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The formula that shows the actual number of atoms of each element in a molecule of a compound.

A laboratory method used to determine the elemental composition of a compound by burning it and measuring the masses of the combustion products.

The percentage of the theoretical yield that was actually attained in a chemical reaction.

The percent by mass of each element in a compound.

An equation that has the same number of atoms of each element on both sides of the reaction.

The quantitative relationship between reactants and products in a balanced chemical reaction.

The amount of substance that contains as many entities as there are atoms in 12 g of carbon-12.

The mass of one mole of a substance, typically measured in grams per mole (g/mol).

The substance that is totally consumed when the chemical reaction is complete.

The maximum amount of product that can be produced from a given amount of reactant, according to the balanced chemical equation.

The amount of product actually produced when the chemical reaction is carried out in an experiment.

The condition under which the volume of a gas is often measured; 0 degrees Celsius and 1 atmosphere of pressure.

The simplest whole number ratio of atoms of each element in a compound.

The volume occupied by one mole of a gas at a given temperature and pressure, often assumed to be 22.4 L at STP (Standard Temperature and Pressure).

The numbers used in a balanced chemical equation to show the proportion of reactants and products.

The calculation of reactants and products in chemical reactions in chemistry.

The substance that is not used up completely in a reaction.

The ratio of moles of one substance to the moles of another substance in a balanced chemical equation.

The number of atoms, ions, or molecules in one mole of a substance: $6.022 \times 10^{23}$ entities per mole.