32. Consider the following two standard reduction potentials:Pt2"(aq) + 2 e → Pt (s); E° = 1.180 VPb2"(aq) + 2 e→ Pb(s); E° = -0.130 V%3DPart 1. Which of the following is the balanced overall reaction and standard cell potential of a working electrochemical (orvoltaic) cell constructed from half-cells with the given half reactions? Note that "working" means that theelectrochemical reaction is spontaneous.a)" Pt2 (aq) + Pb(s) → Pt(s) + Pb²*(aq); Ecelnl= 1.310 V+ Pb(s) → Pt(s) + Pb²*(aq); £%3Db)Pt(s) + Pb²*(aq) → Pt2*(aq) + Pb(s);Ecell -1.310 Vc)Pt2"(aq) + Pb²*(aq)→ Pt(s) + Pb(s);= 1.050 V%3D->celld)" Pr2"(aq) Een=0.655 V+ Pb(s) –Pt(s) + Pb²*(aq);%3Dcelle)Pt(s) + Pb²"(aq) → Pt2*(aq) + Pb(s); £cell=-0.655 Vf) none of the above Part 2. In the above working electrochemical (or voltaic) cell in Part 1, what species is reduced in cathode?a) Pt (s)b) Pt2* (aq)c) Pb (s)d) Pb²* (aq)e) None of the abovePart 3. From Part 1, one can conclude thata) Pt (s) is a stronger reducing agent than Pb (s).b) Pb (s) is a stronger reducing agent than Pt (s).c) Pt (s) is a stronger oxidizing agent than Pb (s).d) Pb (s) is a stronger oxidizing agent than Pt (s).e) none of the above

We have given reduction potential of two half cells. Higher the value of reduction potential of the…

32. Consider the following two standard reduction potentials: Pt2"(aq) + 2 e → Pt (s); E° = 1.180 V Pb"(aq) + 2 e → Pb(s); E° = –0.130 V Part 1. Which of the following is the balanced overall reaction and standard cell potential of a working electrochemical (or voltaic) cell constructed from half-cells with the given half reactions? Note that "working" means that the electrochemical reaction is spontaneous. a) Pt2"(aq) + Pb(s) → Pt(s) + Pb²"(aq); = 1.310 V cell Pt(s) + Pb* (aq) – Pt"(aq) + Pb(s); cell - 1.310 V Pt* (aq) + Pb3 (aq) → Pt(s) + Pb(s); cell = 1.050 V d) p Pr*"(aq) + Pb(s) → Pt(s) + Pb²"(aq); cell 0.655 V e) Pt(s) + Pb²"(aq) → Pt2"(aq) + Pb(s); £cel 0.655 V f) none of the above

32. Consider the following two standard reduction potentials: Pt2"(aq) + 2 e → Pt (s); E° = 1.180 V Pb"(aq) + 2 e → Pb(s); E° = –0.130 V Part 1. Which of the following is the balanced overall reaction and standard cell potential of a working electrochemical (or voltaic) cell constructed from half-cells with the given half reactions? Note that "working" means that the electrochemical reaction is spontaneous. a) Pt2"(aq) + Pb(s) → Pt(s) + Pb²"(aq); = 1.310 V cell Pt(s) + Pb* (aq) – Pt"(aq) + Pb(s); cell - 1.310 V Pt* (aq) + Pb3 (aq) → Pt(s) + Pb(s); cell = 1.050 V d) p Pr*"(aq) + Pb(s) → Pt(s) + Pb²"(aq); cell 0.655 V e) Pt(s) + Pb²"(aq) → Pt2"(aq) + Pb(s); £cel 0.655 V f) none of the above

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 59P

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