Item 11Half-reactionE (V)Cr* (aq) + 3e-- Cr (s)|-0.74Fe* (aq) + 2e-- Fe (s)-0.440Fe+(ag) +e-- Fe2+(s)+0.771Sn4+(aq) + 2e- -Sn2(aq)+0.154Part AThe standard cell potential (E) for the voltaic cell based on the reaction below isV.Sn2(aq) + 2FE3+(aq)2Fe2(aq) + Sn* (aq)O +0.48+1.21-0.46+0.617O +1.39SubmitRequest Answer

In the given reaction, At anode:- oxidation Sn2+→ Sn4++ 2e- E°reduction=+0.514 V At…

Half-reaction E' (V) Cr* (aq) + 3e-- Cr (s) -0.74 Fe2 (aq) + 2e- - Fe (s) -0.440 Fe" (aq) +e- - Fe* (s) 3+ +0.771 Sn** (aq) + 2e- - Sn* (aq) +0.154 Part A The standard cell potential (EC) for the voltaic cell based on the reaction below is V. Sn2* (aq) + 2FE3* (aq) → 2Fe?* (aq) + Sn* (aq) O +0.46 O +1.21 O -0.46 O +0.617 O +1.39 Submit Request Answer

Half-reaction E' (V) Cr* (aq) + 3e-- Cr (s) -0.74 Fe2 (aq) + 2e- - Fe (s) -0.440 Fe" (aq) +e- - Fe* (s) 3+ +0.771 Sn** (aq) + 2e- - Sn* (aq) +0.154 Part A The standard cell potential (EC) for the voltaic cell based on the reaction below is V. Sn2* (aq) + 2FE3* (aq) → 2Fe?* (aq) + Sn* (aq) O +0.46 O +1.21 O -0.46 O +0.617 O +1.39 Submit Request Answer

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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7
Using the following half-cell equations and their standard electrode potentials: Fe"(aq) + e 5 Fc2"(aq) E' = +0.77 V Cu?"aq) + 2e 5 Cu(s) E = +0.34 V what is the cell diagram? A Pt|Fe?"aq), Fe"(aq) || Cu²"(aq) | Cu(s) B Cu (aq)| Cu(s) || Fe²"aq), Fe"(aq) | 32. Pt c Cu(s)|Cu²*(aq) || Fe²"aq), Fe*"(aq) | Pt D Pt| Fe"(aq), Fe²“aq) || Cu(s) | Cu²"(aq)
Part A If a voltaic cell is created between a Am"/Am electrode and a Fe*/Fe electrode, what species is being oxidized? O Am"(ag) O Fe(s) O Fe"(ag) O Am(s)
Consider the following half-reactions: Half-reaction E° (V) 2+ Hg"(aq) + 2e → Hg(1) 0.855V Co**(aq) + 2e → Co(s) -0.280V 2+ Fe"(aq) + 2e → Fe(s) |-0.440v (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Hg*(aq) oxidize Fe(s) to Fe2*(aq)?| (6) Which species can be oxidized by Co2*(aq)? If none, leave box blank.
q19
6. The above diagram shows a Galvanic constructed from Ag|AGNO3(aq) and Ni|Ni(NO3)2(aq) half-cells and the half-cell electrode potentials are as follows: Ag*(aq) + e--> Ag(s); E° = 0.80 V %3! Ni2*(aq) + 2e --> Ni(s); E° = - 0.23 V Calculate the Ecell at 25°C when the electrolyte concentrations are: [Ag*] = 1.3 x %3D 10-4 M and [Ni2+] = 0.10 M. %3D
For the galvanic cell: Zn(s) + 2Tl+(aq) 2Tl(s) + Zn2+(aq) Eocell = 0.42 V The standard reduction potential for the half cell Zn2+(aq) + 2e– Zn(s) is Eored = –0.76 V What is the standard reduction potential for Tl+(aq) + e– Tl(s) Eored = ? V a. +0.17 V b. –0.17 V c. –0.34 V d. +0.34 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.
Consider the following half-reactions: Half-reaction ° (V) Br2(1) + 2e → 2Br°(aq) |1.080V Sn²+ (aq) + 2e . Sn(s) |-0.140V Zn2*(aq) + 2e → Zn(s)|-0.763V (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Br2(0) oxidize Zn(s) to Zn2*(aq)? (6) Which species can be oxidized by Sn2*(aq)? If none, leave box blank.
For the galvanic cell: Zn(s) + 2TI*(aq) 2TI(s) + Zn2*(aq) What is E°cel? Standard Electrode Potentials: Zn2*(aq) + 2e Zn(s) E° = -0.76 V TI*(aq) + eTI(s) E° = -0.34 V O 0.42 V O -0.42 V O 1.1 V O -1.1 V
Calculațe Eo cell from the tabulated standard reduction potentials for each of the following reactions in aqueous solution. Then calculate AG° and K at 25°C from E° cell' F = 9.65 x 10 J/V•mol e R = 8.314 J/mol•K Acidic solution Standard reduction potential, E (Volts) Cu2" (ag) + e Cu'(ag) + e Cu(s) Mno, (aq) + 8H"(aq) + 5e Mn?"(aq) + 4H,0 Fe (aq) + e – Fe? (aq) Cu*(aq) 0.153 0.521 1.507 0.771 Basic solution Zn(OH) (s) + 2e → Zn(s) + 40H (aq) Mno, (aq) + 2H,O + 3e MnO,(s) + 4OH(aq) -1.22 0.588
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)