Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations...

Question

Question

Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations provided. Then, determine i

science chemistry

Add a comment Improve this question Transcribed image text

Answer 1

Answer #1

oxidation Pt is) Pt2 lop) +200 - E,9 -1.20V Fear (og) + 200 Fers) - - -0.454 Reduction - Net Reactani. Egl) & EqC2) PE (S) &

Add a comment

Answer 2

Similar Homework Help Questions

Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations...

Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations provided. Then, determine if the cells are spontaneous or nonspontaneous as written. Refer to the table of standard reduction potentials (E Pt(s)Fe2+(aq) Pt2+(aq) + Fe(s) [Fe2+ [Pt2+] = 0.0023 M = 0.011 M The cell is V E = O not spontaneous. O spontaneous Cu(s)2 Ag (aq) Cu2+(aq) + 2 Ag(s) [Cu2+0.031 M [Ag*] = 0.031 M The cell is V E = O...
Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations...

Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations provided. Then, determine if the cells are spontaneous or nonspontaneous as written. QUESTION 1) Pt(s)+Fe2+(aq)−⇀↽−Pt2+(aq)+Fe(s) [Fe2+]=0.0013 M[Pt2+]=0.048 M E= ____ V? The cell is not spontaneous or spontaneous. QUESTION 2) Cu(s)+2Ag+(aq)−⇀↽−Cu2+(aq)+2Ag(s) [Cu2+]=0.017 M [Ag+]=0.017 M E= ____ V? The cell is not spontaneous or spontaneous. QUESTION 3) Co2+(aq)+Ti3+(aq)−⇀↽−Co3+(aq)+Ti2+(aq) [Co2+] = 0.065 M [Co3+] = 0.025 M [Ti3+] = 0.0060 M [Ti2+] = 0.0118 M...
Calculate the cell potential, ? , for the given reactions at 25.00 °C using the ion...

Calculate the cell potential, ? , for the given reactions at 25.00 °C using the ion concentrations provided. Then, determine if the cells are spontaneous or nonspontaneous as written. Refer to the table of standard reduction potentials (?∘red) . Pt(s)+Fe2+(aq)↽−−⇀Pt2+(aq)+Fe(s) [Fe2+]=0.0045 M[Pt2+]=0.022 M ?= V The cell is spontaneous. not spontaneous. Cu(s)+2Ag+(aq)↽−−⇀Cu2+(aq)+2Ag(s) [Cu2+]=0.013 M[Ag+]=0.013 M ?= V The cell is spontaneous. not spontaneous. Co2+(aq)+Ti3+(aq)↽−−⇀Co3+(aq)+Ti2+(aq) [Co2+] = 0.055 M[Co3+] = 0.020 M [Ti3+] = 0.0055 M[Ti2+] = 0.0090 M ?= V...

Question 7 of 16 > Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentr...

Question 7 of 16 > Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations provided. Then, determine if the cells are spontaneous or nonspontaneous as written. Refer to the table of standard reduction potentials (E ). Pt(s) + Fe2+ (aq) = P22+ (aq) + Fe(s) [Fe2+] = 0.0017 M [P12+] = 0.040 M The cell is O spontaneous. O not spontaneous Cu(s) + 2 Ag+ (aq) = Cu2+(aq) + 2 Ag(s) [Cu2+] =...
Calculate the cell potential, ? , for the given reactions at 25.00 °C using the ion...

Calculate the cell potential, ? , for the given reactions at 25.00 °C using the ion concentrations provided. Then, determine if the cells are spontaneous or nonspontaneous as written. Refer to the table of standard reduction potentials (?∘red) . Pt(s)+Fe2+(aq)↽−−⇀Pt2+(aq)+Fe(s) [Fe2+]=0.0014 M[Pt2+]=0.041 M
Based on the sign of the standard cell potential, Ecell, classify these reactions as spontaneous or...

Based on the sign of the standard cell potential, Ecell, classify these reactions as spontaneous or nonspontaneous as written. Assume standard conditions. Refer to the list of standard reduction potentials. Spontaneous as written Nonspontaneous as written Answer Bank Au + (aq) + 3 Ag(s) Au(s) + 3 Ag* (aq) 1,(s) + Cu() — 21(aq) + Cu2+ (aq) Ni2+ (aq) + Pb(s) Ni(s) + Pb2+ (aq)

Calculate the cell potential for the reaction below when the concentrations of ions are: [Ag+ ]...

Calculate the cell potential for the reaction below when the concentrations of ions are: [Ag+ ] = 0.010 M and [Cu2+] = 0.750 M, at 25 °C. Cu(s) + 2Ag+ (aq) --> Cu2+(aq) + 2Ag(s) Given the standard reduction potentials: Cu2+(aq) + 2e– → Cu(s) Eϴ = 0.34 V Ag+ (aq) + e– → Ag(s) Eϴ = 0.80 V (A) 0.35 V (B) 0.44 V (C) 0.46 V (D) 0.48 V (E) 0.57 V
Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 °C Cu(s) Cu2 (0...

Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 °C Cu(s) Cu2 (0.12 M |Fe2 (0.0012 M) Fe(s) E2 =-0.440 V Efe/Fe = 0.339 V Cu2t/Cu Is the electrochemical cell spontaneous or not spontaneous Ecell V as written at 25 °C? not spontaneous spontaneous Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 °C. Pt(s) Sn2(0.0060 M), Sn4+(0.14 M) Fe3+(0.13 M), Fe2+(0.0056 M) Pt(s)...
Pt(s) + Fe2+ (aq) - P+2+ (aq) + Fe(s) [Fe2+] = 0.0083 M [P+2+] = 0.030...

Pt(s) + Fe2+ (aq) - P+2+ (aq) + Fe(s) [Fe2+] = 0.0083 M [P+2+] = 0.030 M The cell is not spontaneous. O spontaneous. Cu(s) + 2 Ag+ (aq) Cu2+ (aq) + 2 Ag(s) (Cu²+] = 0.013 M [Ag+] = 0.013 M The cell is O not spontaneous O spontaneous. Co2+ (aq) + T18+ (aq) [Co2+] = 0.060 M (T3+1 = 0.0060 M Co + (aq) + Ti”+ (aq) Co+] = 0.050 M [Ti?+] = 0.0115 M E-L v The...

Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr2+]=0.891 M...

Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr2+]=0.891 M and [Fe2+]=0.0120 M. Use the standard reduction potentials in this table. Cr(s)+Fe2+(aq)↽−−⇀ Cr2+(aq)+Fe(s) E= V

Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations...

Homework Answers