1 Write the balanced half reactions of the following reactions: a. NiO2 + 2 H20+ Fe...
Please show all work. Thank you. 1 Write the balanced half reactions of the following reactions: a. NiO2 + 2 H2O + Fe -Ni (OH)2 + Fe(OH)2 in basic solution b. CO2 + 2 NH,OH →CO + N2 + 3H2O in basic solution WRC c. 2 H+ + H,02 + 2 Fe2+ + Fe3+ + 2 H2O in acidic solution CE d. H+ + 2 H2O + 2 MnO4 + 5 SO2 → Mn* + 5 HSO4 in acidic solution
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...
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...
(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...
49) Balance the equations for the following reactions: (a) S203 +12I +S40 (in acidic solution) (b) Co (aq) +HO2 (a) Co(OH)s(s) (in basic solution) (c) [Fe(CN)6]3 (aq) + N2H4(aq) ? [Fe(CN)6]4 (aq) + N2(g) (in basic solution) (d) Mn2+H202 MnO2 + H20 (in basic solution)
1)What is the overall cell reaction of a galvanic cell employing the following half-reactions? NiO2(s) + 2H2O + 2e- ⇄ Ni(OH)2(s) + 2OH-(aq), E°NiO2= 0.49 V; Fe(OH)2(s) + 2e- ⇄ Fe(s) + 2OH-(aq), E°Fe(OH)2= − 0.88 V. A)NiO2(s) + 2Fe(s) + 2H2O → Ni(OH)2(s) + 2Fe(OH)2(s) B)NiO2(s) + Fe(s) + 2H2O → Ni(OH)2(aq) + Fe(OH)2(aq) C)NiO2(s) + Fe(s) + 2H2O → Ni(OH)2(s) + Fe(OH)2(s) D)Ni(OH)2(s) + Fe(OH)2(s) → NiO2(s) + Fe(s) + 2H2O 2)What is the standard cell potential of...
Write the balanced redox reaction for each of the following: a. H2O2(aq) + Fe2+(aq) → H2O(l) + Fe3+(aq) in acidic solution b. Cu(s) + HNO3(aq) → Cu2+(aq) + NO(g) + H2O(l) in acidic solution c. Bi(OH)3(s) + SnO22–(aq) → Bi(s) + SnO32–(aq) in basic solution
A chemist designs a galvanic cell that uses these two half-reactions: standard reduction potential half-reaction + O2(9)+4 H (aq)+4e' 2H20) = 1.23 V red Ered Fe+. (аq) Fe3(aq)+e = +0.771 V Answer the following questions about thiss cell Write a balanced equation for the half-reaction that happens at the cathode Write a balanced equation for the half-reaction that happens at the anode Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous...
Assuming the following pair of half-reactions below takes place in an acidic solution, write a balanced equation for the overall reaction. Fe-Fe3+ + 3e Bry+2e2Br Fe+Br2+ Fe3+ + 2Br te Fe+Br2+ Fe3+ + 2Br 2Fe +3Br2+2Fe3+ + 6Br"
Fill in the blanks with the appropriate numbers to balance the half reactions and the overall reactions. Note: H,O, OH", H,0 and e" (and CT") are repeated on both sides, obviously some will be 0. 1) MnO, + Cu - MnO, + Cu?" in acidic solution. MnO, + 2 H,0 + OH' + 3 e MnO, + OH,O + 4H+ Oc I Cu + OH,O + OH+ 0 0 - | Cu? + OH,O + OH' + 20 3 Cu...