Chemical Reactions and Stoichiometry Quiz

Study Notes

Stoichiometry: Quantitative study focused on reactants and products in chemical reactions.
Chemical Equations: Represent reactions with reactants on the left and products on the right.
Balancing Equations: Essential to maintain mass; uses coefficients (numbers in front) and subscripts (numbers in formula).

Combination Reaction: Involves two or more substances combining to form a single product.
Decomposition Reaction: A single substance breaks down into two or more simpler substances.
Combustion Reaction: Rapid reactions, typically involving hydrocarbons and oxygen, producing carbon dioxide and water.

Percent Composition: Calculated as ((\text{number of atoms} \times \text{atomic weight}) / \text{FW of the compound} \times 100).
Formula Weight: Sum of atomic weights of all elements in a chemical or empirical formula.
Molecular Weight: Total of atomic weights for atoms in a molecule.

Mole: A unit for measuring chemical quantities, equating to Avogadro's number (approximately (6.022 \times 10^{23}) entities).
Molar Mass: The mass of one mole of a substance, expressed in grams per mole (g/mol).

Determining Empirical Formula: Start with mass percent of elements, convert to grams, use molar mass to find moles, and calculate mole ratios.
Molecular Formula from Empirical Formula: Molecular formula shows multiples of the empirical formula based on molecular weight divided by empirical formula weight.

Limiting Reactant: The reactant that is present in the smallest stoichiometric amount, limiting product formation.
Excess Reactant: The reactant that remains after the reaction is complete.
Theoretical Yield: Maximum possible product amount based on stoichiometric calculations.
Actual Yield: Measured amount of product actually produced in a reaction.
Percent Yield: A measure of efficiency, calculated by ((\text{Actual Yield}/\text{Theoretical Yield}) \times 100).