Fill in the Blank 2 points Question at position 4 Consider the UNBALANCED redox reaction: NH3 (aq) + MnO4 (aq) MnO2 (s) + NO3 (aq) Part A: Balance the half-reactions (acidic solution). Hint: The coefficients are only for each half-reaction balanced individually before they are combined. Enter each coefficient as a whole number. Balance charge with e Balance H with H+ Balance O with H2O (if no e, type 0) (if no H+, type 0) (if no H2O, type 0) Type coefficient to balance all atoms but O and H (if no H2O, type 0) (if no H+, type 0) (if no e, type 0) e + H+ + H2O + NH3 (aq) NO3 (aq) + H2O + H+ + e Half-Reaction 1 Question Blank 1 of 39 0 Question Blank 2 of 39 0 Question Blank 3 of 39 3 Question Blank 4 of 39 1 Question Blank 5 of 39 1 Question Blank 6 of 39 0 Question Blank 7 of 39 9 Question Blank 8 of 39 8 e + H+ + H2O + MnO4 (aq) MnO2 (s) + H2O + H+ + e Half-Reaction 2 Question Blank 9 of 39 3 Question Blank 10 of 39 4 Question Blank 11 of 39 0 Question Blank 12 of 39 1 Question Blank 13 of 39 1 Question Blank 14 of 39 2 Question Blank 15 of 39 0 Question Blank 16 of 39 0

Part D: What is the balanced net redox reaction (acidic solution)? Hint: On a separate piece of paper, combine the half-reactions after multiplying by the factors in Part C and simplify the overall redox equation to the net redox reaction by removing chemical species that occur on both sides of the equation. Enter each coefficient as a whole number. Net e Net H Net H20 (if noe , (if no Ht (if no H20, (if no HO, (if no HT, (if noe , Main Reaction Coefficients type O) type 0) type O) type 0) type 0) type O) e + H+ + H20 + NHg (aq) + MnO4 (aq) - Mno2 (5) + NO3"(aq) + HZO + H +e Balanced Redox 0 5 0 3 8 8 3 type your al type your al 0 Reaction