Stoichiometry Test

Stoichiometry

The study of quantitative relationships between reactants and products in a chemical reaction.

Limiting Reactant

The reactant that controls the amount of product formed.

Excess Reactant

A reactant that is left over after the reaction is complete.

Coefficients in a balanced chemical equation

Indicate both the number of molecules and the number of moles.

Law of Conservation of Mass

The total mass of reactants equals the total mass of products.

Amount of Product Formation Determiner

The limiting reactant.

Haber Process Ratio

For every 2 moles of ammonia produced, 6 moles of hydrogen are consumed.

Conservation of Mass in Chemical Reactions

The mass of reactants equals the mass of products.

Solution

A homogeneous mixture of two or more pure substances.

Solute

The substance being dissolved in a solution.

Solvation

The process in which solvent particles pull solute particles apart and surround them.

Dissolution of Ionic Compounds

Ionic compounds dissolve in water due to ion-dipole interactions that overcome the lattice energy.

Like Dissolves Like Principle

Substances with similar intermolecular forces tend to dissolve in each other.

Vitamin A Solubility

It is soluble in fat but not in water due to its mostly nonpolar structure.

Unsaturated Solution

A solution that contains less solute than the maximum amount that can dissolve at a given temperature.

Supersaturated Solution

Contains more solute than would normally dissolve at that temperature.

Molarity (M) Definition

Moles of solute per liter of solution.

Dissolution vs. Chemical Reactions

Dissolution is a physical change where the original solute can be recovered.

KNO₃ Cooling Experiment Outcome

Approximately 30g of KNO₃ will precipitate out of solution when cooled.

Solubility of Cerium Sulfate at High Temperatures

Decreasing solubility as temperature increases is explained by ion-dipole interactions.

Resulting Concentration after Water Evaporation

The solute particles will be twice as concentrated, but the solution will remain unsaturated.

Solvent

A substance that dissolves a solute, resulting in a solution. Solvents are usually liquids but can also be gases or solids.

Mixture

A combination of two or more substances that are not chemically bonded. Mixtures can be homogeneous or heterogeneous.

Precipitate

A solid that forms and separates from a liquid solution during a chemical reaction.

Crystallization

The process by which a solid forms from a solution, resulting in the formation of a crystal structure. Crystallization occurs when the concentration of a solute exceeds its solubility.

Solvation

The process by which solvent molecules surround and interact with solute particles, facilitating their dispersion in a solution.

Precipitation

The process by which a solid forms from a solution during a chemical reaction, typically when the concentration of the solute exceeds its solubility.

Dissolution

The process by which a solid solute dissolves in a solvent to form a homogeneous solution, involving the interaction of solute and solvent molecules.