balance pls show work its just to check HW12 Balance the following redox in acidic/basic medium MnO- + Fe2+ → Mn2+ +...
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)
More Practice Balancing Redox Reactions in Acid and Basic Solution Balance the following redox reaction in both acidic and basic solution using the half reaction method outlined in Recitation 10, Part III. 3. Unbalanced: PbO2(s) + Mn2+(aq) → Pb2+ (aq) + MnO4- (aq) 4. Unbalanced: SO42-(aq) + Cr3+(aq) → SO2(g) + Cr2O72-(aq)
Chem101 Lab - Copper Chemistry Balance the redox reactions below: 1) Mno. (aq) + Fe2+ (aq) - Fe3+ (aq) + Mn2+ (aq) in acidic condition 2) Cr20,2-(aq) +-(aq) Cr3+ (aq) + 12 (s) in acidic condition 3) Ni2+ (aq) + S20,2- (aq) → Ni02(s) + S0,- (aq) in basic condition 4) Al(s) + Br03(aq) ALO2(aq) + Br-(aq) in basic condition
5) Balance the following redox reactions. For each one, identify the reducin and the oxidizing agent. (acidic solution) a) Cr2O72- + NO2 = Cr3+ + NO3- (basic solution) b) H O2 + Cio2 = 02 + ClO2- (acidic solution) c) Mnox + VÕ2+ = Mn2+ + V(OH)4* d) AIS) + Noz = NH4+ + A102 (basic solution) e) 103- + 1 = 12 (acidic solution) f) SCN-+ Br03- = Br + SO42- + HCN (acidic solution)
Balance the following redox equations by the ion-electron method: (a) H2O2 + Fe2+ → Fe3+ + H2O (in acidic solution) (b) Cu + HNO3 → Cu2+ + NO + H2O (in acidic solution) (c) CN− + MnO4− → CNO− + MnO2 (in basic solution)
1. Balance the following reactions: a) PbO2 +Mn2+ =Pb2+ + MnO-4 (acidic medium) b) Ce4+ + AsO-2 =Ce3+ + AsO3-4 (basic medium) c) C2O2-4 +MnO-4 = Mn2+ +CO2 (acidic medium) d) CN- +MnO-4 = CNO- + MnO2 (acidic medium) e) CrO-2 + ClO- = CrO2-4 + Cl- ( basic medium)
Balance the following equations. (Use the lowest possible whole-number coefficients. These may be zero.) (a) Cr202-(aq) + NO2 (aq) = Cr3+ (aq) + NO3"(aq) Cr20,2- + NO3 + H+ + H2O= Cr3+ + NO3 + H+ + H20 (b) Mn04 (aq) + CH3OH(aq) Æ Mn2+ (aq) + HCO2H(aq) MnO4 + CH3OH + H+ + H2O= Mn2+ + HCO2H + H+ + H2O (c) ClO2(aq) + H2O2(aq) = C102 (aq) + O2(9) C102 + H2O2 + OH + H20 = ClO2...
Balance following redox reactions in acidic conditions using the half-reaction method a. Fe + Ag+ → Fe2+ + Ag b. I- + SO42- → H2S + I2 c. Cu + NO3- → Cu2+ + NO2 d. PbO₂ + CI- → Pb2+ + Cl₂
POSTLAB 1. Compare your data with that of the class, and discuss. 2. Balance the following redox equations: CrO2 + Fe2+ Cr3+ + Fe3+ (in acidic solution) MnO4 + CIO, MnO, +CIOA (in basic solution) 3. Write balanced net ionic equations for the three reactions carried out in Part A given that the sulfur-containing product is the bisulfate anion. 192
Balance the following redox reactions: a) CN− + MnO4− → CNO− + MnO2 (basic solution) b) O2 + As → HAsO2 + H2O (acidic solution) c) Br− + MnO4− → MnO2 + BrO3− (basic solution) d) NO2 → NO3− + NO (acidic solution) e) ClO4− + Cl− → ClO− + Cl2 (acidic solution) f) AlH4− + H2CO → Al3+ + CH3OH (basic solution)