You have balanced reactions:
1) H2O2 + 2Fe2 + + 2H + → 2H2O + 2Fe3 +
2) 3Cu + 2HNO3 + 6H + → 3Cu2 + + 2NO + 4H2O
3) 2Bi (OH) 3 + 3SnO22- → 3SnO32- + 2Bi + 3H2O
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Write the balanced redox reaction for each of the following: a. H2O2(aq) + Fe2+(aq) → H2O(l)...
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)
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)
Part III: Oxidation and Reduction of H2O2 1. Reduction of H2O2: H2O2(aq) + Cr(OH)3(S) (BASIC) • Observations · Evidence of the oxidation of Cr3+ • Reduction Half Reaction • Oxidation Half Reaction • Overall Balanced Redox Reaction · Explain occurrence or non-occurrence of reaction by calculating cell. 2. Oxidation of H2O2: H2O2(aq) + FeCl3(aq) • Observations • Evidence of the oxidation of H2O2 • Reduction Half Reaction • Oxidation Half Reaction • Overall Balanced Redox Reaction • Explain occurrence or...
(10 pts) Balance the following redox reactions by first separating the oxidation and reduction half-reactions. a. Cut (aq) + Fe (s) Fe3+ (aq) + Cu(s) b. Cu(s) + HNO3 (aq) Cu2+ (aq) + NO (g) (basic solution) c. NH(aq) + O2(g) → N03 (aq) + H2O(l) (acidic solution) d. Cd(s) + NiO(OH)(s) + Ca(OH)2(s) + Ni(OH)2(s) (Nicad battery) e. The oxidation of iodide ion (1) by permanganate ion (MnO4) in basic solution to yield molecular iodine (12) and manganese(IV) oxide...
H2O2 (aq) + Fe?" (aq) → Fe* (aq) + H2O (1) Write a balanced ionic equation for the equation above in an acidic solution. ii) Write a balanced ionic equation for the equation above in a basic solution.
Balancing redox equation in acidic solution, please show work! S2O32-+I2 ----> I-+S4O62- Balancing redox equation in basic solution, using ion-electron method Bi(OH)3+SnO22----->SnO32-+Bi
1)A voltaic cell operates at 298 K according to the following reaction: 4 Fe2+(aq) + O2 (g) + 4 H+(aq) → 4 Fe3+ (aq) + 2 H2O (l) What is the emf of this cell when [Fe2+] = 6.5908E-4 M, [Fe3+] = 0.699 M, pressure O2 = 0.540 atm and pH = 3.10? 2)A voltaic cell operates at 298 K according to the following reaction: 3 Fe2+(aq) → Fe (s) + 2 Fe3+ (aq) What is the emf of this...
1- Consider the following redox reaction: Fe(s) + Cu2+(aq) --> Fe2+(aq) + Cu(s) EoCell = 0.78 V If [Cu2+] = 0.3 M, what [Fe2+] is needed so that Ecell = 0.76 V 2- Calculate the Eocell for the following redox reaction: Cu(s) + 2Ag+(aq) --> Cu2+(aq) + 2Ag(s)
26. Determine the redox reaction represented by the following cell notation. Fe(s) I Fe2+(aq) I| Cu2+(aq) I Cu(s) A) Cu(s) + Fe2+(aq) B) Fe(s)+Cu2+(aq) Cu(s)+ Fe2+(aq) C) 2 Fe(s)+ Cu2+(aq)Cu(s) + 2 Fe2+(aq) D) 2 Cu(s) + Fe2+(aq)Fe(s)+ 2 Cu2+(aq) E) 3 Fe(s) + 2 Cu2+(aq) 2 Cu(s)+3 Fe2+(aq) Fe(s) + Cu2+(aq)
use the example to answer 8,9,10&11 Here's an example: Balance the following redox reaction, which occurs in acidic solution: Fe (aq)+ MnO4'(aq) -Fe (aq) + Mn (aq) Solution: +2 +7 +3 Step 1) +2 Fe2 (aq)+ MnOa (aq) Fe(aq) + Mn2 (aq) Fe (aq) MnO4 (aq) Mn2 (aq) 1 Fe on each side; 1 Mn on each side; no adjustment necessary Fe2 (aq) Fe 3'(aq) + e 5 e + MnO4(aq) Fe (aq) Fe (aq) + e (2+ on each...