Write the balanced half-reactions and a balanced redox equation for each of the following reactions in acidic solution:
a.
b.
c.
d.
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EBK BASIC CHEMISTRY
- (7.12) A technician plates a faucet with 0.86 g Cr metal by electrolysis of aqueous Cr2(SO4)3. If 12.5 min is allowed for the plating, what current is needed? Molar mass of Cr: 51.996 g/mol Analysis/Strategy: mass of Cr ® mol Cr mol e¯ (or Faraday) ® coulombs ® amperes Reduction half-reaction of chromium solution to chromium metal: Cr* ,+3, (aq) e¯ ® Cr(s) + chromium solution, Cr2(SO4)3, has the ions: [Cr*3 s04-²] Answer: The current needed is ampere. (2 sig fig)arrow_forwardConsider the unbalanced reaction below occurring in acidic solution: PbO₂ (s) + (aq) Pb2+ (aq) + 1₂(5) Which of the following reactions is the properly balanced net redox reaction? O PbO₂(s) + 21-(aq) + 4H*(aq) O PbO₂(s) +41-(aq) + 4H*(aq) O PbO₂(s) +1-(aq) + 2H*(aq) - O PbO₂(s) + 21-(aq) - 1 Pb2+ (aq) + 12(s) + 2H₂O() Pb2+ (aq) +212(s) + 2H₂O() Pb2+ (aq) + 1₂(s) + H₂O() Pb2+ (aq) + 1₂(s) + O₂(g)arrow_forward(7.7) A voltaic cell based on the half- reactions: In (aq) – In*3(ag) + 2e™ (aq) Br2() +2e¯→ 2Br¯(ag) The standard emf for this cell is +1.46 V. Using the data below, calculate, E'red for the reduction of In*3 to In*1. Br2() + 2e¯ → 2B1¯(ag) (cathode) E red(cathode) = E %3D Br(aq) = +1.06 V (See Table below) Choices: (A) +0.40 V (B) -0.40 V (C) + 2.50 V (D) -2.50 V Answer: E'red for the reduction of In+3 = to In*1 (in volts) STANDARD REDUCTION POTENTIALS at 25°C; Reduction Half Reaction F: (g) + 2e → 2F (aq) HO, (aq) + 2H" (aq) + 2e 2H;0 PbO(3) +4H" (ag) + So (ag) + 2e PbSO(s) + HO MnO. (aq) + 8H" (aq)+ Se+ Ma" (ag) + 4H,o Au" (aq) + 3e Au (s) Ch (g) + 2e 2C (ag) CrO (aq) + 14H" (aq) + 6e →2Cr" (aq) + TH:O MnO: (3) i 4H" (aq) 2e Ma (aq) 2H:0 O: (g) + 4H" (aq) + 4e + 2H:0 Br: () +2e + 2Br (ag) NO, (aq) + 4I" (aq) + 3e + NO (g) + 2H:0 2Hg (aq) + 2e Hg" (aq) Hgr" (aq) + 2e→ 2Hg () Ag (aq) +e Ag (s) Fe (aq) + e Fe (aq) O: (g) - 21 (aq) + 2e HO: (ag) E MnO" (aq) + 2H0 + 3e MnO: (3) + 40H…arrow_forward
- Complete and balance the following redox reaction in basic solution Zn(s) → Zn(OH),*(aq) + H,(g) 4 4- 2- D2+ 3+ 4+ + 1 2 3 4 6. 7 8 9. O3 O6 O7 (s) (1) (g) (aq) + e Zn H* OH Reset • x H,0 Delete 9. 4. 3. 2.arrow_forward(27) What is the value of the equilibrium constant (Keq) when the following redox reaction takes place at 727°C? Mn (s) + Sn¹+ (aq) → Mn²+ (aq) + Sn²+ (aq) (A) 2.55 x 10¹3 (B) 2.76 x 10¹8 (C) 7.62 x 1036 (D) 5.23 x 10-15 (E) 3.62 x 10-1⁹ The most convenient form of the equation for this one might not be on your note sheet. I suggest using: RT ECELL -In K nF (28) An archaeologist claims that a bone in her collection is from a saber-toothed tiger that is believed to have the carbon-1arrow_forwardFill in the blanks: (7.14) In the electrolysis of CUSO4, how much copper is plated out on the cathode by a current of a 0.75A in 10 minutes? (Cu 63.546 g/mol) Analysis/Strategy: ampere & time coulombs ® mol e¯ (or Faraday) ® mol Cu (R mass of Cu Reduction half-reaction of copper solution to copper metal: Cu*²(aq) + e¯ ® Cu(s) copper solution, CUSO4, has the ions: [Cu*2 SOq] Answer: The mass of copper plated out is g Cu. (3 sig fig)arrow_forward
- (7.1b) Complete and balance the following by ion-electron method. Reactions are taking place in acidic solution. b) Mn*2(aq) + BiO3 (aq) Bi* (aq) + Mn04 (aq) Analysis: Oxidation-Half reation: Balancing atoms & charges: Mn*2(aq) Mn04 (aq) H20 - + H* + e Reduction-Half reation: Balancing atoms and charges: BiO3 (aq) H* + Bi* (aq) e H20 Balancing electrons lost & gained Multiply oxidation-half reaction by e's Multiply reduction-half reaction by es Final balanced equation: Continue nextarrow_forwardQuestion 10 of 25 Complete and balance the following redox reaction in acidic solution NO2(g) → NO3 (aq) + NO(g) 04- O+ 2+ 3+ O4+ 1 4 6. 7 9. O2 3 4 O5 O6 07 O8 O9 (s) (1) (g) (aq) H e N H* OH H2O H30* Reset x H2O Delete MacBook Pro 80 000 DII DD F2 F3 F4 F5 F6 F7 F8 F9 F10 %23 %24 3 5 3. 2.arrow_forward9. 8. m Balance the following redox reaction in basic solution. Mn0,(s)+Br,(1) MnO,(aq)+Br (aq) Mno, (s) + Br, (1) - Mno, (aq) + Br (aq) 00arrow_forward
- Complete and balance the following redox reaction in basic solution Zn(s) + 4 OH (aq) Zn(OH), +2 e 04- 02 04+ 1 4. 6. 8 9. 02 (s) (1) (g) (aq) H* H30* e Zn H H20 OH Reset • z H20 Delete 7. LO 3. question 9arrow_forwardComplete and balance the following half-reaction in acidic solution As(s) → H2ASO, (aq) 04- 3. 2+ 口4+ 1 4. 6. 8. 9. 12 Os O6 (s) (1) (g) (aq) As H* H20 H30* OH Resgt • æ H2O Deletearrow_forwardVISUALIZATION Batteries Zn(s) + 2 OH-(aq)→ ZnO(s) + H2O(2) + 2e D:00 HgO(s) + H20(€) + 2e →Hg(2) + 20H (aq) Consider the animation describing opperation of the mercury battery. What is the formula of the oxidizing agent used in the battery? Recheck Next (1 of 6) 2nd attempt Submit Answer Try Another Version 3 item attempts remainingarrow_forward
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