**Question:**What half reaction occurs at the anode during the electrolysis of molten potassium bromide:- ○ K ----> K⁺ + e⁻- ○ K + e⁻ ----> K⁻- ○ Br₂ + 2 e⁻ ----> 2Br⁻- ○ 2Br⁻ ----> Br₂ + 2 e⁻- ○ 2H₂O + 2e⁻ ----> H₂ + 2OH⁻**Explanation:**During the electrolysis of molten potassium bromide (KBr), the anode is the site of oxidation. Bromide ions (Br⁻) lose electrons to form bromine gas (Br₂). Thus, the correct half-reaction that occurs at the anode is:- ○ 2Br⁻ ----> Br₂ + 2 e⁻This reaction involves the oxidation of bromide ions to molecular bromine.

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What half reaction occurs at the anode during the electrolysis of molten potassium bromide: OK----> K+ē OK+ē----> K Br₂ + 2 ē> 2Br¯ 2Br ----> > Br₂ + 2 ē 2H₂O + 2ē ---> H₂ + 2OH¯

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

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