Question

Balance the chemical equation: \(\text{Fe} + \text{H}_2\text{O} \rightarrow \text{Fe}_3\text{O}_4 + \text{H}_2\)

Hint:

Start balancing with the most complex molecule or the atom that appears in the fewest number of compounds.

Answer 1

Step 1: Understanding the Concept:
Balancing an equation ensures the Law of Conservation of Mass is satisfied, meaning the number of atoms of each element is equal on both the reactant and product sides.

Step 2: Key Formula or Approach:
Count atoms on both sides and use coefficients to balance them step-by-step.

Step 2: Detailed Explanation:
Unbalanced equation: \(\text{Fe} + \text{H}_2\text{O} \rightarrow \text{Fe}_3\text{O}_4 + \text{H}_2\)
Reactant side: \(1\text{ Fe}\), \(2\text{ H}\), \(1\text{ O}\)
Product side: \(3\text{ Fe}\), \(2\text{ H}\), \(4\text{ O}\)
1. Balance Fe atoms: Multiply Fe on the reactant side by 3.
\(3\text{Fe} + \text{H}_2\text{O} \rightarrow \text{Fe}_3\text{O}_4 + \text{H}_2\)
2. Balance O atoms: Multiply \(\text{H}_2\text{O}\) on the reactant side by 4.
\(3\text{Fe} + 4\text{H}_2\text{O} \rightarrow \text{Fe}_3\text{O}_4 + \text{H}_2\)
3. Balance H atoms: Now there are \(8\text{ H}\) atoms on the reactant side. Multiply \(\text{H}_2\) on the product side by 4.
\(3\text{Fe} + 4\text{H}_2\text{O} \rightarrow \text{Fe}_3\text{O}_4 + 4\text{H}_2\)
Check: \(3\text{Fe}, 8\text{H}, 4\text{O}\) on both sides. The equation is balanced.

Step 3: Final Answer:
The balanced equation is \(3\text{Fe} + 4\text{H}_2\text{O} \rightarrow \text{Fe}_3\text{O}_4 + 4\text{H}_2\).