MnO4^- (aq) + I2(s) ----------> Mn^2+(aq) + IO3^- (aq)
The oxidation number of Mn in MnO4^- is + 7
The oxidation number of I in IO3^- is + 5
The oxidation number of Mn is decreases from +7 to +2 . Mn is reduced .
The oxidation number of I is increases from 0 to +5 . I2 is oxidized.
I2 is oxidized
B. I2 >>>>answer
In the following reaction, is oxidized. MnO2 (aq) + 12 (5) Mn2+ (aq) + 105 (aq)...
plz hwlp me pass QUESTION 12 What element is oxidized in the following redox reaction? MnO2 (s) + H+ (aq) + HNO2(aq) → Mn2+ (aq) + NO3- (aq) + H20(1) O a. Mn Ob.o OCH Od.N
Balance the following basic Redox reaction: Cr3+ (aq) + MnO2 (s) ----------> Mn2+ (aq) + CrO4 2- (aq)
Complete and balance the following half-reaction in basic solution Mn2+(aq) → MnO2(s)
Balance the following redox reaction in acidic solution.... Mn2+(aq)+Zn2+(aq)=MnO2(s)+Zn(s)
Piece #1 (1/2 pt) Consider the following reaction (unbalanced): MnO2 (s) + H3AsO3(aq) -Mn²+ (aq) + H2AsO(aq) Split the reaction into two half-reactions. Oxidation half reaction: H:AsO3(aq) → H3 AsO, (aq) Reduction half reaction: MnO2 (s) Mn (aq) Piece #2 (1/2 pt) Consider the following half-reaction: MnOz(s) - Mn2+ (aq) Balance everything but oxygen and hydrogen atoms. MnO2 (s) + 2e Mn (aq) Piece W3 (1/2 pu) Take your answer to Piece #2 and balance the oxygen by adding a...
Puzzle #1 (1-1/2 pt) Balance the following reaction in acidic solution. MnO2 (s) + H3A5O3 (aq) --Mn+ (aq) + H3AsO4(aq) Puzzle #2 (3 pt) Balance the following reaction in basic solution Croa? (aq) + 12 (s) — Cr(OH); (s) + 103(aq)
5. Consider the following redox reaction at 25 °C: (10 points) MnO2 (s) → Mn? (aq) + MnOs (aq) (a) Balance the equation in acid (b) Calculate Eºcell (c) Calculate AGran (d) Calculate Hint!!! After balancing your half-reactions, determine which reaction is oxidation and which reaction is the reduction and use Eºcell = Ecath (red) -Eanode (ow)
An MnO2(s) /Mn2+(aq) electrode in which the pH is 10.27 is prepared.Find the [Mn2+] necessary to lower the potential of the half-cell to 0.00 V (at 25 ∘C).
Consider the following UNBALANCED reaction IN ACIDIC SOLUTION: Fe2+(aq) + MnO4-(aq) ⟶ Fe3+(aq) + Mn2+(aq) a. (5) Species that is oxidized (be specific – i.e. identify which atom and if there are multiple atoms with different charges, identify the correct one) b. (5) Species that is reduced (same instructions as above) c. (10) Full Balanced oxidation ½ reaction (‘full’ means with regard to mass (atoms) and charges.) d. (10) Full Balanced reduction ½ reaction e. (9) Complete Balanced Reaction Using...
Balance the following half-reaction occurring in basic solution MnO2(8) - Mn(OH)2(s) MnO2 (s) + H22(aq) + 2e - Mn(OH)2(s) MnO2(s) + 2H2O(l) + 26 - Mn(OH)2(s)+ 2OH(aq) MnO2(s) + 2H2O(l) - Mn(OH)2(3)+20H(aq) MnO2(s) + H2(g) - Mn(OH)2(s) + 2e- MnO2(s) + 2H2O(1) + 4e - Mn(OH)2(s)+ (OH)2 (aq)