[15] Balance the following redox reactions: {3 points
each}
a) Cr2O72-(aq) + Cl-(aq) → Cr3+(aq) + Cl2(g) (acidic medium)
b) Al(s) + MnO4-(aq) → MnO2(s) + Al(OH)4-(aq) (basic medium)
a) Cr2O72-(aq) + Cl-(aq) ? Cr3+(aq) + Cl2(g) (acidic medium)
O.H.R R.H.R
2Cl^- (aq) ------------> Cl2(g) Cr2O7^2- (aq) ----------> 2Cr^3+ (aq)
2Cl^- (aq) ------------> Cl2(g) Cr2O7^2- (aq) ----------> 2Cr^3+ (aq)+ 7H2O(l)
2Cl^- (aq) ------------> Cl2(g) Cr2O7^2- (aq) +14H^+ (aq)----------> 2Cr^3+ (aq)+ 7H2O(l)
2Cl^- (aq) ------------> Cl2(g)+2e^- Cr2O7^2- (aq) +14H^+ (aq)+6e^- ----------> 2Cr^3+ (aq)+ 7H2O(l)
6Cl^- (aq) ------------> 3Cl2(g)+6e^-
Cr2O7^2- (aq) +14H^+ (aq)+6e^- ----------> 2Cr^3+ (aq)+ 7H2O(l)
-----------------------------------------------------------------------------------------------------------
Cr2O7^2- (aq) +6Cl^- (aq) +14H^+ (aq)- ----------> 2Cr^3+ (aq)+3Cl2(g) + 7H2O(l)
b) Al(s) + MnO4-(aq) ? MnO2(s) + Al(OH)4-(aq) (basic medium)
O. H.R R.H.R
Al(s) --------> [Al(OH)4]^- MnO4^- (aq) --------------> MnO2(s)
Al(s) +4H2O(l)--------> [Al(OH)4]^- MnO4^- (aq) --------------> MnO2(s)+2H2O(l)
Al(s) +4H2O(l) +4OH^- (aq) -----> [Al(OH)4]^- + 4H2O MnO4^- (aq) +4H2O(l)------> MnO2(s)+2H2O(l)+ 4OH^-(aq)
Al(s) +4H2O(l) +4OH^-(aq) ---> [Al(OH)4]^- +4H2O+3e^- MnO4^- (aq) +4H2O(l)+3e^- --> MnO2(s)+2H2O+ 4OH^-(aq)
Al(s) +4H2O(l) +4OH^-(aq) ---> [Al(OH)4]^- +4H2O+3e^-
MnO4^- (aq) +4H2O(l)+3e^- --> MnO2(s)+2H2O+ 4OH^-(aq)
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Al(s) + MnO4^- (aq) +2H2O(l) ------------> [Al(OH)4]^- (aq) + MnO2(s)
[15] Balance the following redox reactions: {3 points each} a) Cr2O72-(aq) + Cl-(aq) → Cr3+(aq) +...
Balance the following Redox Equations in Basic Mediums. Redox Reactions in Basic Solution 1. Al(s) + MnO4¯ (aq) ¾® MnO2(s) + Al(OH)4¯ (aq) 2. NO2¯ (aq) + Al(s) ¾® NH3(aq) + AlO2¯ (aq) 3. Cr(s) + CrO42-(aq) ¾® Cr(OH)3(s) Note: Cr(OH)3 is found in BOTH half reactions! 4. Cl2(aq) + Br2(l) ¾® OBr¯ (aq) + Cl¯ (aq) 5. S8(aq) + MnO4¯ (aq) ¾® SO42-(aq) + MnO2(s)
Balance the redox reactions: basic: ClO-(aq)+Cr(OH)4-(aq)----> CrO42-(aq)+Cl-(aq) MnO4-(aq)+Br-(aq)--> MnO2(s)+BrO3-(aq) NO2-(aq)+Al(s)--->NH3(g)+AlO2- Aidic: ClO4-(aq)+Cr(OH)4---->ClO3-(aq)+Cl2(g)
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 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)
Redox Reactions: Balance the reaction and determine which is the oxidizing and reducing agent in each case. 2. Cr* + Sn" Cr: Sn + 3. NaBr + Cl2 → NaCl + Br2 MnO,(s) (basic O2 (g) + 5. MnO (aq) H2O2 (aq) medium) 6. Cr2O72- → Cr+ (aq) SO2 SO2 (aq) (acidic)
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)
How do I solve the following redox reactions? What are the balanced half-reactions? What is the final balanced equation? Problems 1. MnO4 (aq) + SO32- (aq) → MnO2 (s) + SO42- (aq) in basic solution 2. NO2" (aq) + Al(s) NH3(aq) + Al(OH)4 (aq) in basic solution 3. Mn2+ (aq) + NaBiO3 (s) → Bi* (aq) + MnO4 (aq) + Nat (aq) in acidic solution 4. As2O3 (s) + NO3- (aq) → H3ASO4 (aq) + N2O3 (aq) in acidic solution...
Balance each of the following RedOx reactions occurring in basic conditions: Mn2+(aq) + MnO41-(aq) → MnO2(s) Cl2(g) → ClO31-(aq) + Cl1-(aq)
Balance the following redox reactions that occur in basic solution A) Zn (s) + MnO4-1 (aq) -> Zn(OH)4-2 (aq) + MnO2 (s) B) NO3-1 (aq) + Si (s) -> NH3 (aq) + SiO3-2 (aq)