Draw a chemical equation to represent the redox reaction that occurs when methane (CH4) burns in the presence of oxygen (O2). Identify the reactant that is reduced and the reactant that is oxidized. Of the four molecules that should be in your equation, point out the one that has bonds with the highest potential energy.

Verified step by step guidance

1. Write the balanced chemical equation for the combustion of methane: CH_4 + 2O_2 \rightarrow CO_2 + 2H_2O.
2. Identify the oxidation states of carbon in CH_4 and CO_2. In CH_4, carbon is in the -4 oxidation state, and in CO_2, it is in the +4 oxidation state.
3. Identify the oxidation states of oxygen in O_2 and H_2O. In O_2, oxygen is in the 0 oxidation state, and in H_2O, it is in the -2 oxidation state.
4. Determine which reactant is oxidized and which is reduced. Methane (CH_4) is oxidized as carbon's oxidation state increases, and oxygen (O_2) is reduced as its oxidation state decreases.
5. Identify the molecule with the highest potential energy bonds. Methane (CH_4) has C-H bonds, which are high in potential energy compared to the bonds in CO_2 and H_2O.

Key Concepts

Redox Reactions

Redox reactions, or reduction-oxidation reactions, involve the transfer of electrons between two substances. In these reactions, one reactant undergoes oxidation (loses electrons) while another undergoes reduction (gains electrons). Understanding these processes is crucial for identifying which substances are oxidized and reduced in a chemical equation.

Combustion of Methane

The combustion of methane (CH4) is a specific type of redox reaction where methane reacts with oxygen (O2) to produce carbon dioxide (CO2) and water (H2O). This reaction releases energy in the form of heat and light, making it an exothermic process. Recognizing the products formed helps in determining the changes in oxidation states of the reactants.

Potential Energy of Bonds

The potential energy of chemical bonds refers to the energy stored in the bonds between atoms. In the context of the combustion of methane, the bonds in methane (CH4) have higher potential energy compared to the bonds in the products (CO2 and H2O). This difference in energy is what drives the reaction, as breaking high-energy bonds releases energy when forming lower-energy products.