Fill in the coefficients you get from balancing the the reaction below using the half-reaction method. Be sure you simplify all the coefficients into the smallest whole number ratios for this final answer (i.e.- Standard Form). If the substance does not appear in the final equation put a "0" for the coefficient and don't forget to place a "1" in the spaces where the coefficient of 1 goes. If you leave the space blank it will be marked incorrect. (Reaction j) MnO4 (aq) + CHSCH3(aq) + H20(1) + H*(aq) ----------> C&H&CO2(aq) + Mn2 (aq) + H20(1) + H*(aq) How many electrons were transferred in the balanced reaction? electrons

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Predict products and states as needed.  Balance each equation.  Check yes or no regarding oxidation-reduction (redox) behavior.  Type each reaction with one of the following terms.  Be sure to put in states as needed (??).   Double-Replacement, Neutralization (DR-N)            Combustion (C)          Single Replacement (SR)    Combination or Synthesis (S)                        Double Replacement, Precipitation  (DR-PPT) Decomposition (D)     a) H2O2 (l)    →    H2O (l)   +  O2 (g)                                                         Redox? Y £   N £                                                                                                                           Reaction Type _____     b) Mg(OH)2 (s)  +  CH3COOH (aq) →  ?    +    ?                                                                          Redox? Y £   N £…

. In performing the lab reaction, the student made a mixture of 3 reaction components in a beaker. This was done by mixing 13.00 mL of 0.00250 M Fe³(aq) with 11.00 mL of 0.00250 M SCN (aq) and 6.00 ml. of deionized H₂O. Upon mixing these solutions (total volume of 30.00 mL), the final solution turned a deep. red color. The absorbance of this equilibrium mixture was measured and the concentration of Fe(SCN)2 was determined to be 3.00 x 10 M with the use of the Beer's Law constant (k). Determine the equilibrium constant (K) for the reaction from these values by completing the ICE table below. Be sure to report your final value of K at the bottom. (5 points) 3/15 Initial (mmol) Fe³+ Equilibrium (M) (aq) Fe (aq) 0.008 Change (mmol) -3X105 Equilibrium (mmol)X106 + SCN- (aq) Fet][SCN) 3X105 SCN (aq) = Fe(SCN)2- (aq) Fe(SCN)² (aq) 0 +3×105 X 0.02 3x05 7.7x1556 3 x 105 3.00 x 105 M 2+ Fe ² (aq) + SON (ag) → Fe (SCN) ²+ (aq) (fe+³) = 13X 0.002 = 0.008 30 SCN³) = 30X0.002 0.02 30 Fet ³ (aq) +…