For the reaction Ni2*(aq) + 2FE2*(aq) → Ni(s) + 2Fe³*(aq), the standard cell potentlal E'cell IsMultiple ChoiceO -0.52 V.-2.81 V.-1.02 V.1.02 V.-2.81 V.

The answer to this question is given below:

For the reaction NI2*(aq) + 2FE2*(aq) – NI(s) + 2FE3*(aq), the standard cell potential Ecell is Multiple Choice -0.52 V. -2.81 V. -1.02 V. 1.02 V. -2.81 V.

For the reaction NI2(aq) + 2FE2(aq) – NI(s) + 2FE3*(aq), the standard cell potential Ecell is Multiple Choice -0.52 V. -2.81 V. -1.02 V. 1.02 V. -2.81 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...

See similar textbooks

Similar questions

1 2 B A galvanic cell is composed of these two half-cells, with the standard reduction potentials shown: Co2(aq) + 2e Co(s) E° -0.28 volt; Cd2+ (aq) + 2e-Cd(s) E°--0.42 volt. What is the standard free energy change in kJ for the cell reaction of this galvanic cell? Report your answer in whole number. Do not put unit in your answer. Type your answer...
The measured cell potential, Ecel, for the cell shown is -0.3573 V at 25 °C. Calculate the H* concentration. PI(s) | H, (g,0.855 bar) |H* (aq. ? M) || Cd²*(aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell and their respective standard reduction potential values, E", are given. 2H"(aq) + 2e H,(g) Cd (aq) + 2e Cd(s) E = 0.00 V E = -0,403 V 2.45 x10-6 [H*) = Incorect
For the following electrolyte-concentration cell consisting of two cells back to back by electrodes, What is the suitable Nernst Equation at 25 0C? Pt;H2,HCl(a1),AgCl(s),Ag,| Ag, AgCl(s),HCl(a2),H2;Pt
Three voltaic cells can be constructed from solutions Pb(NO3)2(aq) and the corresponding metal electrodes. of Cuso (aq), ZnSOa(aq), and Reaction E Zn?daa) + 2e s zn(s) -0,7626V Pbaas + 2e 5 Pb (S) - 0.1251 V Calculate the standard cell potential for each voltaic cell combination. For a spontaneous reaction, E'cell must be positive when E'anode is subtracted from E'cathode. Use the standard potentlals from p. 119 for calculations. 1. * 2e- ニ Cucs) 0. 340 V Agčaa) e- 5 Ag(s) 0.7991 2. Identify which metal electrode serves as the cathode and which metal electrode serves as the anode. Tabulate the results from questions 1 and 2: E'cell Cell Anode Cathode Cu/Zn Cu/Pb Pb/Zn 3.a. Using the Nernst Equation, calculate the expected voltage (Etheo) for a cell which consists of 0.0300 M Pb(NOs)2(aq) and 0.0400 M CuSO (aq). b. Glve the conventional cell notation for this cell, assuming a salt bridge separates the two half- cells.
Given the following two half-reactions, determine which overall reaction is spontaneous, and calculate its standard cell potential. Cd2*(aq) + 2 e- Cd(s); E° = -0.403 V Zn2"(aq) + 2 e-Zn(s); E° = -0.763 V O A. Cd(s) + Zn2*(aq) OB. Cd(s) + Zn(s)¯ OC. ca²*(aq) + Zn²*(aq)' Cd2+(aq) + Zn(s); E° = -0.360 V Cd2*(aq) + Zn²+(aq); E° = -1.166 V PCd(s) + Zn(s); E° = +1.166 V O D. Cd2+(aq) + Zn(s) cd(s) + Zn2*(aq); E° = +0.360 V
Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e → 2F*(aq) 2.870V Co2+*(aq) + 2e → Co(s) |-0.28OV 2+ Mg"(aq) + 2e → Mg(s) -2.37OV (1) The weakest oxidizing agent is: enter formula (2) The strongest reducing agent is: (3) The strongest oxidizing agent is: (4) The weakest reducing agent is: (5) Will Mg(s) reduce F2(g) to F"(aq)? (6) Which species can be reduced by Co(s)? If none, leave box blank.
Calculate the potential of the cell when; [I] = 0.75 M, pH = 8.90, T= 300 K, P(H2) = 60 torr. Of course (R = 8.314 J/mol.K) and (F = 96500 J/V.mol).
+2 t- 4) Consider the following redox reactions and their standard cell potentials: (acidic conditions) (basic conditions) S,0, (aq) + Cl2(g) = HCI0(aq) + So,"(aq) (acidic conditions) cell =-1.31 V E°cell = +0.10 V E° cell = +0.37 V E°. C2(g) + Bio*(aq) = Bi(s)+ HCIO(aq) So(aq) + 03(g) = S20 (aq) + 02(g) a) Using the ½ rxn method, balance the three redox reactions under the conditions indicated. b) Write each balanced redox reaction in the spontaneous direction and indicate its corresponding standard cell potential. c) Between these 3 redox reactions there are FOUR oxidizing agents and FOUR reducing agents. (Hint: You may need to consider the balanced equations.) i) Place the FOUR oxidizing agents in order of decreasing oxidizing strength. (From the strongest OA to the weakest OA.) ii) Place the FOUR reducing agents in order of decreasing reducing strength. ( (From the strongest RA to the weakest RA.)
The cell potential of the following electrochemical cell depends on the gold concentration in the cathode half- cell: Pt(s) | H2 (g, 1.0 bar) | H+(aq, 1.0 mol L-1) | Au3+(aq, ? mol L-1) | Au(s) What is the concentration of Au3+ in the solution if is Ecell is 1.24 ? Express your answer using two significant figures and don't include the exponent (e.g. if your answer is 2.5×10-4, only write 2.5)
A galvanic cell using Cu"/Cu and Cu?+/Cu was set up at 293 K and the non-standard cell potential was determined to be 0.175 V. Determine the concentration of ions in the cathode's solution if the concentration at the anode is 0.7787 M: (cathode)(M) number (rtol=0.03, atol=1e-08)
Given the following standard reduction half reactions calculate the standard cell potential (E°cell) to 2 decimal places. O2(g) + 4H+ + 4e" 1 4H* (aq) 2H20L) ; E°red. = 1.23 V A13+ (aq) + Зе Al(s) ; E°red. = -1.66 V
9