The combustion of methane: CH₄ + 2O₂ → CO₂ + 2H₂O.

The decomposition of water: 2H₂O → 2H₂ + O₂.

The displacement of zinc by copper: Zn + CuSO₄ → ZnSO₄ + Cu.

An example of a synthesis reaction is the formation of water: 2H₂ + O₂ → 2H₂O.

The digestion of food in the stomach is a decomposition reaction.

The rusting of iron is an example of a decomposition reaction.

The combination of hydrogen and oxygen to form water is a decomposition reaction.

An example of a decomposition reaction is the breakdown of water (H2O) into hydrogen (H2) and oxygen (O2) gas when electricity is passed through it.

A single replacement reaction is a chemical reaction where one element replaces another in a compound.

A single replacement reaction is when elements are created from nothing in a chemical process.

A single replacement reaction involves two compounds exchanging elements.

A single replacement reaction is a process where two elements combine to form a compound.

The exchange of ions between two compounds resulting in new compounds.

The combination of two elements to form a compound.

The breakdown of a compound into its elements.

The formation of a gas from a single compound.

2 H2 + O2 -> 2 H2O

CH4 + 2 O2 -> CO2 + 2 H2O

2 CH4 + 3 O2 -> 2 CO + 4 H2O

C3H8 + 5 O2 -> 3 CO2 + 4 H2O

Change in state of matter

Increase in mass

Absence of odor

Signs of a chemical reaction include color change, temperature change, gas production, and formation of a precipitate.

Reactants are the final products of a chemical reaction.

Reactants are substances that do not change during a reaction.

Reactants are the starting materials that undergo change in a chemical reaction.

Reactants are the energy sources required for a reaction to occur.

Exothermic reactions are faster than endothermic reactions; endothermic reactions are slower.

Exothermic reactions occur only in gases; endothermic reactions occur only in liquids.

Exothermic reactions absorb energy; endothermic reactions release energy.

Exothermic reactions release energy; endothermic reactions absorb energy.

A redox reaction is a type of reaction that does not involve electron transfer.

A redox reaction is a process that only involves the formation of new compounds.

A redox reaction is a reaction where two substances are combined without any change in their oxidation states.

A redox reaction is a chemical reaction involving the transfer of electrons, where one substance is oxidized and another is reduced.

Catalysts change the products of a chemical reaction.

Catalysts slow down chemical reactions by increasing activation energy.

Catalysts speed up chemical reactions by lowering activation energy.

Catalysts are consumed in the reaction and do not affect the overall energy change.

Mass is created during chemical reactions.

The total mass increases in chemical reactions.

The total mass remains constant in chemical reactions.

Mass can be lost in chemical reactions.

Balancing chemical equations is only important for organic reactions.

Balancing chemical equations is significant because it reflects the conservation of mass and provides accurate stoichiometric relationships.

It is a method to increase the temperature of a reaction.

Balancing equations is irrelevant to real-world applications.

A combustion reaction involving an acid and a base.

An example of an acid-base reaction is the neutralization of hydrochloric acid (HCl) with sodium hydroxide (NaOH), which produces water (H2O) and sodium chloride (NaCl).

The reaction of water with carbon dioxide to form glucose.

A reaction between two metals producing a gas.

Increasing temperature reduces collision frequency between reactants.

Concentration has no effect on reaction rates whatsoever.

Higher temperature decreases reaction rates by slowing down molecules.

Temperature increases reaction rates by providing energy; higher concentration increases rates by increasing collision frequency.