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Piece #1 (1/2 pt) Consider the following reaction (unbalanced): MnO2 (s) + H3A50; (aq) →Mn?" (aq) + H3AsOa(aq) Spl...
Piece #1 (1/2 pt) Consider the following reaction (unbalanced): MnO2 (s) + H3A50; (aq) →Mn?" (aq) + H3AsOa(aq) Split the reaction into two half-reactions. Piece #2 (1/2 pt) Consider the following half-reaction: MnO2(s) Mn2+ (aq) Balance everything but oxygen and hydrogen atoms. Piece #3 (1/2 pu) Take your answer to Piece #2 and balance the oxygen by adding a water to add oxygen where needed. hyon Piece #4 (1/2 pu) Take your answer to Piece #3 and balance the H'...
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...
Problem 1: Balance the following reaction in (a) acidic solution and (b) basic solution MnO2 (s) + H Asos (aq) → Mn2+ (aq) + HASO (aq) (a) Acidic solution 1. Split the reaction into two half-reactions. Mn q + ac Mnat HAs Oy > Hj As Oy + ae" 2. Consider the following half reaction: MnO2 (s) → Mn2+ (aq) Balance everything but oxygen and hydrogen atoms. MnOade > Moi 3. Take your answer to (2) and balance the oxygen...
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)
Write unbalanced oxidation half-reaction for the following process. Mn3+(aq)→MnO2(s)+Mn2+(aq) Express your answer as a chemical equation. Identify all of the phases in your answer. Write unbalanced oxidation half-reaction for the following process. Fe2O3(s)+CO(g)→Fe(s)+CO2(g) Express your answer as a chemical equation. Identify all of the phases in your answer. Write unbalanced reduction half-reaction for the following process. Fe2O3(s)+CO(g)→Fe(s)+CO2(g) Express your answer as a chemical equation. Identify all of the phases in your answer.
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)
1. Consider the unbalanced redox reaction taking place in an acidic aqueous solution VO,* (aq) + S0,- (aq) → VO" (aq) + S0,- (aq) The unbalanced oxidative half-reaction for this redox reaction is: VO,* (aq) → VO" (aq) (la) Because the reaction takes place in aqueous solution, the reaction can be balanced by adding water. a. Add water to reaction (la) to balance the oxygen. This will give reaction (1b). (1b) Because the reaction takes place in an acidic solution,...
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)
Consider the unbalanced half reaction shown below: (MnO4)-(aq) → MnO2(s) When this half reaction is balanced with the lowest possible whole number coefficients how many electrons will there be in the balanced half reaction?
1. A voltaic cell is constructed based on the following redox reaction: Sn2+ (aq) + Mn (s)àSn (s) + Mn2+ (aq) Calculate Ecell at 25 oC under the following conditions: (a) Standard conditions (b) [Sn2+] = 0.0200 M; [Mn2+] = 4.00 M (c) [Sn2+] = 0.500 M; [Mn2+] = 0.00250 M 2. Consider the following redox reaction at 25oC: MnO2 (s)àMn2+ (aq) + MnO4- (aq) (a) Balance the equation in acid (b) Calculate Eocell (c) CalculateDGorxn (d) Calculate K Hint!!!...