We can be sure that a mole of table sugar (C12H22O11) and a mole of vitamin C (C6H8O6) are equal in their:

• A. number of molecules
• B. volume occupied at STP
• C. mass in grams
• D. number of carbon atoms

Answer: (A)

Verified step by step guidance

1. Recall the definition of a mole: one mole of any substance contains Avogadro's number of particles (molecules, atoms, ions, etc.), which is approximately \$6.022 \times 10^{23}$ particles.
2. Since both table sugar (C12H22O11) and vitamin C (C6H8O6) are given in moles, one mole of each contains the same number of molecules, regardless of their chemical formula or molecular weight.
3. Understand that the mass in grams of one mole of each substance is different because their molar masses differ. Calculate molar mass by summing the atomic masses of all atoms in the molecular formula.
4. Recognize that volume occupied at STP (Standard Temperature and Pressure) applies specifically to gases, so it is not relevant for solids like table sugar and vitamin C.
5. Note that the number of carbon atoms differs because one molecule of table sugar has 12 carbon atoms, while one molecule of vitamin C has 6 carbon atoms, so one mole of each will have different total carbon atoms.