22.3. Balancing Redox Equations http://www.ck12.org
Lesson Review Questions
- Write half-reactions for the following redox processes:
a. Fe + V 2 O 3 →Fe 2 O 3 + VO
b. K 2 Cr 2 O 7 + SnCl 2 + HCl→CrCl 3 + SnCl 4 + KCl + H 2 O
c. K 2 Cr 2 O 7 + H 2 O + S→SO 2 + KOH + Cr 2 O 3 - Write the balanced chemical equations for the following reactions:
a. Magnesium carbonate is heated strongly to produce magnesium oxide and carbon dioxide gas.
b. Hydrogen peroxide decomposes to produce water and oxygen gas.
c. Solid potassium chlorate is heated in the presence of manganese dioxide as a catalyst to produce potas-
sium chloride and oxygen gas.
d. Lead sulfide reacts with molecular oxygen to form sulfur dioxide and lead(II) oxide. - Write oxidation and reduction half-reactions for the following single-replacement reaction: Fe(s) + CuSO 4 (aq)
→FeSO 4 (aq) + Cu(s). - Use the half-reaction method to balance the following redox equation: As 4 + NaOCl + H 2 O→NaCl +
H 3 AsO 4.
Further Reading / Supplemental Links
Explanation and practice for balancing redox equations: http://www.mpcfaculty.net/mark_bishop/redoxbalance
oxidation.htm
Points to Consider
- Although oxidation and reduction processes must occur simultaneously, they do not necessarily have to occur
in the same space. How can this be used to generate electricity, which is essentially the flow of electrons
through a wire?