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178 Chapter 4 Stoichiometry of Chemical Reactions A balanced chemical equation often may be derived from a qualitative description of some chemical reaction by a fairly simple approach known as balancing by inspection. Consider as an example the decomposition of water to yield molecular hydrogen and oxygen. This process is represented qualitatively by an unbalanced chemical equation: H2 O ⟶ H2 + O2 (unbalanced) Comparing the number of H and O atoms on either side of this equation confirms its imbalance: H 1 × 2 = 2 1 × 2 = 2 2 = 2, yes O 1 × 1 = 1 1 × 2 = 2 1 ≠ 2, no The numbers of H atoms on the reactant and product sides of the equation are equal, but the numbers of O atoms are not. To achieve balance, the coefficients of the equation may be changed as needed. Keep in mind, of course, that the formula subscripts define, in part, the identity of the substance, and so these cannot be changed without altering the qualitative meaning of the equation. For example, changing the reactant formula from H2O to H2O2 would yield balance in the number of atoms, but doing so also changes the reactant’s identity (it’s now hydrogen peroxide and not water). The O atom balance may be achieved by changing the coefficient for H2O to 2. Element Reactants Products Balanced? 2H2 O ⟶ H2 + O2 (unbalanced) 1 × 2 = 2 4 ≠ 2, no 1 × 2 = 2 2 = 2, yes The H atom balance was upset by this change, but it is easily reestablished by changing the coefficient for the H2 Element Reactants Products Balanced? H 2 × 2 = 4 O 2 × 1 = 2 product to 2. 2H2O⟶2H2+O2 (balanced) Element Reactants Products Balanced? H 2 × 2 = 4 2 × 2 = 2 4 = 4, yes O 2 × 1 = 2 1 × 2 = 2 2 = 2, yes These coefficients yield equal numbers of both H and O atoms on the reactant and product sides, and the balanced equation is, therefore: 2H2 O ⟶ 2H2 + O2 Example 4.1 Balancing Chemical Equations This content is available for free at http://cnx.org/content/col11760/1.9PDF Image | Stoichiometry of Chemical Reactions
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