+ Cell Potential and EquilibriumThe equilibrium constant, K, for a redox reaction is related to the standardpotential, E, by the equationIn K FERTwhere 72 is the number of moles of electrons transferred, F (the Faradayconstant) is equal to 96,500 C/(mol e-). R (the gas constant) is equal to8.314 J/(mol K), and T is the Kelvin temperature.Standard reduction potentials▾ Part AUse the tableExpress your answer numerically.▸ View Available Hint(s)K=ΥΠΙ ΑΣΦ 9Reduction half-reactionAg+ (aq) +eAg(s)Cu²+ (aq) +201>Cu(s)Sn+ (aq) + 4e →→Sn(s)2H+ (aq) +2e →H₂(g)Ni2+ (aq) + 2e →Ni(s)Fe²+ (aq) + 2e →Fe(s)Zn²+ (aq) +2e →Zn(s)Al³+ (aq) + 3e →Al(s)Mg²+ (aq) + 2e →Mg(s)standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 °C) for the following reaction:Fe(s) + Ni²+ (aq) →>Fe²+ (aq) + Ni(s)?E (V)0.800.340.1500.26-0.450.76-1.662.3729 oReview | Constants | Period Part BCalculate the standard cell potential (E) for the reactionif K = 8.82x10-³Express your answer to three significant figures and include the appropriate units.▸ View Available Hint(s)SubmitValueUnitsX(s) +Y+ (aq) X+ (aq) +Y(s)?

Answered: Image /qna-images/answer/f533e901-6886-4e33-9c0b-ff2c9d372427.jpg

+ Cell Potential and Equilibrium The equilibrium constant, K. for a redox reaction is related to the standard potential, E, by the equation nFE RT In K where 11 is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96.500 C/(mol e). R (the gas constant) is equal to 8.314 J/(mol K), and T is the Kelvin temperature. Standard reduction potentials ▼ Part A Express your answer numerically. View Available Hint(s) K= IVE ΑΣΦ ] + Reduction half-reaction Ag (aq) +eAg(s) Cu²+ (aq) + 2e Sn (aq) + 4e Sn(s) 2H+ (aq) +2e →>H₂(g) ? Ni²+ (aq) + 2e Fe2+ (aq) +2e Zn²+ (aq) + 2e AP (aq) + 3e Mg2+ (aq) + 2e Cu(s) Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 °C) for the following reaction: Fe(s) + Ni²+ (aq) >Fe²+ (aq) + Ni(s) E° (V) 0.80 0.34 0.15 0 -0.20 Ni(s) 0.45 Fe(s) Zn(s) Al(s) Mg(s) -2.37 0.76 -1.68 < 29 o Review Constants | Period

+ Cell Potential and Equilibrium The equilibrium constant, K. for a redox reaction is related to the standard potential, E, by the equation nFE RT In K where 11 is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96.500 C/(mol e). R (the gas constant) is equal to 8.314 J/(mol K), and T is the Kelvin temperature. Standard reduction potentials ▼ Part A Express your answer numerically. View Available Hint(s) K= IVE ΑΣΦ ] + Reduction half-reaction Ag (aq) +eAg(s) Cu²+ (aq) + 2e Sn (aq) + 4e Sn(s) 2H+ (aq) +2e →>H₂(g) ? Ni²+ (aq) + 2e Fe2+ (aq) +2e Zn²+ (aq) + 2e AP (aq) + 3e Mg2+ (aq) + 2e Cu(s) Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 °C) for the following reaction: Fe(s) + Ni²+ (aq) >Fe²+ (aq) + Ni(s) E° (V) 0.80 0.34 0.15 0 -0.20 Ni(s) 0.45 Fe(s) Zn(s) Al(s) Mg(s) -2.37 0.76 -1.68 < 29 o Review Constants | Period

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...

See similar textbooks

Similar questions

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?
Consider the following reaction and its AG" at 25.00 °C. Mg(s) + Ni" (aq) – Mg²* (aq) + Ni(s) AG = -408.0 kJ/mol Calculate the standard cell potential, E for the reaction. E = V cell Calculate the equilibrium constant, K, for the reaction. K =
A certain metal M forms a soluble sulfate salt M₂SO4. Suppose the left half cell of a galvanic cell apparatus is filled with a 2.00 M solution of M₂ SO4 and the right half cell with a 10.0 mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 25.0 °C. left Which electrode will be positive? x10 right X Ś ? What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. 0 Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.
= A certain half-reaction has a standard reduction potential Ered +1.24 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 1.00 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the cathode of the cell. Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. 0 O yes, there is a minimum. red Ono minimum Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. O yes, there is a maximum. no maximum 0 E = v red By using the information…
How do you complete part b of this question?
4. A cell uses the following reaction: a. Zn (s) + 2 H* (aq) → Zn²* (aq) + H2 (g) (a) Determine the emf of the cell under standard conditions. (b) When PH,=1.0 atm and [Zn²*] = 1.0 M, the cell potential is 0.560 V. Determine the concentration of H* in the cathode compartment. Zn2“(aq) + 2e¯ → Zn(s) -0.763 2H*(aq) + 2e¯ –→ H2(g) b.
Calculate the K and AG for the following reaction at 25 °C: с Zn(s) + CuSO₂ (aq) = ZnSO₂(aq) + Cu (s) Note: Reference the Standard reduction potentials at 25 °℃ and Fundamental constants tables for additional information. Part 1 of 2 Round your answer to 3 significant digits. K с Part 2 of 2 = AGO = x10 Round your answer to 4 significant digits. kJ mol X Ś x10
The free energy change for the following reaction at 25 °C, when [Cr**]= 2.80×103 M and [H= 1.11 M, is 94.0 kJ: 2Cr*(2.80×10³ M) + H,(g)2Cr*(aq) + 2.00H*(1.11 M) AG = 94.0 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?
O ELECTROCHEMISTRY = Understanding concentration cells ODDOD 3/5 A certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell apparatus is filled with a 1.50 M solution of MNO3 and the right half cell with a 150. mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 30.0 °C. Which electrode will be positive? Oleft right ? What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. 0 Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.