Write the spontaneous reaction of the following reactions as a cell diagram. (If the reaction is notspontaneous, rearrange the reaction to make it spontaneous then write the cell diagram.)Follow the general format of a cell diagram: Anode II Cathodea. Nics) + Sn2+ (aq)Ni2+ (ag) + Sn(s)b. Cu(s) + Fe2+Cu2"(ag) + Fe(s)(ag)Below are standard reduction potential:Cu2+ (aq)+ 2e-Cu (s)E° = +0.34Sn2+ (ag) +Sn (s)E° = -0.142e-Ni2+ (ag) +Ni (s)E° = -0.262e-Fe2* (aq) +Fe (s)Eo = -0.452e-

We have to predict the cell notation of given reaction such that they gives spontaneous reaction.

Vrite the spontaneous reaction of the following reactions as a cell diagram. (If the reaction is not pontaneous, rearrange the reaction to make it spontaneous then write the cell diagram.) ollow the general format of a cell diagram: Anode II Cathode a. Nics) + Sn²* (aq) Ni2* (aq) + Sn(s) b. Curs) + Fe2* (aq) Cu2"(ag) + Fe(s) elow are standard reduction potential: Cu2+ (aq) + 2e- Cu (s) E° = +0.34 Sn2+ (aq) + 2e- Sn (s) E° = -0.14 Ni2+ 2e- Ni (s) E° = -0.26 + Fe2* (aq)+ 2e- Fe (s) Eo = -0.45

Vrite the spontaneous reaction of the following reactions as a cell diagram. (If the reaction is not pontaneous, rearrange the reaction to make it spontaneous then write the cell diagram.) ollow the general format of a cell diagram: Anode II Cathode a. Nics) + Sn²* (aq) Ni2* (aq) + Sn(s) b. Curs) + Fe2* (aq) Cu2"(ag) + Fe(s) elow are standard reduction potential: Cu2+ (aq) + 2e- Cu (s) E° = +0.34 Sn2+ (aq) + 2e- Sn (s) E° = -0.14 Ni2+ 2e- Ni (s) E° = -0.26 + Fe2* (aq)+ 2e- Fe (s) Eo = -0.45

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...

See similar textbooks

Similar questions

Consider the voltaic cell diagrammed below: Pb (s)| Pb²+ (aq)l| H2 (g)| H* (aq) | Pt (s) a) Write the balanced chemical equation that occurs in the voltaic cell depicted in the diagram. b) If the concentration of Pb2+ in this cell is 0.035 M and the pH is 1.60, what pressure of H2 (g) would keep the cell reaction in equilibrium?
What is the reducing agent in the redox reaction represented by the following cell notation? Cd(s) | Cd2+ (aq) || K+ (aq) | K(s) OA. K+ (aq) OB.K(s) c. Cd(s) OD.Cd²+ (aq)
Use the cell notation to answer the question: Pt(s) | Sn2+(aq), Sn4+(aq) || Ag+(aq) | Ag(s) What element represents the cathode in the cell notation? A. Pt(s) B. Sn2+(aq) C. Sn4+(aq) D. +(aq) E. Ag(s)
H11. Consider the voltaic cell H+ (aq, ?? M) H₂(g, 1 atm)||Cu(s) Cu²+ (aq. 0.1 M). Ecell for this cell at 25 C was +0.360V. What was the pH of the anode solution? A. 0 ABCDE B. C. D. E. 0.89 3.2 7.0 11.7
Which of the following is the correct shorthand notation for the overall cell reaction given below. Mg(s) + Cu2+(aq) → Mg2+(aq) + Cu(s) Select one: a. Mg(s) | Mg2+(aq) || Cu2+(aq) | Cu(s) b. Cu(s) | Mg2+(aq) || Cu2+(aq) | Mg(s) c. Mg(s) | Cu2+(aq) || Mg2+(aq) | Cu(s) d. Cu(s) | Cu2+(aq) || Mg2+(aq) | Mg(s)
3. What is the correct cell notation for a voltaic cell based on the reaction below? Ni²*(aq) + Zn(s) → Ni(s) + Zn²*(aq) a) Zn(s) | Zn²*(aq) || Ni²*(aq) | Ni(s) b) Zn(s) || Zn²*(aq), Ni²*(aq) | Ni(s) c) Ni(s) || Ni²*(aq), Zn²*(aq) || Zn(s) d) Ni(s) | Zn² (aq) || Ni²*(aq) | Zn(s) e) Ni(s) | Ni?*(aq) || Zn²*(aq) | Zn(s) :2+ 2+ 2+
Consider the cell diagram: Pb(s)|Pb(NO3)2(aq)||FeCl3(aq)|Fe(s). Write the balanced net-ionic equations for the half-reactions that occur at the two electrodes. a. Anode= b. Cathode=
Given the cell notation: Snis) | Sn2* (aq) || Fe3* (aq) | Fe(s) The oxidation number of Sn 1 Select ] V, Sn is I Select ] Electrons are transferred from [Select] v to I Select )