Questions: Balance the chemical equation below using the smallest possible whole number stoichiometric coefficients. CH₃CH₂CH₃(g) + O₂(g) → CO₂(g) + H₂O(g)

Solution Steps

First, identify the number of each type of atom in the reactants and products. The unbalanced equation is:

\[ \text{CH}_3\text{CH}_2\text{CH}_3(g) + \text{O}_2(g) \rightarrow \text{CO}_2(g) + \text{H}_2\text{O}(g) \]

• Reactants:

  • Carbon (C): 3 (from \(\text{CH}_3\text{CH}_2\text{CH}_3\))
  • Hydrogen (H): 8 (from \(\text{CH}_3\text{CH}_2\text{CH}_3\))
  • Oxygen (O): 2 (from \(\text{O}_2\))

• Products:

  • Carbon (C): 1 (from \(\text{CO}_2\))
  • Hydrogen (H): 2 (from \(\text{H}_2\text{O}\))
  • Oxygen (O): 3 (1 from \(\text{CO}_2\) and 2 from \(\text{H}_2\text{O}\))

Balance the carbon atoms by ensuring the number of carbon atoms in the reactants equals the number in the products. Since there are 3 carbon atoms in the reactant \(\text{CH}_3\text{CH}_2\text{CH}_3\), place a coefficient of 3 in front of \(\text{CO}_2\):

\[ \text{CH}_3\text{CH}_2\text{CH}_3(g) + \text{O}_2(g) \rightarrow 3\text{CO}_2(g) + \text{H}_2\text{O}(g) \]

Balance the hydrogen atoms by ensuring the number of hydrogen atoms in the reactants equals the number in the products. Since there are 8 hydrogen atoms in the reactant \(\text{CH}_3\text{CH}_2\text{CH}_3\), place a coefficient of 4 in front of \(\text{H}_2\text{O}\):

\[ \text{CH}_3\text{CH}_2\text{CH}_3(g) + \text{O}_2(g) \rightarrow 3\text{CO}_2(g) + 4\text{H}_2\text{O}(g) \]

Balance the oxygen atoms by ensuring the number of oxygen atoms in the reactants equals the number in the products. The products now have \(3 \times 2 + 4 \times 1 = 10\) oxygen atoms. Therefore, place a coefficient of 5 in front of \(\text{O}_2\):

\[ \text{CH}_3\text{CH}_2\text{CH}_3(g) + 5\text{O}_2(g) \rightarrow 3\text{CO}_2(g) + 4\text{H}_2\text{O}(g) \]

Final Answer