Tempjetes Symbo Gibbs energy change, ArG", is related to cell potential, Ee. by the equation A,G" = -nFEl Part A where nis the number of moles of electrons transferred and F = 96 500 C mol- is the Faraday's constant. Calculate the standard Gibbs energy change at 25 °C for the following reaction: Mg(s) + Fe?+ (ag)→Mg**(ag) + Fe(s) Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) ndo Tempjetes Symbos 25 kevboard shortcuts Help redo AG = Value Units Submit Part B Calculate the standard cell potential at 25 °C for the reaction X(s) + 2Y*(ag) X (ag) + 2Y(0) where A,H° = -831 k.J mol and A,S° = -319 JK'mol Express your answer to three significant figures and include the appropriate units. > View Available Hint(s) undo redo keyboard shortcuts Help Ecel Value Units

Tempjetes Symbo Gibbs energy change, ArG", is related to cell potential, Ee. by the equation A,G" = -nFEl Part A where nis the number of moles of electrons transferred and F = 96 500 C mol- is the Faraday's constant. Calculate the standard Gibbs energy change at 25 °C for the following reaction: Mg(s) + Fe?+ (ag)→Mg**(ag) + Fe(s) Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) ndo Tempjetes Symbos 25 kevboard shortcuts Help redo AG = Value Units Submit Part B Calculate the standard cell potential at 25 °C for the reaction X(s) + 2Y*(ag) X (ag) + 2Y(0) where A,H° = -831 k.J mol and A,S° = -319 JK'mol Express your answer to three significant figures and include the appropriate units. > View Available Hint(s) undo redo keyboard shortcuts Help Ecel Value Units

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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26. Given the following electrode (reduction) potentials: Ag* + e --> Ag; E° = 0.80 V Zn2+ + 2e --> Zn; E° = -0.76 V For a Voltaic cell represented by the cell notation: Zn(s)|Zn2*(aq)||Ag*(aq)|Ag(s), what is the cell potential (Ecell) when the electrolyte concentrations are as follows: [Ag*] = 1.3 x 10-5 M, and [Zn2*) = 1.0 M ? (A) 2.36 V (B) 1.56 V (C) 0.84 V (D) 0.04 V
Consider the following galvanic cell: Agls) | Ag"(3.0 x 104 M) || Fe3"(1.1 × 10³ M), Fe²"(0.040 M) | Pt(s) Choose the correct cell potential. O Ecel - - 0.12V Ecell = + 0.09 V O Ese = - 0.15 V O Eçel = + 0.12 V eTextbook and Media Hint Determine the sign of the electrodes in the cell. The left side half-cell is the v and charged. The right side half cell is the v and charged. Enter the equation for the spontaneous cell reaction. (Enter states of matter in your answer.)
8. Suppose that the concentrations of NaF and KCI were each 0.10 M in the cell Pb(s) PbF₂(s) F (aq)||Cl(aq)| AgCl(s) Ag(s) Using the half-reactions 2 AgCl(s) + 2e = 2Ag(s) + 2Cl and PbF2(s) +2e = Pb(s) + 2F- and, calculate the cell voltage.
Use the References to access important values if needed for this question. Consider the following half-reactions: Half-reaction E° (V) Br2(1) + 2e → 2Br°(aq)||1.080V 2+ Sn"(aq) + 2e - → Sn(s) ||-0.140OV 2+ Zn"(aq) + 2e¯ →Zn(s)|-0.763V (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 Zn(s) reduce Br2(1) to Br (aq)? (6) Which species can be oxidized by Sn2*(ag)? If none, leave box blank.
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The free energy change for the following reaction at 25 °C, when [H*] = 1.11 M and [Sn2+] = 1.21x10-3 M, is -43.9 %3D kJ: 2H*(1.11 M) + Sn(s) H2(g) + Sn2+(1.21x10-3 M) AG = -43.9 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction v forward reverse
Consider the following cell. Ag(s)|AgCI(s)|NaCI(aq)|Hg2Cl2(s)|Hg(/)|Pt(s) (a) Write the half-cell reactions. (Include states-of-matter under the given conditions in your answer.) Cathode: chemPad Help Greek - Anode: chemPad O Help X.X"| Greek - (b) The standard emfs of the cell at several temperatures are as follows. T/K 291 298 303 311 E°/mV 43.0 45.4 47.1 50.1 Calculate the values of A,G°, A,Sº, and A,H° for the reaction at 303 K. A,G°: A,S° kJ•mol-1 J-mol -1.к-1 %3D A,H° kJ•mol-1
The free energy change for the following reaction at 25 °C, when [Sn2+] = 1.19 M and [Zn2+] = 7.83×10-3 M, is -133 kJ: Sn2+(1.19 M) + Zn(s)→ Sn(s) + Zn2+(7.83×10-3 M) AG = -133 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction?
Q1
For the following electrolyte-concentration cell consisting of two cells back to back by electrodes, What is the suitable Nernst Equation at 25 0C? Pt;H2,HCl(a1),AgCl(s),Ag,| Ag, AgCl(s),HCl(a2),H2;Pt
+|| Σ D. For the cell shown, the measured cell potential, Ecell, is-0.3621 V at 25 °C. Pt(s) | H, (g, 0.853 atm) | H* (aq, ? M) || Cd²+(aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E°, are 2H*(aq) + 2 e¯ – H, (g) A 00'0 = 07 24, Cd2+ (aq) + 2 e Cd(s) E° = -0.403 V %3D Calculate the Ht concentration. M. = [,H] 10:23 AM M. 11/9/2021 7734 F4 F5 F7 F8 F10 F11 F12 PrtScr Insert Delete Eゴ #3 Backspace 2$ ) 4. 5. 9. 7. R } 1 Enter F. K. H. Sh
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.