TABLE 17.1 Standard Reduction Potentials at 25°CE°(V)Reduction Half-Reaction2 F (aq)F(g) + 2eH;O,(ag) + 2 H*(aq) + 2 eMnO, lag) + 8 H"(ag) + 5eClg) + 2eCr,0,"(ag) + 14 H*(aq) + 6 eOg) + 4 H*(aq) + 4eBry() + 2eAg*(ag) + eFe"(ag) + eOg) + 2 H*(ag) + 2eIyls) + 2eOg) + 2 H,O) + 4eCu*(ag) + 2 eSnt"(ag) + 202.87WeakerStrongeroxidizingagentreducing2 H;ODMn"(ag) + 4 H,O)2 CHag)→2 Cr*cag) + 7 H;On- 2 H¿O)→ 2 Bríag)Ag(s)1.781.51agent1.361.331.231.090.800.77H;O;laq)0.700.544 OH"Gag)0.40» Cuts)→ Sn°"(aq)→ H;(g)0.340.152 H*(ag) + 20P (ag) + 2eNi"(ag) + 2 eCd" (ag) + 2eFe"(ag) + 2eZn"(ag) + 2ePb(s)-0.13Ni(s)-0.26» Cd(s)→ Fets)-0.40-0.45Zn(s)-0.762 H;O) + 2e• H;(g) + 2OHlnq)-0.83Al(ag) + 3eMg"(ag) + 2 eNa*(ag) + eLi"(ag) + eAl(s)-1.66Mg(s)→ Na(s)-2.37WeakerStrongerreducingagent-2.71oxidizingagentLi(s)-3.04Using Table 17.1, find E° for 2 H 20( )→ 2 H 2( g) + O 2(5).-2.06 V-0.40 V-1.23 V-0.80 V

At Anode :- 2 H2O (l) -----> O2 (g) + 4 H+ (aq) + 4 e- At Cathode :- { H+ (aq) + e- ------>…

TABLE 17.1 Standard Reduction Potentials at 25°C Reduction Half-Reaction (V) 2 F (nq) F(g) + 2e H;O,(ag) + 2 H*Caq) + 2 e MnO, lag) + 8 H"(ag) + 5e Clg) + 2e Cr,0,"(ag) + 14 H*(aq) + 6e Og) + 4 H*(aq) + 4e Bry() + 2e Ag*(aq) + e Fe"(ag) + e Ogg) + 2 H*(aq) + 2e Iyls) + 2e Og) + 2 H;O) + 4 e Cu*(ag) + 2 e Snt"(aq) + 2e 2.87 Weaker Stronger oxidizing 1.78 reducing 2 H;O) Mn(ag) + 4 H;O) 2 CHag) →2 Cr*cag) + 7 H;On - 2 H¿O) → 2 Brtag) Ag(s) Fe²*(aq) H;O,laq) agent 1.51 agent 1.36 1.33 1.23 1.09 0.80 0.77 0.70 0.54 4 OH"Gaq) » Cuts) → Sn°"(aq) 0.40 0.34 0.15 2 H*(aq) + 2 e H;(g) P (ag) + 2e Ni"(ag) + 2 e Cd"(ag) + 2e Fe"(ag) + 2e Zn"(ag) + 2e Pb(s) -0.13 Ni(s) -0.26 → Cd(s) → Fels) -0.40 -0.45 Zn(s) -0.76 2 H;O) + 2e Al(ag) + 3e Mg"(ag) + 2 e Na*(aq) + e Li'(ag) + e • H;(g) + 2OHnq) → Al(s) Mg(s) → Na(s) -0.83 -1.66 -2.37 Stronger reducing agent Weaker -2.71 oxidizing agent Li(s) -3.04 Using Table 17.1, find E° for 2 H 20( )→ 2 H 2( g) + O 2(5). -2.06 V -0.40 V -1.23 V -0.80 V

TABLE 17.1 Standard Reduction Potentials at 25°C Reduction Half-Reaction (V) 2 F (nq) F(g) + 2e H;O,(ag) + 2 HCaq) + 2 e MnO, lag) + 8 H"(ag) + 5e Clg) + 2e Cr,0,"(ag) + 14 H(aq) + 6e Og) + 4 H(aq) + 4e Bry() + 2e Ag(aq) + e Fe"(ag) + e Ogg) + 2 H(aq) + 2e Iyls) + 2e Og) + 2 H;O) + 4 e Cu(ag) + 2 e Snt"(aq) + 2e 2.87 Weaker Stronger oxidizing 1.78 reducing 2 H;O) Mn(ag) + 4 H;O) 2 CHag) →2 Crcag) + 7 H;On - 2 H¿O) → 2 Brtag) Ag(s) Fe²(aq) H;O,laq) agent 1.51 agent 1.36 1.33 1.23 1.09 0.80 0.77 0.70 0.54 4 OH"Gaq) » Cuts) → Sn°"(aq) 0.40 0.34 0.15 2 H(aq) + 2 e H;(g) P (ag) + 2e Ni"(ag) + 2 e Cd"(ag) + 2e Fe"(ag) + 2e Zn"(ag) + 2e Pb(s) -0.13 Ni(s) -0.26 → Cd(s) → Fels) -0.40 -0.45 Zn(s) -0.76 2 H;O) + 2e Al(ag) + 3e Mg"(ag) + 2 e Na(aq) + e Li'(ag) + e • H;(g) + 2OHnq) → Al(s) Mg(s) → Na(s) -0.83 -1.66 -2.37 Stronger reducing agent Weaker -2.71 oxidizing agent Li(s) -3.04 Using Table 17.1, find E° for 2 H 20( )→ 2 H 2( g) + O 2(5). -2.06 V -0.40 V -1.23 V -0.80 V

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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here is the full question. can you please please not reject it and answer
At a temperature of 25 ° C the galvanic element Pt | MnO4- 0,10M, Mn2 + 0,1M, pH = 1 | Ag + 0.0001M | Ag has the electromotive force 0,80V. Calculate the standard electrode potential of Ag + if E ° (MnO4 -, H + | Mn2 +) = 1.50V