Oxidation : Cu+ (aq) ----------> Cu2+ (aq) + e-
Reduction : Fe3+ (aq) + e- ----------> Fe2+ (aq)
Eocell = Eored - Eoox
= 0.771 - 0.153
= 0.618 V
Q = [Cu2+] [Fe2+] / [Cu+] [Fe3+]
= (0.04) x (0.29) / (0.20 ) (0.13)
= 0.446
Ecell = Eo - 8.314 x 323 / 1 x 96485 ln Q
= 0.618 - 0.02783 ln 0.446
Ecell = 0.640 V
yes . the following cell is spontaneous at 50 °C
9) Is the following reaction spontaneous at 50°C? Cu (0.20M) Cu?"(0.04M)||Fe(0.13M)|Fe? (0.29M)
Calculate for the reaction: Zn! Zn2+ (0.60M)| |Cu2+ (0.20M)|Cu Given the following: Cu2+(aq) + Zn(s) Cu(s) + Zn2+(aq) Eo-1.10V
For the spontaneous as written at 25°C. A) Cu(s) I Cu (0.10 M)IFe (0.0053 M) I Fe(s) O Spontaneous O Not B) Pt(s) ISn2(0.0021 M), Sn (0.15 M) II Fe2 (0.0012 M), Fe (0.12 M) I Pt(s) O Not Spontaneous
A-D
9. Use the data given below for the following reaction at 25 C. Fe 04 (s)+ 4 H2(g) 3 Fe (s) + 4 H2O (1), (12+4+4+10-30) Fe Oa(S) 146.4 APH (kJ/mol) -1118.4 H:(g) 130.6 H2O(I) Fe(s) 27.28 S' (J/K/mol) 69.61 -285.83 0 (5+5+2+5=12) (a) Calculate AS,ys, AS,urr, ASuniy and AG at 25°C. ASy's Hh 172 (b) Is the reaction spontaneous at 25°C from entropic point of view? (4) (c) Is the reaction spontaneous at 25°C from free energy point...
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)...
19. Which of the following describes the net reaction that occurs in the cell, a. Cu Cd2+ - Cu2- +Cd c. Cu2+ Cd2+Cu + Cd d. Cu2+ Cd b. Cu + Cd ? Cu2+ + Cd2+ Cu Cd2+ e. 2Cu 20. direction given) under standard electrochemical conditions? Which one of the following reactions is spontaneous (in the b. Cu Fe Cu Fe2 c. 2Au e. 2Hg +
Consider the following reaction at 25 °C; Cu2+ (aq) + Fe (s) → Cu (s) + Fe2+ (aq); E0cell = 0.78 V (25 °C) What would be the value of Ecell at 25 °C, if [Fe2+] = 0.40 M and [Cu2+] = 0.040 M.
6. Determine whether the following cell reaction is spontaneous or not at 25°C, and calculate a cell potential. Cu Cu +(0.394 M) || Cu²+(0.258 M) Cu Cu²+(aq) + 2e → Cu(s); <° = 0.34 V
If the following reaction could happen spontaneously, which metal (Cu or Fe) is more reactive (has stronger reducing ability) ? Fe + Cu2+ -> Fe2+ + Cu Explain!
Consider the following cell reaction at 18°C: Ca(e)+Cu+ (aq) + Ca2+ (aq) + Cu() Calculate the standard cell potential of this cell from the standard electrode potentials, and from this, obtain AG" for the cell reaction. Calculate AF. Use these values of AN and AG to obtain AS for the cell reaction. Ca²+ (aq) +20 + Ca() --2.76 V Cu? (g) +20 + Cu(s) - 0.84 V AH;(O.*()) -- 542.8 kJ/mol AH;(Out (as)) - 64.8 kJ/mol V AG- AH- kJ...
38. The following redox half reactions are combined in a voltaic cell. Which reaction occurs at the cathode and what is the Eceu? Fe2+(aq) + 2e → Fe(s) E°=-0.44 V Cu²+(aq) + 2e → Cu(s) E°= 0.34 V a) b) c) d) Cu2+(aq) + 2e → Cu(s), Ecell = 0.78 V Fe2+(aq) + 2e → Fe(s), Ecel = 0.78 V Fe2+(aq) + 2e → Fe(s), Ecell =-0.10 V Cu²+(aq) + 2e → Cu(s), Ecel = 0.10 V Cu²+ (aq) +...