G. C. 1-4 Understanding Oxidizing Strengths in Redox Reactions 31 SYSTEM 3: 0cr
ID: 1086200 • Letter: G
Question
G. C. 1-4 Understanding Oxidizing Strengths in Redox Reactions 31 SYSTEM 3: 0cr (aq) + 2Br"(aq) + 11,0 d,t, 17. Record your observations below cr (aq) + B(aq) + 2011. (aq) 18. Based on your observations, did a redox reaction occur? Explain how you determined this. If a reaction occurred, complete questions 19-25. 19. Which atom is oxidized, and what are its initial and final oxidation numbers? 20. Which atom is reduced, and what are its initial and final oxidation numbers? 21. Which substance (not atom) is being oxidized? 22. Which substance (not atom) is being reduced? 23. Write the half-equation for the oxidation reaction. 24. Write the half-equation for the reduction reaction. 25. What other ions are in solution and what are their roles?Explanation / Answer
For the given reaction,
OCl- (aq) + 2Br- (aq) + H2O (l) <==> Cl- (aq) + Br2 (aq) + 2OH- (aq)
17. The color changes from colorless to yellow.
18. The appearence of yellow color due to formation of Br2 shows the reaction has occured. This is a redox reaction. Br- from -1 oxidation state goes to 0 oxidation state in Br2 (oxidized). Cl goes from +1 to -1 oxidation state (reduced).
19. Br is oxidized from -1 to 0 oxidation state.
20. Cl from +1 goes to -1 oxidation state, so it is reduced.
21. Br- is being oxidized.
22. OCl- is being oxidized.
23. half-equation for oxidation,
2Br- (aq) ---> Br2 (aq) + 2e-
24. half-equation for reduction,
OCl- (aq) + H2O (l) + 2e- --> Cl- (aq) + 2OH- (aq)
25. Other ions in solution, OH-, which is to balance the H and O in equation.
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