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A collection of flashcards summarizing key vocabulary and concepts from a chemistry lecture focusing on stoichiometry, empirical formulas, balancing equations, and limiting reactants.
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Empirical Formula
A chemical formula that shows the simplest ratio of elements in a compound.
Molecular Formula
The formula that shows the actual number of atoms of each element in a molecule.
Balancing Chemical Equations
The process of making sure that the number of atoms of each element is the same on both the reactant and product sides.
Stoichiometry
The calculation of reactants and products in chemical reactions.
Stoichiometric Ratio
The ratio of moles of reactants and products obtained from a balanced chemical equation.
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 can be produced from a given quantity of reactants.
Percent Yield
The ratio of the actual yield to the theoretical yield, expressed as a percentage.
Combustion Reaction
A chemical reaction that involves the rapid combination of a substance with oxygen, producing heat and light.
Molar Mass
The mass of one mole of a substance, typically measured in grams per mole.
Complete Combustion
A reaction where a hydrocarbon reacts with oxygen to produce carbon dioxide and water.
Dimensional Analysis
A mathematical technique used to convert units and solve problems involving measurements.
Excess Reactant
The reactant that remains after a chemical reaction has completed.
Hydrocarbon
An organic compound consisting solely of hydrogen and carbon, typically used as fuels.
Mole
A unit used in chemistry to measure the amount of substance, equivalent to approximately 6.022 x 10²³ particles.
Diatomic Oxygen
Molecular oxygen that consists of two oxygen atoms, which is necessary for combustion.
Chemical Equation
A symbolic representation of a chemical reaction, showing the reactants and products.