CHE 211 Lesson 6: Percent Composition and Empirical Formula

These flashcards cover key concepts related to the percent composition and empirical formulas discussed in Lesson 6 of CHE 211.

Percent Composition

The percentage by mass of each element in a compound.

Molar Mass

The mass of one mole of a substance, typically expressed in grams per mole (g/mol).

Empirical Formula

The simplest whole-number ratio of elements in a compound.

Molecular Formula

A chemical formula that shows the number and types of atoms in a molecule, which may be a multiple of the empirical formula.

Transition Metal

Metals that have partially filled d orbitals, capable of forming various oxidation states and compounds.

Iron Oxides

Compounds formed from iron and oxygen, such as FeO, Fe2O3, and Fe3O4.

Calculating Percent by Mass

Formula to determine the percentage of an element in a compound: %X = (mass of X / total mass) * 100.

Dividing by Smallest Number of Moles

A step in determining the empirical formula where each element's moles are divided by the smallest mole value.

Combining Atom Ratio

The ratio of different atoms in a compound, which is crucial for deriving the empirical formula.

Vitamin C Composition

Percent mass data including 40.9% C, 54.5% O, 4.58% H, with a molar mass of 176 g/mole.