Acetylene 1C2H22 and nitrogen 1N22 both contain a triple bond, but they differ greatly in their chemical properties. (c) Write balanced chemical equations for the complete oxidation of N2 to form N2O51g2 and of acetylene to form CO21g2 and H2O1g2. Write a balanced chemical equation for the complete oxidation of acetylene to form CO2( g) and H2O(g).

Key Concepts

Balancing Chemical Equations

Balancing chemical equations is essential in chemistry to ensure that the law of conservation of mass is upheld. This means that the number of atoms of each element must be the same on both sides of the equation. To balance an equation, coefficients are adjusted in front of the chemical formulas, allowing for the correct stoichiometric relationships between reactants and products.

Combustion Reactions

Combustion reactions involve the reaction of a substance with oxygen to produce energy, typically in the form of heat and light. For hydrocarbons like acetylene, complete combustion results in carbon dioxide (CO2) and water (H2O) as products. Understanding the stoichiometry of these reactions is crucial for writing balanced equations and predicting the amounts of reactants and products involved.

Oxidation States

Oxidation states (or oxidation numbers) are used to keep track of electron transfer in chemical reactions, particularly in redox reactions. In the context of the question, nitrogen in N2 has an oxidation state of 0, while in N2O5, it has a +5 oxidation state. Recognizing changes in oxidation states helps in understanding the nature of the reaction and the products formed during oxidation.