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

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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