Write the balanced chemical equation for each reaction. b. Solid iron(III) oxide reacts with hydrogen gas to form solid iron and liquid water.

Verified step by step guidance

1. Step 1: Write down the unbalanced chemical equation. In this case, the reactants are solid iron(III) oxide (Fe2O3) and hydrogen gas (H2), and the products are solid iron (Fe) and liquid water (H2O). So, the unbalanced equation is: Fe2O3(s) + H2(g) → Fe(s) + H2O(l)
2. Step 2: Balance the equation by adjusting the coefficients in front of the chemical formulas. Start by balancing the elements that appear in only one compound on each side. In this case, start with iron (Fe). There are 2 Fe atoms in Fe2O3 on the left side, so put a coefficient of 2 in front of Fe on the right side: Fe2O3(s) + H2(g) → 2Fe(s) + H2O(l)
3. Step 3: Next, balance the hydrogen atoms. There are 2 H atoms in H2 on the left side and 2 H atoms in H2O on the right side, so the hydrogen atoms are already balanced.
4. Step 4: Finally, balance the oxygen atoms. There are 3 O atoms in Fe2O3 on the left side and 1 O atom in H2O on the right side. To balance the oxygen atoms, put a coefficient of 3 in front of H2O on the right side: Fe2O3(s) + H2(g) → 2Fe(s) + 3H2O(l)
5. Step 5: Now, recheck the hydrogen atoms since we have changed the number of H2O molecules. There are 2 H atoms in H2 on the left side and 6 H atoms in 3H2O on the right side. To balance the hydrogen atoms, put a coefficient of 3 in front of H2 on the left side: Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l). Now, the equation is balanced.

Key Concepts

Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms of each element is the same on both sides of the equation. This is based on the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. To balance an equation, coefficients are adjusted in front of the chemical formulas to achieve equal atom counts.

Types of Chemical Reactions

The reaction described is a redox reaction, where oxidation and reduction occur simultaneously. In this case, iron(III) oxide (Fe2O3) is reduced to iron (Fe), while hydrogen gas (H2) is oxidized to water (H2O). Understanding the roles of oxidizing and reducing agents is crucial for identifying the changes in oxidation states during the reaction.

States of Matter in Chemical Reactions

In chemical equations, the physical states of the reactants and products are indicated using symbols: (s) for solid, (l) for liquid, and (g) for gas. This information is important for understanding the conditions under which the reaction occurs and can affect the reaction's feasibility and rate. In the given reaction, solid iron(III) oxide and hydrogen gas react to produce solid iron and liquid water.