186.24 g/mol, c₆h₇n
express your answer as a chemical formula.
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submit

Explanation:

Step1: Calculate the molar mass of the empirical formula

The empirical formula is \(C_6H_7N\).
The molar mass of \(C\) is \(12.01\space g/mol\), of \(H\) is \(1.008\space g/mol\), and of \(N\) is \(14.01\space g/mol\).

$$M_{empirical}=(6\times12.01)+(7\times1.008)+14.01$$

$$M_{empirical}=72.06 + 7.056+14.01$$

$$M_{empirical}=93.126\space g/mol$$

Step2: Find the ratio of molar masses

The molar mass of the compound is \(M = 186.24\space g/mol\)

$$n=\frac{M}{M_{empirical}}=\frac{186.24}{93.126}\approx2$$

Step3: Determine the molecular formula

Multiply the sub - scripts in the empirical formula by \(n = 2\)
The molecular formula is \(C_{6\times2}H_{7\times2}N_{1\times2}=C_{12}H_{14}N_2\)

Answer:

\(C_{12}H_{14}N_2\)