(a)
Interpretation:
The following half reaction in acidic medium should be balanced.
Concept Introduction :
A half reaction for a redox
In oxidation, loss of electrons occurs whereas in reduction, gain of electrons occurs.
A balanced reaction is a reaction in which number of atoms and charges should be equal on both reactant as well as on product side.
(b)
Interpretation:
The following half reaction in acidic medium should be balanced.
Concept Introduction :
A half reaction for a redox chemical reaction shows the half component of a given redox reaction which means it will show the oxidation and reduction of half reactions separately.
In oxidation, loss of electrons occurs whereas in reduction, gain of electrons occurs.
A balanced reaction is a reaction in which number of atoms and charges should be equal on both reactant as well as on product side.
(c)
Interpretation:
The following half reaction in acidic medium should be balanced.
Concept Introduction :
A half reaction for a redox chemical reaction shows the half component of a given redox reaction which means it will show the oxidation and reduction of half reactions separately.
In oxidation, loss of electrons occurs whereas in reduction, gain of electrons occurs.
A balanced reaction is a reaction in which number of atoms and charges should be equal on reactant as well as on product side.
(d)
Interpretation:
The following half reaction in acidic medium should be balanced.
Concept Introduction :
A half reaction for a redox chemical reaction shows the half component of a given redox reaction which means it will show the oxidation and reduction of half reactions separately.
In oxidation, loss of electrons occurs whereas in reduction, gain of electrons occurs.
A balanced reaction is a reaction in which number of atoms and charges should be equal on both reactant as well as on product side.
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Basic Chemistry
- (7.11) A voltaic cell is constructed that uses the following reaction and operates at 298 K: Zn(s) + Cd+2, Cd*2(aq) ® + (S)uZ Zn*2(aq) + Cd(s) a) What is the emf of the cell under standard conditions? Zn*2 (ag) + 2e¯ ® Zn(s) E°cell = -0.76 V cd*2 (aq) + 2e¯ ® Cd(s) E°cell = -0.40 V Answer: The emf of the cell is V. Refer to the Table of Standard Reduction Potential below to solve Question (a). STANDARD REDUCTION POTENTIAL AT 25 °c E() Hall Reaction +0.N0 2 H,O) + ze Hg) + 2OH (a) Hal-Reaction Hall-Reaction E(V) Ag"(ng) +e- Ag(s) --0.83 Aglir(s) +e- Ag(s) + Br (ag) AgCKs) +e- Ag(s) + a"(a) Ag(CN), "(a) +e Ag(s)+ 2CN (a) Ag:Cro(s) + 2e 2 Ag(s) + Cro (ag) +0.10 HO, (a) + H,O) + 2e 3OH (ay) +0.22 H,O(ng) + 2H"(ag) + 2e 2 H;O() -0.31 Hg/ (a) + 2e 2 Hg() +0.45 2g"(ay) + 2e 1Hg (a) -0.15 Hg" (a) + 2e - Hg() +0.01 s) + 2e 21(a) +1.78 +0.79 +0.92 Agl(s) +e- Ag(s) +I(ay) +0.85 Ag(S0,) (ay) +e Ag(s) + 2 S,0 (ap) +0.54 A (ay) + 3e Al(s) HAso,(a) + 2H'(ay) + 2e - HAsOdany) + HO() Ba"(ag) + 2e -…arrow_forward(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_forwardComplete 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
- Complete 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_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_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
- (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(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_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
- 9. 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_forwardConsider the following half-reactions: Half-reaction I₂(s) + 2e →>>> ► 21 (aq) Sn²+ (aq) + 2e™ Sn(s)-0.140V Al³+ (aq) + 3e > Al(s) -1.660V (1) The strongest oxidizing agent is: (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Al³+ (aq) oxidize I (aq) to I₂(s)? E° (V) 0.535V (6) Which species can be oxidized by Sn2+ (aq)? If none, leave box blank. enter formulaarrow_forwardQuestion 3 of 25 Complete and balance the following half-reaction in acidic solution NO3 (aq) → NO(9g) 04- 2+ 3+ O4+ 1 2 3 4 6. 7 8. 9. 0. 1 O2 O3 O4 O6 (s) (1) (g) (aq) + e H* H20 OH H H3O* Reset • x H2O Delete MacBook Pro 00 000 F4 DII DD F2 F3 F5 F6 F7 F8 F9 FT @ 23 & 吕 %24arrow_forward
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