Consider the cell Pt(s)|H2(g,1atm)|H+(aq,a=1)|Fe3+(aq),Fe2+(aq)|Pt(s) given that Fe3++e−⇌Fe2+ and E∘=0.771V at 298.15 K. If the cell potential...
Consider the cell
Pt(s)|H2(g,1atm)|H+(aq,a=1)|Fe3+(aq),Fe2+(aq)|Pt(s) given that Fe3++e−⇌Fe2+ and E∘=0.771V at 298.15 K.
If the cell potential is 0.683 V, what is the ratio of Fe2+(aq) to Fe3+(aq)?
What is the ratio of these concentrations if the cell potential is 0.807 V?
Homework Answers
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Consider the cell
Pt(s)|H2(g,1atm)|H+(aq,a=1)|Fe3+(aq),Fe2+(aq)|Pt(s)
given that Fe3++e−⇌Fe2+ and E∘=0.771V at 298.15 K.
If the cell potential...
Consider the following cell: Pt(s) | Fe3+ (aq). Fe2(aq) | CIF (aq) C12(e) Pt(s) If the...
Consider the following cell: Pt(s) | Fe3+ (aq). Fe2(aq) | CIF (aq) C12(e) Pt(s) If the standard reduction potentials of the Fe3+/Fe2+ and Cl2/Cl" couples are +0.77 and +1.36 V, respectively, calculate the value of Efor the given cell. +1.00 V O +1.77 v +0.59 V +2.13 V +0.95 V
please help! :( Cell potential for the following cell was measured to 0.889 V at 25 ° C Pt (s) H2 (g, 0.95 bar) H(aq...
please help! :(
Cell potential for the following cell was measured to 0.889 V at 25 ° C Pt (s) H2 (g, 0.95 bar) H(aq, 0.0010 M) || Fe3 + (aq 0.0010 M), Fe2 + (aq, 0.010 M) | Pt (s) a) Write the reaction formula for the cell b) Calculate the normal potential of the redox pair Fe3 Fe2+
Consider the following cell diagram: Pt(s) | Fe3+(aq) , Fe2+(aq) || Cl–(aq) | Cl2(g) | Pt(s)...
Consider the following cell diagram: Pt(s) | Fe3+(aq) , Fe2+(aq) || Cl–(aq) | Cl2(g) | Pt(s) The reaction utilized by this cell is Question 8 options: Fe2+(aq) + 2Cl–(aq) --> Fe(s) + Cl2(g) Fe(s) + Cl2(g) --> Fe2+(aq) + 2Cl–(aq) 2Fe3+(aq) + 2Cl–(aq) --> 2Fe2+(aq) + Cl2(g) Fe3+(aq) + Cl–(aq) --> Fe2+(aq) + 1/2Cl2(g) 2Fe2+(aq) + Cl2(g) --> 2Fe3+(aq) + 2Cl–(aq)
1.) Given the following notation for an electrochemical cell Pt(s) | H2(g) | H+(aq) || Ag+(aq)...
1.) Given the following notation for an electrochemical cell Pt(s) | H2(g) | H+(aq) || Ag+(aq) | Ag(s), what is the balanced overall (net) cell reaction? A. H2(g) + 2Ag(s) ® H+(aq) + 2Ag+(aq B. H2(g) + 2Ag+(aq) ® 2H+(aq) + 2Ag(s) C. H2(g) + Ag+(aq) ® H+(aq) + Ag(s D. 2H+(aq) + 2Ag(s) ® H2(g) + 2Ag+(aq) E. 2H+(aq) + 2Ag+(aq) ® H2(g) + 2Ag(s) 2.) Calculate E°cell for the following (nonspontaneous) reaction: Cd(s) + 2Fe3+(aq) ® 2Fe2+(aq) + Cd2+(aq) → A. -0.37...
Separate galvanic cells are made from the following half-cells: cell 1: H+(aq)/H2(g) and Pb2+(aq)/Pb(s) cell 2:...
Separate galvanic cells are made from the following half-cells: cell 1: H+(aq)/H2(g) and Pb2+(aq)/Pb(s) cell 2: Fe2+(aq)/Fe(s) and Zn2+(aq)/Zn(s) Which of the following is correct for the working cells? Standard reduction potentials, 298 K, Aqueous Solution (pH = 0): Cl2(g) + 2e --> 2C1-(aq); E° = +1.36 V Fe3+(aq) + e --> Fe2+(aq); E° = +0.77 V Cu2+(aq) + 2e --> Cu(s); E° = +0.34 V 2H+(aq) + 2e --> H2(g); E° = 0.00 V Pb2+(aq) + 2e --> Pb(s);...
Consider the following electrochemical cell: Pt | Cu2+ (aq) | Cu+ (aq) || Fe2+ (aq) |...
