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V Homework Assignment 1. Balance the following reaction: MnO4BC2042B 6 Mn2 + CO2 in acid a....
Balance the following redox equations by the half-reaction method: (a) Mn2+ + H2O2 → MnO2 +...
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)
Balance the following redox equations by the ion-electron half-reaction method: (a) (acid solution): VŽ+ + V(OH)....
Balance the following redox equations by the ion-electron half-reaction method: (a) (acid solution): VŽ+ + V(OH). - VO2 (b) (acid solution): C 02 + MnO - CO2(g) + Mn (c) (basic solution): Cr(OH), (s) + H2O2 → CrO
Assignment 8 - Electrochemistry 1. Consider the reaction: 2Felip) +2170g) →2Feldg) +12(aq) Is the reaction spontaneous?...
Assignment 8 - Electrochemistry 1. Consider the reaction: 2Felip) +2170g) →2Feldg) +12(aq) Is the reaction spontaneous? Explain. (2 marks) (3 marks) 2. Balance the following half-reaction: CO2- C(OH), (basic) (3 marks) 3. Balance the following redox reaction: CIO, +Al+CI+A1 (acidic) 4. Consider the following reaction: Cr20,2- +6Br” +14H2Cr +3Bry + 7H,0 In a redox titration, 15.58 mL of 0.125 M Cr,0,2- was needed to completely oxidize the Br" in a 25.00 mL sample of NaBr. Calculate the (Br") in the...
1. (a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) BiO;- (aq)...
1. (a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) BiO;- (aq) → BIO+ (aq) (ii) (acid solution) C002 (s) → Co2+ (aq) (iii) (base solution) Cr(OH).- (aq) → CrO2- (aq) (iv) (base solution) TeO 2- (aq) → H.Te0.2- (aq) (b) Which of the above equations are oxidation half-reactions? (c) Give the formulas of the reactants that become oxidized in the course of the reaction.
Balance each of the following in BASE: a) CN-+ MnO4-®CNO-+ MnO2(hint: treat CN as a UNIT with...
Balance each of the following in BASE: a) CN-+ MnO4-®CNO-+ MnO2(hint: treat CN as a UNIT with a single oxidation number…this shortcut will not show you which of C or N is being oxidized or reduced, but it will show you whether oneof them is being oxidized or reduced, which will give you the info you need. This is harder than something I’d put on the exam). b) Mn2++ H2O2®MnO2+ H2O (hint: H2O2has oxygen in the RARE -1 oxidation state. One more...
2. Balance the following redox equations by the ion-electron half-reaction method: (a) (acid solution): MnO (s)...
2. Balance the following redox equations by the ion-electron half-reaction method: (a) (acid solution): MnO (s) + PbO2 (s) → MnO,- + Pb2+ (b) (acid solution): MnO4 + Mn2+ → MnO2 (s) (c) (basic solution): Al (8) + OH → Al(OH) - + H2(g)
Balance the following redox equations by the ion-electron half-reaction method: (a) (acid solution): MnO2 (s) +...
Balance the following redox equations by the ion-electron half-reaction method: (a) (acid solution): MnO2 (s) + Cl → Mn2+ + Cl2 (g) (b) (acid solution): NaBiO; (s) + Ce3+ BiO+ + Ce4+ + Na+ (c) (basic solution): Fe(OH)2 (s) + CrO42- → Fe,0, (s) + Cr(OH)4
1. (a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) HSO3- (aq)...
1. (a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) HSO3- (aq) → SO42- (aq) (ii) (acid solution) Pu(OH)4 (8) ► Pu+ (aq) (iii) (base solution) CN- (aq) → OCN- (aq) (iv) (base solution) RhO42- (aq) → Rh,03 (s) (b) Which of the above equations are oxidation half-reactions? (c) Give the formulas of the reactants that become oxidized in the course of the reactic Balance the following redox equations by the ion-electron half-reaction method: (a) (acid...
1. Balance the following reaction in acidic solution. I-(aq) + MnO4-(aq) Mn2+(aq) + I2(s) 2....
1. Balance the following reaction in acidic solution. I-(aq) + MnO4-(aq) Mn2+(aq) + I2(s) 2. Write a balanced net ionic equation for the following reaction in basic solution using both methods for balancing a redox reaction: Zn(s) + NO3-(aq) à NH3 (aq) + Zn(OH)42- (aq) 3. Write a balanced net ionic equation for the following reaction in basic solution using both methods for balancing a redox reaction: MnO4-(aq) + C2H5OH(aq) à Mn2+(aq) + HC2H3O2 (aq)
Balance the following reaction in ACIDIC conditions: H2C204 + Mn04" ---> CO2 + Mn2+ How many...
Balance the following reaction in ACIDIC conditions: H2C204 + Mn04" ---> CO2 + Mn2+ How many water molecules are there and are they a reactant or a product?
Balance the following redox equations by the ion-electron half-reaction method: (a) (acid solution): VŽ+ + V(OH). - VO2 (b) (acid solution): C 02 + MnO - CO2(g) + Mn (c) (basic solution): Cr(OH), (s) + H2O2 → CrO
Assignment 8 - Electrochemistry 1. Consider the reaction: 2Felip) +2170g) →2Feldg) +12(aq) Is the reaction spontaneous? Explain. (2 marks) (3 marks) 2. Balance the following half-reaction: CO2- C(OH), (basic) (3 marks) 3. Balance the following redox reaction: CIO, +Al+CI+A1 (acidic) 4. Consider the following reaction: Cr20,2- +6Br” +14H2Cr +3Bry + 7H,0 In a redox titration, 15.58 mL of 0.125 M Cr,0,2- was needed to completely oxidize the Br" in a 25.00 mL sample of NaBr. Calculate the (Br") in the...
1. (a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) BiO;- (aq) → BIO+ (aq) (ii) (acid solution) C002 (s) → Co2+ (aq) (iii) (base solution) Cr(OH).- (aq) → CrO2- (aq) (iv) (base solution) TeO 2- (aq) → H.Te0.2- (aq) (b) Which of the above equations are oxidation half-reactions? (c) Give the formulas of the reactants that become oxidized in the course of the reaction.
2. Balance the following redox equations by the ion-electron half-reaction method: (a) (acid solution): MnO (s) + PbO2 (s) → MnO,- + Pb2+ (b) (acid solution): MnO4 + Mn2+ → MnO2 (s) (c) (basic solution): Al (8) + OH → Al(OH) - + H2(g)
Balance the following redox equations by the ion-electron half-reaction method: (a) (acid solution): MnO2 (s) + Cl → Mn2+ + Cl2 (g) (b) (acid solution): NaBiO; (s) + Ce3+ BiO+ + Ce4+ + Na+ (c) (basic solution): Fe(OH)2 (s) + CrO42- → Fe,0, (s) + Cr(OH)4
1. (a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) HSO3- (aq) → SO42- (aq) (ii) (acid solution) Pu(OH)4 (8) ► Pu+ (aq) (iii) (base solution) CN- (aq) → OCN- (aq) (iv) (base solution) RhO42- (aq) → Rh,03 (s) (b) Which of the above equations are oxidation half-reactions? (c) Give the formulas of the reactants that become oxidized in the course of the reactic Balance the following redox equations by the ion-electron half-reaction method: (a) (acid...
Balance the following reaction in ACIDIC conditions: H2C204 + Mn04" ---> CO2 + Mn2+ How many water molecules are there and are they a reactant or a product?
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