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9. I2 + Cl03 IO3 + Cl" (acidic) 10. MnO4 + NH3 → MnO2 (s) + NO; (basic) 11. Mg (s) + ReO4 Mg* + Re (acidic) 12 NO (ooidie)

9. I2 + Cl03 IO3 + Cl" (acidic) 10. MnO4 + NH3 → MnO2 (s) + NO; (basic) 11. Mg (s) + ReO4 Mg* + Re (acidic) 12 NO (ooidie)

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.61QP: Order the following oxidizing agents by increasing strength under standard-state conditions: O2(g);...
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Balance the following redox reactions given the pH of the solution stated. 

9. I2 + ClO3 → IO3 + Cl° (acidic) 10. MnO4 + NH3 → MnO2 (s) + NO; (basic) 2+ 11. Mg (s) + ReO4 –→ Mg* + Re (acidic) 12. Ag (s) + NO3 → Ag" + NO (acidic) 13. Fe(CN),* + Cr2O; → Fe(CN), + CrO4² (basic) 2+ 14. MnO4 + C¿0,²- → CO, + Mn² (acidic)
Transcribed Image Text:9. I2 + ClO3 → IO3 + Cl° (acidic) 10. MnO4 + NH3 → MnO2 (s) + NO; (basic) 2+ 11. Mg (s) + ReO4 –→ Mg* + Re (acidic) 12. Ag (s) + NO3 → Ag" + NO (acidic) 13. Fe(CN),* + Cr2O; → Fe(CN), + CrO4² (basic) 2+ 14. MnO4 + C¿0,²- → CO, + Mn² (acidic)
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