QuestionJune 10, 2025

56. 2MnO_(4)^-(aq)+10Br^-(aq)+16H^+(aq)arrow 2Mn^2+(aq)+5Br_(2)(aq)+8H_(2)O(l) How many electrons are transferred in the reaction represented by the balanced equation above? (A) 8 (B) 5 I (C) 10 (D) 6 (E) 12

56. 2MnO_(4)^-(aq)+10Br^-(aq)+16H^+(aq)arrow 2Mn^2+(aq)+5Br_(2)(aq)+8H_(2)O(l) How many electrons are transferred in the reaction represented by the balanced equation above? (A) 8 (B) 5 I (C) 10 (D) 6 (E) 12
56.
2MnO_(4)^-(aq)+10Br^-(aq)+16H^+(aq)arrow 2Mn^2+(aq)+5Br_(2)(aq)+8H_(2)O(l)
How many electrons are transferred in the reaction represented by the balanced equation above?
(A) 8
(B) 5 I
(C) 10
(D) 6
(E) 12

Solution
4.7(195 votes)

Answer

20 Explanation 1. Identify Oxidation States Mn changes from +7 in MnO_4^- to +2 in Mn^{2+}, and Br changes from -1 in Br^- to 0 in Br_2. 2. Calculate Electron Transfer for Mn Each Mn gains 5 electrons: 2 \times 5 = 10 electrons total for Mn. 3. Calculate Electron Transfer for Br Each Br loses 1 electron: 10 \times 1 = 10 electrons total for Br. 4. Total Electron Transfer Total electrons transferred = 10 (Mn) + 10 (Br) = 20 electrons.

Explanation

1. Identify Oxidation States<br /> Mn changes from +7 in $MnO_4^-$ to +2 in $Mn^{2+}$, and Br changes from -1 in $Br^-$ to 0 in $Br_2$.<br /><br />2. Calculate Electron Transfer for Mn<br /> Each Mn gains 5 electrons: $2 \times 5 = 10$ electrons total for Mn.<br /><br />3. Calculate Electron Transfer for Br<br /> Each Br loses 1 electron: $10 \times 1 = 10$ electrons total for Br.<br /><br />4. Total Electron Transfer<br /> Total electrons transferred = 10 (Mn) + 10 (Br) = 20 electrons.
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