Write balanced equations for the formation of the following compounds from their elements. (a) Iron(III) oxide

Verified step by step guidance

1. Identify the elements involved in forming Iron(III) oxide. Iron(III) oxide is composed of iron (Fe) and oxygen (O).
2. Determine the oxidation states of the elements in the compound. In Iron(III) oxide, iron has an oxidation state of +3, and oxygen has an oxidation state of -2.
3. Write the unbalanced chemical equation using the symbols of the elements and the compound. The unbalanced equation is: \(Fe + O_2 \rightarrow Fe_2O_3\).
4. Balance the chemical equation. Start by balancing the atoms that appear in the least amount of substances in the equation. In this case, balance the iron (Fe) atoms first, followed by the oxygen (O) atoms.
5. Check the balanced equation to ensure that the number of atoms for each element is the same on both sides of the equation. The balanced chemical equation should be: \(4Fe + 3O_2 \rightarrow 2Fe_2O_3\).

Key Concepts

Chemical Equations

Chemical equations represent the reactants and products in a chemical reaction. They must be balanced to obey the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. Each element's number of atoms must be the same on both sides of the equation.

Formation Reactions

A formation reaction is a specific type of chemical reaction where elements combine to form a compound. In these reactions, the elements are in their standard states, and the product is typically a single compound. For example, the formation of iron(III) oxide involves the reaction of iron and oxygen.

Oxidation States

Oxidation states (or oxidation numbers) indicate the degree of oxidation of an atom in a compound. They help in determining how electrons are transferred during reactions. In iron(III) oxide, iron has an oxidation state of +3, which is crucial for balancing the equation and understanding the compound's formation.