We can be sure that a mole of table sugar and a mole of vitamin C are equal in theira. mass.b. volume.c. number of atoms.d. number of molecules.

Verified step by step guidance

1. Identify the concept of a mole in chemistry, which is a unit that measures the amount of substance.
2. Understand that one mole of any substance contains Avogadro's number of entities, which is approximately \(6.022 \times 10^{23}\).
3. Recognize that these entities can be atoms, molecules, ions, etc., depending on the substance.
4. Consider that a mole of table sugar and a mole of vitamin C both contain the same number of molecules, as they are both measured in moles.
5. Conclude that the correct answer is related to the number of molecules, as a mole is defined by the number of entities, not by mass or volume.

Key Concepts

Mole Concept

The mole is a fundamental unit in chemistry that quantifies the amount of substance. One mole contains approximately 6.022 x 10^23 entities, which can be atoms, molecules, or ions. This concept allows chemists to relate mass and number of particles in a substance, making it essential for stoichiometric calculations.

Molecular Composition

Molecular composition refers to the types and numbers of atoms that make up a molecule. For example, table sugar (sucrose) has a different molecular formula than vitamin C (ascorbic acid), leading to different properties. Understanding molecular composition is crucial for comparing substances at the molecular level.

Avogadro's Law

Avogadro's Law states that equal volumes of gases, at the same temperature and pressure, contain an equal number of molecules. This principle extends to all substances, indicating that one mole of any substance contains the same number of molecules, regardless of the substance's mass or volume. This is key to understanding why a mole of sugar and a mole of vitamin C are equal in the number of molecules.