Balance the following redox equation and identify the species oxidized and the species reduced Cr2O7-2 (aq) + Sn+2 (aq) ---> Cr+3 (aq) +Sn+4 (aq

Balance the following redox reaction in aqueous basic solution: 3- NO3 (ag) + Fe(CN),- → NO(9) + Fe(CN)6' + Fe(CN)6 (aq) (ад)

Write a balanced redox reaction for the reaction shown below.   Cr(s) │ Cr+3 (aq) ║ Fe+2(aq) │ Fe(s)

Balance the following oxidation-reduction occurring in acidic solution. MnO 4 ^ - (aq)+Co^ 2+ (aq) Mn^ 2+ (aq)+Co^ 3+ (aq) Identify the oxidation half-reaction, reduction half-reactionoxidizing agent and reducing agent as well as balancing in acidic conditions.

Balance the following redox reaction in basic solution. 2+ + Cr(OH)3(s) + Cu²+ (aq) Cro (aq) + Cut (aq) 2+ Cr(OH), (s) + Cu²+ (aq) → Cro¾¯ (aq) + Cut (aq)

Balance the following redox reaction that occurs in a basic solution: N₂O₄(aq) + TeO₃²⁻(aq) → Te(s) + NO₃¹⁻(aq))

Complete and balance the following redox equation in basic solution. Br2(l) + Al(OH)4–(aq) ⟶ Br–(aq) +  AlO42–(aq)

Write balanced half-reactions for the following redox reaction: 2+ 2+ 3+ MnO4(aq) +8 H* (aq) +5 Fe²+ (aq) Mn²+ (aq) + 4H₂O(1)+5 Fe³+ (aq)

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2103 (aq) +12H* (aq) + 5Co (s) → 1₂ (s) + 6H₂O (1) +5Co²+ (aq) 2+ Suppose the cell is prepared with 5.23 M IO3 and 2.31 M H in one half-cell and 6.84 M Co in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.

Balance the following redox reaction in acidic solution. Fe²+(aq)+MnO2(s) Fe3+ (aq)+Mn2+ (aq) Fe2+ (aq) + MnO2 (s) - - Fe3+ (aq) + Mn2+(aq) ローロ ē ☑