stoichiometry

2. Shows equal numbers of atoms of each element on each side of the equation.
4. Numbers placed in front of the chemical formulas for the reactants and products of a reaction to balance the equation.
9. A unit used to measure the amount of a substance; one mole contains 6.02 × 10²³ particles.
13. 6.02 × 10²³ formula units of a substance in one mole.
14. The substances formed as a result of a chemical reaction.
16. States that the total mass of the products of a chemical reaction is the same as the total mass of the reactants.
17. The quantity of product actually obtained from a reaction, which is always less than or equal to the theoretical yield.
18. A reactant that is completely consumed in a reaction, which stops the reaction.
19. The formula weight of a molecular formula.
20. The sum of the atomic weights of the atoms in a compound’s formula.

1. Compares the actual yield to the theoretical yield using the equation.
3. Reactions in which two reactants combine to form one product.
5. Reactions in oxygen in which a substance, typically a hydrocarbon, reacts rapidly with O₂ to form CO₂ and H₂O.
6. The quantity of product calculated to form when all of the limiting reactant reacts.
7. A technique for determining the empirical formulas of compounds containing only carbon, hydrogen, and/or oxygen.
8. The starting substances in a chemical reaction that undergo change.
10. The study of the quantitative relationships between chemical equations.
11. Can be determined from a substance’s percent composition by calculating the relative number of moles of each atom in 100 g of the substance.
12. Reactions in which a single reactant forms two or more products.
15. The mass of one mole of atoms, molecules, or other formula units expressed in grams.