A compound has an empirical formula of CH and a molecular ion at m/z = 26. The compound could be

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Re-stating the problem: a compound has an empirical formula of CH and a molecular ion at m/z = 26, and we must choose among four options.
Option a. ethyne: This is C2H2. The empirical formula CH corresponds to a 1:1 ratio of C to H. A molecular formula that is a simple multiple of CH could be C2H2 (twice the empirical unit). The molecular ion mass would be 2×12 (carbon) + 2×1 (hydrogen) = 24 + 2 = 26, which matches the given m/z. Therefore, ethyne (C2H2) is consistent with the data.
Option b. propyne: This molecule is C3H4. Its empirical formula would be CH0.67 or more simply not matching CH as a whole-number ratio; moreover, the molar mass would be 3×12 + 4×1 = 36 + 4 = 40, which does not align with m/z 26. Hence this cannot fit the given empirical formula or mass.
Option c. ethane: This is C2H6. The empirical formula would reduce to CH3, not CH, so the empirical formula would not be CH. Its molar mass is 2×12 + 6×1 = 24 + 6 = 30, which again does not match m/z 26. Therefore this option is inconsistent with the data.
Option d. ethene: This is C2H4. The empirical formula would reduce to CH2, not CH, so the empirical formula would not be CH. Its molar mass is 2×12 + 4×1 = 24 + 4 = 28, which does not match the observed m/z 26. Thus this option is also incompatible with the given information.
In summary, only the formulation C2H2 aligns with an empirical CH and a molecular ion at m/z 26, while the other choices fail to satisfy either the empirical formula constraint or the mass specification.

A compound has an empirical formula of CH and a molecular ion at m/z = 26. The compound could be

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