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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For the cell shown, the measured cell potential, Ecell, is –0.3521 V at 25 °C. Pt(s) | H,(g, 0.785 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) + 2e- - H, (g) E° = 0.00 V Cd²* (aq) + 2e" - Cd(s) E° = -0.403 V Calculate the H* concentration. [H*] = M
Use the References to access important values if needed for this question. Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e → 2F(aq) 2.870V 2+ Pb"(aq) + 2e → Pb(s)||-0.126V - Fe2+ "(aq) + 2e¯ –→ Fe(s) |-0.440V| (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 Fe(s) reduce F2(g) to F(aq)? (6) Which species can be reduced by Pb(s)? If none, leave box blank.
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
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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For the cell shown, the measured cell potential, Ecell, is -0.3587 V at 25 °C. Pt(s) | H, (g, 0.839 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 2 H* (aq) + 2 e H, (g) E° = 0.00 V Cd2+ (aq) + 2 e Cd(s) E° = -0.403 V Calculate the Ht concentration. [H*] = %3D rIC ho C TV OLER EEDO DCD 24 4/2 DELL PrtScr Insert Home End F8 F9 F10 F11 F12 F4 F5 F6 F7
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?
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The cell potential of the following cell is determined using an unspecified concentration of acid. What is [H*]given that the measured cell potential is -0.366 V and the anode reduction potential (E') is 0.222 V at 25°C? Agls) | AgCl(s) | CI(1.0 M) || H*(aq, ? M) | H2(g, 1.0 atm) | Pt(s) O 6.1x 102 M O 3.7 x 103M O 4.9x 105 M