oxidation half reaction ---------------------------------------------reduction half reaction
Fe^2+(aq) -----> Fe^3+(aq) --------------------------------- MnO4^-(aq) ---------------> Mn^2+(aq)
Fe^2+(aq) -----> Fe^3+(aq) --------------------------------- MnO4^-(aq) ---------------> Mn^2+(aq)+4H2O(l)
Fe^2+(aq) -----> Fe^3+(aq) --------------------------------- MnO4^-(aq) +8H^+(aq)---------------> Mn^2+(aq)+4H2O(l)
Fe^2+(aq) -----> Fe^3+(aq) +e^- ------------------------ MnO4^-(aq) +8H^+(aq) + 5e^- --------------> Mn^2+(aq)+4H2O(l)
5Fe^2+(aq) -----> 5Fe^3+(aq) +5e^-
MnO4^-(aq) +8H^+(aq) + 5e^- --------------> Mn^2+(aq)+4H2O(l)
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5Fe^2+(aq) + MnO4^-(aq) +8H^+(aq) ----------> 5Fe^3+(aq)+Mn^2+(aq)+4H2O(l)
2.
oxidation half reaction ---------------------------------------------reduction half reaction
2I^-(aq) -----> I2(s) --------------------------------------------Cr2O7^2- (aq) -----------> 2Cr^3+ (aq)
2I^-(aq) -----> I2(s) ------------------------------------------ Cr2O7^2- (aq) -----------> 2Cr^3+ (aq) + 7H2O(l)
2I^-(aq) -----> I2(s) ------------------------------------------- Cr2O7^2- (aq) +14H^+(aq) -----------> 2Cr^3+ (aq) + 7H2O(l)
2I^-(aq) -----> I2(s) +2e^- -------------------------------- Cr2O7^2- (aq) +14H^+(aq) +6e^- -----------> 2Cr^3+ (aq) + 7H2O(l)
6I^-(aq) -----> 3I2(s) +6e^-
Cr2O7^2- (aq) +14H^+(aq) +6e^- -----------> 2Cr^3+ (aq) + 7H2O(l)
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Cr2O7^2- (aq) +14H^+(aq)+ 6I^-(aq) ------------------> 2Cr^3+ (aq) + 7H2O(l) + 3I2(s)
3.
oxidation half reaction ---------------------------------------------reduction half reaction
Ni(s) ------> NiO2(s) --------------------------------------------------- S2O8^2-(aq) ---------> 2SO4^2- (aq)
Ni(s) +2H2O(l)------> NiO2(s) ----------------------------------------- S2O8^2-(aq) ---------> 2SO4^2- (aq)
Ni(s) +2H2O(l)+ 4OH^-(aq) -----> NiO2(s) +4H2O(l)----------- S2O8^2-(aq) ---------> 2SO4^2- (aq)
Ni(s) +2H2O(l)+ 4OH^-(aq) -----> NiO2(s) +4H2O(l)+2e^- ----------- S2O8^2-(aq) +2e^- ---------> 2SO4^2- (aq)
Ni(s) +2H2O(l)+ 4OH^-(aq) -----> NiO2(s) +4H2O(l)+2e^-
S2O8^2-(aq) +2e^- ---------> 2SO4^2- (aq)
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Ni(s) + S2O8^2-(aq) + 4OH^-(aq) ---------> NiO2(s) + 2SO4^2- (aq) + 2H2O(l)
4.
oxidation half reaction ---------------------------------------------reduction half reaction
Al(s) -----> AlO2^-(aq) ------------------------------------------BrO3^-(aq) -------> Br^-(aq)
Al(s) +2H2O(l)-----> AlO2^-(aq) ------------------------------BrO3^-(aq) -------> Br^-(aq) + 3H2O(l)
Al(s) +2H2O(l)+4OH^-(aq) ---> AlO2^-(aq) +4H2O(l)+3e^- -BrO3^-(aq) +6H2O(l)+5e^- ->Br^-(aq) +3H2O(l)+6OH^-(aq)
5Al(s) +10H2O(l)+20OH^-(aq) ---> 5AlO2^-(aq) +20H2O(l)+15e^-
3BrO3^-(aq) +18H2O(l)+15e^- ->3Br^-(aq) +9H2O(l)+18OH^-(aq)
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5Al(s) + 3BrO3^-(aq) + 2OH^-(aq) -----------> 5AlO2^-(aq) + 3Br^-(aq) +H2O(l)
Chem101 Lab - Copper Chemistry Balance the redox reactions below: 1) Mno. (aq) + Fe2+ (aq)...
balance pls show work its just to check HW12 Balance the following redox in acidic/basic medium MnO- + Fe2+ → Mn2+ + Fe3+ (acidic) Cr2O72- + C,H-OH → Cr3+ + CO2 (acidic) Ag + CN- + 02 → Ag(CN)2- (basic) Cr2O72- + S032– → Cr3+ + SO42- (acidic) C1,02 + H2O2 → C102 +02 (basic) MnO4 + C H204 → Mn2+ + CO2 (acidic) Sn + NO3- → SnC162- + NO2 (basic)
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 each of the following redox reactions occurring in basic solution MnO-(4) (aq) + Br- (aq) ---> MnO2(s) + BrO3 - (aq)
Complete and balance the following redox reactions in acidic medium, be sure to label the oxidizing and reducing agents in each. S(s) + HNO3(aq) → H2SO3(aq) + N2O(g) BrO3 - (aq) + N2H4(g) → Br- (aq) + N2(g) Complete and balance the following redox reactions in basic medium, be sure to label the oxidizing and reducing agents in each. NO2 - (aq) + Al(s) → NH4 + (aq) + AlO2 - (aq) H2O2(aq) + ClO2(aq) → ClO2 - (aq) +...
[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)
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)
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
1. Balance the following redox equation in acidic solution. What is the coefficient of the water? CH3OH(aq) + CrO72-(aq) --> CH2O(aq) + Cr3+(aq) a. 1 b. 2 c. 4 d. 6 e. 7 2. Balance the following redox equation in basic solution. What is the coefficient of the water? NO2-(aq) + Al(s) --> NH3(g) + AlO2-(aq) a. 1 b. 2 c. 4 d. 6 e. 7
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)
Consider the unbalanced redox reaction: MnO−4(aq)+Zn(s)→Mn2+(aq)+Zn2+(aq) Balance the equation in acidic solution. Part B- Determine the volume of a 0.475 M KMnO4 solution required to completely react with 3.35 g of Zn.