Given the balanced redox reaction: 6 I− + 2 MnO4− + 4 H2O(l) 3 I2(s) + 2 MnO2(s) + OH−

Given the balanced redox reaction: 6 I− + 2 MnO4− + 4 H2O(l) 3 I2(s) + 2 MnO2(s) + OH− Which of the following statements regarding the reaction represented by the equation above is correct? (A) Iodide ion is oxidized by hydroxide ion. (D) The oxidation number of Mn remains the same. (B) MnO4− is oxidized by iodide ion. (E) The oxidation number of Iodine changes from −1 to 0. (C) The oxidation number of Mn changes from +7 to +2.

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