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Chapter 4 Stoichiometry of Chemical Reactions 195 Step 5. Balance charge by adding electrons. The iron half-reaction shows a total charge of 2+ on the left side (1 Fe2+ ion) and 3+ on the right side (1 Fe3+ ion). Adding one electron to the right side bring that side’s total charge to (3+) + (1−) = 2+, and charge balance is achieved. The chromium half-reaction shows a total charge of (1 × 2−) + (14 × 1+) = 12+ on the left side (1 Cr2 O7 2− ion and 14 H+ ions). The total charge on the right side is (2 × 3+) = 6 + (2 Cr3+ ions). Adding six electrons to the left side will bring that side’s total charge to (12+ + 6−) = 6+, and charge balance is achieved. Fe2+ ⟶Fe3++e− Cr2O72−+14H+ +6e− ⟶2Cr3++7H2O Step 6. Multiply the two half-reactions so the number of electrons in one reaction equals the number of electrons in the other reaction. To be consistent with mass conservation, and the idea that redox reactions involve the transfer (not creation or destruction) of electrons, the iron half-reaction’s coefficient must be multiplied by 6. 6Fe2+ ⟶ 6Fe3+ + 6e− Cr2O72−+6e− +14H+ ⟶2Cr3++7H2O Step 7. Add the balanced half-reactions and cancel species that appear on both sides of the equation. 6Fe2++Cr2O72−+6e− +14H+ ⟶6Fe3++6e− +2Cr3++7H2O Only the six electrons are redundant species. Removing them from each side of the equation yields the simplified, balanced equation here: 6Fe2++Cr2O72−+14H+ ⟶6Fe3++2Cr3++7H2O A final check of atom and charge balance confirms the equation is balanced. Reactants Products Fe 6 6 Cr 2 2 O77 H 14 14 charge 24+ 24+ Check Your Learning In acidic solution, hydrogen peroxide reacts with Fe2+ to produce Fe3+ and H2O. Write a balanced equation for this reaction. Answer: H2 O2(aq) + 2H+(aq) + 2Fe2+ ⟶ 2H2 O(l) + 2Fe3+PDF Image | Stoichiometry of Chemical Reactions
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