21 On your standard reduction potential table highlight top ten reducing agents

21 on your standard reduction potential table

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21. On your standard reduction potential table, highlight top ten reducing agents (not the whole equation). Model 2: Redox reactions (from the SR as Redox and Relative Reactivities of Metals labs) Net Ionic Reaction Half Reactions Did this reaction occur? Mg + Ag + Ag + Mg 2+ Oxidation: E o ox : Reduction: E o red : Ag + Zn 2+ Zn + Ag + Oxidation: E o ox : Reduction: E o red : Cu + Ag + → Ag + Cu 2+ Oxidation: E o ox : Reduction: E o red : Zn + Mg 2+ → Mg + Zn 2+ Oxidation: E o ox : Reduction: E o red :
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Chemistry POGIL – Standard Reduction Potentials Ms. Park 22. Complete the table above by writing the oxidation/reduction half-reactions for each , as well as the E o values . Refer back to your single replacement lab to determine whether the reaction occurred or not . 23. What do you observe about the reactions that occur? 24. What do you observe about the reactions that do not occur? 25. Spontaneous reactions are ones that occur on their own . Propose a method to determine if a redox reaction will be spontaneous or not. Exercises: Predict whether these reactions are spontaneous or nonspontaneous. Then balance the equations using the half-reaction method. 1. MnO 4 + H 2 C 2 O 4 Mn 2+ + CO 2 2. Cl + Br 2 → Cl 2 + Br
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