Stoichiometry and Chemical Reactions
Studied by 0 people
Call with Kai
Knowt Play
Learn
Practice Test
Spaced Repetition
Match
Flashcards1/47
Earn XP
Description and Tags
These flashcards cover key vocabulary terms and definitions related to stoichiometry, chemical reactions, and solution chemistry.
Name | Mastery | Learn | Test | Matching | Spaced |
|---|
No study sessions yet.
48 Terms
Stoichiometry
The study of the numerical relationships between the quantities of reactants and products in a chemical reaction.
Reactants
The starting substances in a chemical reaction that are transformed into products.
Products
The substances formed as a result of a chemical reaction.
Combination Reaction
A reaction in which two or more reactants combine to form a single product.
Decomposition Reaction
A reaction in which a single compound breaks down into two or more products.
Single Replacement Reaction
A reaction in which one element replaces another element in a compound.
Double Replacement Reaction
A reaction where two compounds exchange ions or bonds to form different compounds.
Combustion Reaction
A reaction in which a carbon-containing compound reacts with oxygen to produce carbon dioxide and water, releasing energy.
Limiting Reactant
The reactant that is completely consumed in a chemical reaction, limiting the amount of product formed.
Theoretical Yield
The maximum amount of product that could be formed from given amounts of reactants.
Actual Yield
The amount of product that is actually produced in a chemical reaction.
Percent Yield
The ratio of the actual yield to the theoretical yield expressed as a percentage.
Molarity (M)
A measure of concentration representing the amount of solute (in moles) divided by the volume of solution (in liters).
Aqueous Solution
A solution in which water is the solvent.
Colligative Properties
Properties that depend on the number of solute particles in a solution, not their identity.
Net Ionic Equation
An equation that shows only the particles that participate in the reaction, excluding spectator ions.
Oxidation-Reduction (Redox) Reaction
A reaction involving the transfer of electrons between substances.
Oxidizing Agent
The substance that gains electrons in a redox reaction.
Reducing Agent
The substance that loses electrons in a redox reaction.
Dissociation
The process by which an ionic compound separates into its ions in solution.
Saturation
A solution that cannot dissolve any more solute at a given temperature.
Supersaturation
A solution that contains more solute than it can theoretically hold at a given temperature.
Stoichiometry
The study of the numerical relationships between the quantities of reactants and products in a chemical reaction.
Reactants
The starting substances in a chemical reaction that are transformed into products.
Products
The substances formed as a result of a chemical reaction.
Combination Reaction
A reaction in which two or more reactants combine to form a single product.
Decomposition Reaction
A reaction in which a single compound breaks down into two or more products.
Single Replacement Reaction
A reaction in which one element replaces another element in a compound.
Double Replacement Reaction
A reaction where two compounds exchange ions or bonds to form different compounds.
Combustion Reaction
A reaction in which a carbon-containing compound reacts with oxygen to produce carbon dioxide and water, releasing energy.
Limiting Reactant
The reactant that is completely consumed in a chemical reaction, limiting the amount of product formed.
Theoretical Yield
The maximum amount of product that could be formed from given amounts of reactants.
Actual Yield
The amount of product that is actually produced in a chemical reaction.
Percent Yield
The ratio of the actual yield to the theoretical yield expressed as a percentage.
Molarity (M)
A measure of concentration representing the amount of solute (in moles) divided by the volume of solution (in liters).
Aqueous Solution
A solution in which water is the solvent.
Colligative Properties
Properties that depend on the number of solute particles in a solution, not their identity.
Net Ionic Equation
An equation that shows only the particles that participate in the reaction, excluding spectator ions.
Oxidation-Reduction (Redox) Reaction
A reaction involving the transfer of electrons between substances.
Oxidizing Agent
The substance that gains electrons in a redox reaction.
Reducing Agent
The substance that loses electrons in a redox reaction.
Dissociation
The process by which an ionic compound separates into its ions in solution.
Saturation
A solution that cannot dissolve any more solute at a given temperature.
Supersaturation
A solution that contains more solute than it can theoretically hold at a given temperature.
Balancing Chemical Equation
The process of ensuring that the number of atoms of each element is the same on both the reactant and product sides of a chemical equation.
Molar Mass
The mass (in grams) of one mole of a substance.
Avogadro's Number
The number of constituent particles (typically atoms or molecules) per mole, equal to 6.022 \times 10^{23} \text{ particles/mol}.
Mole (mol)
The SI unit for amount of substance, defined as the amount of substance that contains 6.022 \times 10^{23} elementary entities (Avogadro's number).
Note 
Flashcards (100)