The compound is C₆H₁₂O₄. Using approximate atomic masses (C=12, H=1, O=16): Mass of C in one molecule = 6 12 = 72 Mass of H in one molecule = 12 1 = 12 Mass of O in one molecule = 4 16 = 64 Total mass of one molecule (or molar mass) = 72 + 12 + 64 = 148.Let's evaluate the options: A) 22 atoms per mole: One molecule contains 6 + 12 + 4 = 22 atoms. One mole contains Avogadro's number of molecules, so one mole contains 22 Avogadro's number of atoms, not just 22 atoms. Incorrect. B) twice the mass percent of H as compared to the mass percent of C: Mass of C is 72, Mass of H is 12. Is %H = 2 %C? (12/148)100% vs 2 (72/148)100%. This simplifies to 12 vs 272=144. Clearly incorrect. Is %C = 2 %H? 72 vs 212=24. Incorrect. C) six times the mass percent of C as compared to the mass percent of H: This is poorly phrased but implies a ratio. Let's check if %C = 6 %H. Mass of C is 72, Mass of H is 12. 72 = 6 12. Yes, the mass of Carbon in the compound is six times the mass of Hydrogen. Since the mass percentages are (mass of element / total mass) 100%, if Mass of C = 6 Mass of H, then %C = 6 %H. This holds true. D) thrice the mass percent of H as compared to the mass percent of O: Mass of H is 12, Mass of O is 64. Is %O = 3 %H? 64 vs 312=36. Incorrect. Is %H = 3 %O? 12 vs 364. Incorrect.Option C is the only statement that accurately reflects the mass composition of the compound, interpreting "six times the mass percent of C as compared to the mass percent of H" as the mass percent of C being six times the mass percent of H.