CHEM 102 Lab 11 PostLab Redox Reactions (Answered)

Consider your experimental results from part A of this lab. Suppose your strongest reducing agent were added to your strongest oxidizing agent. (Use the lowest possible coefficients. Omit states-of-matter from your answers.) (a) Write the half-reaction for your strongest reducing agent. Mg → Mg2+ + 2e- Mg → Mg2+ + 2 e- Mg --> Mg^2+ + 2e^- (b) Write the half-reaction for your strongest oxidizing agent. MnO4- + 8H+ + 5e- → Mn2+ + 4H2O MnO - 4 + 8 H+ + 5 e- → Mn2+ + 4 H2O MnO_4^- + 8H^+ + 5e^- --> Mn^2+ + 4H_2O (c) Note the number of electrons in each half reaction. In order to balance the number of electrons lost and gained, the oxidation half-reaction must be multiplied by five, five, and the reduction half-reaction must be multiplied by two. two. (d) Write the net redox reaction. 5Mg + 2MnO4 - + 16H+ → 5Mg2+ + 2Mn2+ + 8H2O 2 MnO - 4 + 5 Mg + 16 H+ → 2 Mn2+ + 8 H2O + 5 Mg2+ 5Mg + 2MnO_4^- + 16H^+ --> 5Mg^2+ + 2Mn^2+ + 8H_2O