Consider the following electrochemical cell: Pt | Cu2+ (aq) | Cu+ (aq) || Fe2+ (aq) | Fe3+ (aq)| Pt The cell is constructed by preparing one half-cell with a solution containing 8.33 * 10-3 M FeCl3 and 1.67*10-2 M FeCl2, and preparing the other half-cell with a solution containing 8.33*10-3 M CuCl2 and 0.025 M CuCl. Calculate the cell potential once the half-cells are connected to each other. E°(Cu2+/Cu+) = 0.16 V; E°(Fe2+/Fe3+) = 0.77 V
3. For the cell represented by Pt|Fe3+(0.25 M), Fe2+(0.025 M)||Ce4+(0.035 M), Ce3+(0.050 M)|Pt E o (Fe3+/Fe2+...
3. For the cell represented by Pt|Fe3+(0.25 M), Fe2+(0.025 M)||Ce4+(0.035 M), Ce3+(0.050 M)|Pt E o (Fe3+/Fe2+ = +0.771V, Eo Ce4+/Ce3+ = + 1.44V a) Draw the complete cell represented by the above line diagram and label all the components. b) Write the half-cell reactions and complete redox reaction of the cell. c) Calculate the standard cell potential. d) Calculate the cell potential at the non-standard conditions provided above. e) Was the cell reaction spontaneous?
the Answer is (A) 15. For the given electrochemical cell at 298.15 K: Pt|H2(g, f= 1...
the Answer is (A)
15. For the given electrochemical cell at 298.15 K: Pt|H2(g, f= 1 atm)|HCl(aq, m) |AgCl) |Ago) The following figure is obtained from derivation of the Nernst equation at different molalities of HCl : 0.235 y = 0.223 +0.06x 80.230 – Ecent (2RT/F) In(m/mº) 0.225 0.220 + 0.0 0.1 0.2 (m/m9) 12 (2RT) The figure shows the plot of (Ecell + F In (m/m°)) vs (m/mº)1/2 . Calculate the experimental mean activity coefficient V+ of HCl at...
7.50 Consider the following cell. Pt Cu2+, Cu+ Fe2+, Fe3+ | Pt (a) What is the cell reaction? (b) What is the standard...
7.50 Consider the following cell. Pt Cu2+, Cu+ Fe2+, Fe3+ | Pt (a) What is the cell reaction? (b) What is the standard electro- motive force of the cell at 298.15 K? (c) Calculate Ar Gº for the cell reaction from the standard electromotive force. (d) Calcu- late ArGº for the cell reaction using the AfGº values for the ions in Table C.2. (e) Calculate ArGº for the cell reaction using the AfHº values and Sº values in Table C.2.
Consider the following reaction at 298K. 2 Cr3+ (aq) + 2 r (aq) →→2 Cr2+ (aq)...
Consider the following reaction at 298K. 2 Cr3+ (aq) + 2 r (aq) →→2 Cr2+ (aq) + 12 (8) Which of the following statements are correct? Choose all that apply. n=4 mol electrons delta Gº < 0 OK<1 Eºcell < 0 The reaction is product-favored. Consider the following reaction at 298 K. 3 Fe3+ (aq) + Cr(s) – → 3 Fe2+(aq) + Cr3+(aq) Which of the following statements are correct? Choose all that apply. OK<1 n= 3 mol electrons E°...
Consider the following cell: Pt(s) | Fe3+ (aq). Fe2(aq) | CIF (aq) C12(e) Pt(s) If the standard reduction potentials of the Fe3+/Fe2+ and Cl2/Cl" couples are +0.77 and +1.36 V, respectively, calculate the value of Efor the given cell. +1.00 V O +1.77 v +0.59 V +2.13 V +0.95 V
please help! :(
Cell potential for the following cell was measured to 0.889 V at 25 ° C Pt (s) H2 (g, 0.95 bar) H(aq, 0.0010 M) || Fe3 + (aq 0.0010 M), Fe2 + (aq, 0.010 M) | Pt (s) a) Write the reaction formula for the cell b) Calculate the normal potential of the redox pair Fe3 Fe2+
Separate galvanic cells are made from the following half-cells: cell 1: H+(aq)/H2(g) and Pb2+(aq)/Pb(s) cell 2: Fe2+(aq)/Fe(s) and Zn2+(aq)/Zn(s) Which of the following is correct for the working cells? Standard reduction potentials, 298 K, Aqueous Solution (pH = 0): Cl2(g) + 2e --> 2C1-(aq); E° = +1.36 V Fe3+(aq) + e --> Fe2+(aq); E° = +0.77 V Cu2+(aq) + 2e --> Cu(s); E° = +0.34 V 2H+(aq) + 2e --> H2(g); E° = 0.00 V Pb2+(aq) + 2e --> Pb(s);...
the Answer is (A)
15. For the given electrochemical cell at 298.15 K: Pt|H2(g, f= 1 atm)|HCl(aq, m) |AgCl) |Ago) The following figure is obtained from derivation of the Nernst equation at different molalities of HCl : 0.235 y = 0.223 +0.06x 80.230 – Ecent (2RT/F) In(m/mº) 0.225 0.220 + 0.0 0.1 0.2 (m/m9) 12 (2RT) The figure shows the plot of (Ecell + F In (m/m°)) vs (m/mº)1/2 . Calculate the experimental mean activity coefficient V+ of HCl at...
7.50 Consider the following cell. Pt Cu2+, Cu+ Fe2+, Fe3+ | Pt (a) What is the cell reaction? (b) What is the standard electro- motive force of the cell at 298.15 K? (c) Calculate Ar Gº for the cell reaction from the standard electromotive force. (d) Calcu- late ArGº for the cell reaction using the AfGº values for the ions in Table C.2. (e) Calculate ArGº for the cell reaction using the AfHº values and Sº values in Table C.2.
Consider the following reaction at 298K. 2 Cr3+ (aq) + 2 r (aq) →→2 Cr2+ (aq) + 12 (8) Which of the following statements are correct? Choose all that apply. n=4 mol electrons delta Gº < 0 OK<1 Eºcell < 0 The reaction is product-favored. Consider the following reaction at 298 K. 3 Fe3+ (aq) + Cr(s) – → 3 Fe2+(aq) + Cr3+(aq) Which of the following statements are correct? Choose all that apply. OK<1 n= 3 mol electrons E°...
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