Find Ecell for an electrochemical cell based on the following reaction with [MnO4−]=1.50M, [H+]=1.50M, and [Ag+]=0.0140M. E∘cell for the reaction is +0.88V. MnO4−(aq)+4H+(aq)+3Ag(s)→MnO2(s)+2H2O(l)+3Ag+(aq) Find for an electrochemical cell based on the following reaction with , , and . for the reaction is . 0.75 V 1.01 V 0.84 V 0.92 V
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Find Ecell for an electrochemical cell based on the following reaction with [MnO4−]=1.50M, [H+]=1.50M, and [Ag+]=0.0140M....
19. Calculate EceLL (in V to two decimal places) for an electrochemical cell based on the following half-reactions at equilibrium. In addition, determine ΔG° (in kJ mol-1 to two decimal places) for the reaction under standard conditions (i.e. all concentrations are 1.0 M) and predict the magnitude of K (e.g. very small, very large, etc.) E (o)0.34 V; E red) 0 9 = 1.68 V oxidation : Cu (s) → Cu2+ (aq, .010 M) + 2e- Reductin: MnO4 (aq, 2.0...
Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Sn(s) Sn2+(aq, 1.8 M) II Ag+(aq, 0.55 M)1 Ag(s) Sn2+ (aq) + 2 e Ag+ (aq) + e- Sn(s) Ag(s) E = -0.14 V E = 0.80 V -0.84 V +0.86 V 0 -0.93 V +1.12 V O 0.92 V
A)2Cu(s)+Mn2+(ag)--> 2Cu+(aq)+ Mn(s)Ecell=??VB)Determine whether the reaction is spontaneous as written.Spontaneous or nonspontaneous?C) MNO2(s)+4H+(aq)+Zn(s)--> Mn2+(aq)+2H2O(l)+Zn2+(aq)Ecell=??VD)Determine whether the reaction is spontaneous as written.Spontaneous or nonspontaneous?E)Cl2(l)+2F-(aq)-->F2(aq)+2Cl-(aq)Ecell=??VF)Determine whether the reaction is spontaneous as written.Spontaneous or nonspontaneous?
An electrochemical cell is based on the following two half-reactions: Ox: Pb(s)→Pb2+(aq, 0.26 M )+2e- Red: MnO-4(aq, 1.50 M )+4H+(aq, 2.7 M )+3e-→MnO2(s)+2H2O(l) Compute the cell potential at 25 ∘C.
For the electrochemical cell based on the following cell reaction: 2 F F2(g latm) + Mn(s) (aq, 0.010M) + Mn²+(aq, 0.10M) Rxns Cathode E [V] F2(g) + 2 e + 2.87 2 F (aq) Mn²+(aq) + 2 - 1.18 e Mn(s) a) Determine E cell b) Determine E cell Ecell Ecell - RT/nF in Q
0 What is the Ecell for the cell represented by the combination of the following 4) half-reactions? 2Hg2+(aq) + 2e-→Hg22+(aq) Cr3t(ag)+3eCr(s) E-0.92 V B) 1.28 V 9) 0.18 V A) 2.12 V D) 1.66 V E)-0.18 V 5) Examine the following half-reactions and select the weakest oxidizing agent among the 5)_ species listed. E。= 0.854 V E1.185 V K+(aq) + e-→ K(s) F20(aq) + 2H+(aq) + 4e-→ 2p-(aq) + H20() E。= 2.153 V A) F2o(ag) B) AuBr4Taq) C) Mn2+(ag) D)...
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Ag concentration is 2.68x10-4 M and the Art concentration is 1.06 M ? 3Ag" (aq) + Al(s) +3Ag(s) + Ap+(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given: Submit Answer Retry Entire Group 4 more group attempts remaining What is the calculated value of the cell potential at 298K for an electrochemical cell...
When the Ag" concentration is 1.34 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.534V. What is the Al concentration? 3Ag+ (aq) + Al(s)_3Ag(s) + Al(aq) Answer: M When the Age concentration is 2.55*10*M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.324V. What is the Cr" concentration? 3Ag*(aq) + Cr(8)_3A%(8) + Cr(aq) Answer: M
An electrochemical cell is based on these two half-reactions: Ox: Pb(s) Pb?" (aq, 0.21 mol L ')+2 e Erode = -0.13 (V) Red: Mno. (aq, 1.40 mol L-)+4 H+ (aq, 1.5 mol L-') +3 e MnO2 (s) + 2 H2O (1) Ecathode = 1.68 (V) Part A Compute the cell potential at 25°C. Express your answer to two decimal places and include the appropriate units. Ecell = Value Units Submit Request Answer
The following electrochemical cell was set up in the lab Ag(s)│Ag(NO3)(aq)││KMnO4(aq), HCl(aq), Mn(Cl)2(aq)│Pt(s) What is Ecell° for this galvanic cell? If a more complete description of the cell is Ag(s)│Ag(NO3)(aq, 0.50 M)││KMnO4(aq, 0.50 M), HCl(aq, 2.5 M), Mn(Cl)2(aq, 0.01 M)│Pt(s), Ag(s) what is Ecell? What is the balanced, spontaneous cell reaction for the cell conditions given in b.?