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Chapter 4 Stoichiometry of Chemical Reactions 179 Write a balanced equation for the reaction of molecular nitrogen (N2) and oxygen (O2) to form dinitrogen pentoxide. Solution First, write the unbalanced equation. N2 + O2 ⟶ N2 O5 (unbalanced) Next, count the number of each type of atom present in the unbalanced equation. N 1 × 2 = 2 1 × 2 = 2 2 = 2, yes O 1 × 2 = 2 1 × 5 = 5 2 ≠ 5, no Though nitrogen is balanced, changes in coefficients are needed to balance the number of oxygen atoms. To balance the number of oxygen atoms, a reasonable first attempt would be to change the coefficients for the O2 and N2O5 to integers that will yield 10 O atoms (the least common multiple for the O atom subscripts in these two formulas). N2+5O2 ⟶2N2O5 (unbalanced) Element Reactants Products Balanced? Element N O Element N O Reactants 1 × 2 = 2 Products 2 × 2 = 4 Balanced? 2 ≠ 4, no 5 × 2 = 10 The N atom balance has been upset by this change; it is restored by changing the coefficient for the reactant N2 to 2. 2N2+5O2 ⟶2N2O5 2 × 5 = 10 10 = 10, yes Balanced? 4 = 4, yes 10 = 10, yes Reactants 2 × 2 = 4 5 × 2 = 10 Products 2 × 2 = 4 2 × 5 = 10 The numbers of N and O atoms on either side of the equation are now equal, and so the equation is balanced. Check Your Learning Write a balanced equation for the decomposition of ammonium nitrate to form molecular nitrogen, molecular oxygen, and water. (Hint: Balance oxygen last, since it is present in more than one molecule on the right side of the equation.) Answer: 2NH4NO3 ⟶ 2N2 +O2 +4H2OPDF Image | Stoichiometry of Chemical Reactions
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