When balancing equations for redox reactions in acidic solutions, which of the steps comes before you balance each half-reaction for O by adding H2O? O Balance each half-reaction for charge by adding electrons Balance each half-reaction for H by adding H* O Balance each half-reaction for all elements except H and O O Write skeletal equations for the oxidation and reduction half-reactions

Write a balanced overall reaction from these unbalanced half-reactions.   Cu⟶Cu2+Cu⟶Cu2+     Ag+⟶Ag

Write the balanced molecular and net ionicequations for the reaction between aluminum metal and silver nitrate. Identify the oxidation and reduction half-reactions.

Balance the following half-reactions by adding the appropriate number of electrons (e-). Then, classify each reaction as an oxidation or reduction half-reaction. Note that for each of the four reactions, one of the gray boxes will be left blank and the other will be filled with electron(s). Use the symbol e- to represent an electron. Part 4 + 12(s) + 6H2O(1) > 2I0-3 + 12H+(aq) + --

Balance the half- reaction in basic solution. Use e as the symbol for an electron. half - reaction: Balance the half-reaction in basic solution. Use e as the symbol for an electron. half-reaction: SOS₂0

10. Balance the following redox reaction using the half-reaction method and tell how many electrons are transferred in the reaction. Ag(s) + CN (aq) +O2 (g) → Ag(CN), + H2O (BASIC medium) HINT: CN- is neither oxidized nor reduced

Write a balanced half-reaction for the reduction of nitrate ion (NO3) to gaseous nitrogen dioxide (NO₂) in acidic aqueous solution. Be sure to add physical state symbols where appropriate. 0 ロ→ロ D₁ X Ś

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 ☑