Question

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Answer 1

Answer:

the answer is CH2

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Answer 2

Answer:

CH

Explanation:

We assume 100 g of compound, and divide thru by the atomic masses:

92.3⋅g12.011⋅g⋅mol−1 = 7.65⋅mol⋅C

7.69.3⋅g1.00794⋅g⋅mol−1 = 7.65⋅mol⋅H

So, clearly, the empirical formula is CH.

But we have been given a molecular mass, and it is a fact that the molecular formula is always a multiple of the empirical formula:

Molecular formula = n×(empirical formula)

26⋅g⋅mol−1 = n×(12.011+1,00794)⋅g⋅mol−1

Clearly, n = 2, and molecular formula = C2H2, likely acetylene, HC≡CH.