Balancing redox equations:
Complete and balance the following redox equation occurring in aqueous solution.
C2O42− + BrO3− → CO2 (g) + Br−
0) Write half reactions
C2O42− ---> CO2
BrO3− → Br−
1)Balance elements other than H,O
C2O4-2 --> 2CO2
BrO3− → Br−
2) Balance O atoms with H2O
C2O4-2 --> 2CO2
BrO3− → Br− + 3H2O
3) Balance H+
C2O4-2 --> 2CO2
6H+ + BrO3− → Br− + 3H2O
4) balance electrons
C2O4-2 --> 2CO2 + 2e-
5e- + 6H+ + BrO3− → Br− + 3H2O
5) Balance electrons (5x2)
5C2O4-2 --> 10CO2 + 10e-
10e- + 12H+ + 2BrO3− → 2Br− + 6H2O
6) Add equations an dcnacel terms
10e- + 12H+ + 2BrO3 + 5C2O4-2 --> 10CO2 + 10e- + 2Br− + 6H2O
12H+ + 2BrO3 + 5C2O4-2 --> 10CO2 + 2Br− + 6H2O
Balancing redox equations: Complete and balance the following redox equation occurring in aqueous solution. &n
Problem 2. Complete and balance the following equations for the reactions occurring in basic solution: a. MnO4-(aq)+C2O42-(aq)→MnO2(s)+CO2(g) b. NO2-(aq) + Al(s) → NH3(g) + Al(OH)4-(aq) Answer: a. 4H2O + 2MnO4- + 3C2O42- → 2MnO2 + 8OH- + 6CO2 b. 5H2O + NO2- + OH- + 2Al → NH3+ 2Al(OH)4-
TIL O ELECTROCHEMISTRY Balancing a complex redox equation in acidic or basic solution Balance the following redox reaction in acidic solution. Br" (aq)+NO3(aq) → Br_(1)+NO(g) Br (aq) + NO, (aq) — Bry() + NO(g) 0-0
Balance each of the following redox reactions occurring in basic solution MnO-(4) (aq) + Br- (aq) ---> MnO2(s) + BrO3 - (aq)
3. Balance the following redox equation for a reaction occurring in acidic solution. PbO2 + Cr*3 + H20 → Pb+2 + Crox+ H+ 4. A 4.65 g piece of copper is placed in 2.10 L of a HCl solution of unknown concentration. After the reaction is complete, there is 1.02 g of copper left. What was the concentration of the HCl in the original solution? H2 gas and CuCl2 were produced during this reaction.
2. Balance the following REDOX reaction in acidic aqueous solution. All species are aqueous unless otherwise indicated. What is the reducing agent? BrO3 + Mg(s) Br2(1) + Mg2+
Complete and balance the following redox reaction in basic solution MnO4-(aq) + Br-(aq) → MnO2(s) + BrO3-(aq) Attempts remaining: 3 Complete and balance the following redox reaction in basic solution 103-(aq) + Re(s) → Re04 (aq) + 10-(aq) Attempts remaining: 3
20. Once you balance the following redox reaction occurring in aqueous solution, there are how many water molecules on the right side? H2O2 + HClO → HCIOg + H2O a. 2 b. 4 c. 6 d. 8
Balance the following redox equations by the half-reaction method: (a) Mn2+ + H2O2 → MnO2 + H2O (in basic solution) (b) Bi(OH)3 + SnO22− → SnO32− + Bi (in basic solution) (c) Cr2O72− + C2O42− → Cr3+ + CO2 (in acidic solution) (d) ClO3− + Cl− → Cl2 + ClO2 (in acidic solution) (e) Mn2+ + BiO3− → Bi3+ + MnO4− (in acidic solution)
Balancing Oxidation–Reduction Reactions (Section)Complete and balance the following equations, and identify the oxidizing and reducing agents:(a) Cr2O72-(aq) + I-(aq)→Cr3+(aq) + IO3-(aq) (acidic solution)(b) MnO4-(aq) + CH3OH(aq) →Mn2+(aq) +HCO2H(aq) (acidic solution)(c) I2(s) + OCl-(aq)→IO3-(aq) + Cl-(aq) (acidic solution)(d) As2O3(s) + NO3-(aq)→H3AsO4(aq) + N2O3(aq) (acidic solution)(e) MnO4-(aq) + Br-(aq)→MnO2(s) + BrO3-(aq) (basic solution)(f) Pb(OH)42-(aq) + ClO-(aq)→PbO2(s) + Cl-(aq) (basic solution)
Balance each of the following redox reactions in basic solution. 18.34 Balance each of the following redox reactions in basic solution. (a) CIO-(aq) + CrO(aq) → C1- (aq) + Cro (aq) (b) Br2(aq) + Br (aq) + BrO3(aq) (c) H2O2(aq) + N H(aq) → N2(g) + H2O(O)