A unit used to measure the amount of a substance

A measure of the mass of a substance

A way to calculate the volume of a substance

A method for determining the density of a substance

CH₄ + 2O₂ → CO₂ + 2H₂O

CH₄ + O₂ → CO + 2H₂

CH₄ + 2O₂ → CO₂ + H₂O

CH₄ + O₂ → C + 2H₂O

58.44 g/mol

35.45 g/mol

22.99 g/mol

44.01 g/mol

The reactant that is completely consumed in the reaction

The reactant that is present in excess

The reactant that is present in the smallest amount

The reactant that is present in the largest amount

The ratio of the actual yield to the theoretical yield

The ratio of the theoretical yield to the actual yield

The difference between the actual yield and the theoretical yield

The sum of the actual yield and the theoretical yield

A formula that shows the simplest whole-number ratio of atoms in a compound

A formula that shows the exact number of atoms in a compound

A formula that shows the molecular weight of a compound

A formula that shows the structural arrangement of atoms in a compound

A formula that shows the exact number of atoms in a molecule of a compound

A formula that shows the simplest whole-number ratio of atoms in a compound

A formula that shows the molecular weight of a compound

A formula that shows the structural arrangement of atoms in a compound

An atom is the smallest unit of an element that retains all of its chemical properties, while a molecule is a group of atoms that are held together by chemical bonds.

An atom is the smallest unit of an element that can exist independently, while a molecule is a group of atoms that are held together by physical bonds.

An atom is the smallest unit of an element that can participate in a chemical reaction, while a molecule is a group of atoms that are held together by covalent bonds.

An atom is the smallest unit of an element that can be seen with a microscope, while a molecule is a group of atoms that are held together by ionic bonds.

Mass cannot be created or destroyed in a chemical reaction.

Mass can be created or destroyed in a chemical reaction.

Mass can be created but not destroyed in a chemical reaction.

Mass can be destroyed but not created in a chemical reaction.

PV = nRT

PV = nRT/V

PV = RT/n

PV = n/RT

Molar mass is directly proportional to density.

Molar mass is inversely proportional to density.

Molar mass is independent of density.

Molar mass is equal to density.

A chemical equation shows the reactants and products of a reaction, while a balanced chemical equation shows the reactants and products in stoichiometric proportions.

A chemical equation shows the reactants and products of a reaction, while a balanced chemical equation shows the reactants and products in mole ratios.

A chemical equation shows the reactants and products of a reaction, while a balanced chemical equation shows the reactants and products in mass ratios.

A chemical equation shows the reactants and products of a reaction, while a balanced chemical equation shows the reactants and products in volume ratios.

A homogeneous mixture is a mixture in which the components are evenly distributed throughout the mixture, while a heterogeneous mixture is a mixture in which the components are not evenly distributed throughout the mixture.

A homogeneous mixture is a mixture in which the components are in the same phase, while a heterogeneous mixture is a mixture in which the components are in different phases.

A homogeneous mixture is a mixture in which the components have the same chemical composition, while a heterogeneous mixture is a mixture in which the components have different chemical compositions.

A homogeneous mixture is a mixture in which the components have the same physical properties, while a heterogeneous mixture is a mixture in which the components have different physical properties.

A solution is a homogeneous mixture, while a suspension is a heterogeneous mixture.

A solution is a mixture in which the solute is dissolved in the solvent, while a suspension is a mixture in which the solute is suspended in the solvent.

A solution is a mixture in which the solute is in the same phase as the solvent, while a suspension is a mixture in which the solute is in a different phase than the solvent.

A solution is a mixture in which the solute has a smaller particle size than the solvent, while a suspension is a mixture in which the solute has a larger particle size than the solvent.