Non Standard Electrochemical Cell1. Calculate the emf generated, Gibbs Free-Energy and thestandard Gibbs Free-Energy by the cell in the given notation:Zn, IZn ) || H og)| Hae) Pt)When [Zn ] = 4.0 x 10 M, [H] = 0.010 M, [H] = 1.0 M2. Calculate the emf, E at 298.15K for the given reaction:Cr,0,7H,O(aq)(aq)l+61-- 2Cr * () + 3122-+ 14 H*(aq)(aq)[Cr,0, 2-]= 2.0 M; [H'] = 1.0 M; [I-']= 1.0 M;[Cr *] = 1.0x10 - M and [H,O] = 1.0 x 10 -$ MCalculate the free-energy occurring in the system.When3. If the voltage of Zn-H" cell is 0.542 V at 25 ° C, What is theconcentration of the H'?when : [Zn 2] = 0.01 M and [H,] = 1.0 M4. A galvanic cell consists of a chromium, Cr bar in a chromicsulfate solution, Cr,(SO.), containing 0.25 moles and a silver,Ag bar in a silver sulfate solution (Ag,So, ) containing 0.35moles in a 3 L solution. and a sodium sulfate solution use as asalt bridge solution. The silver electrode is positive relative tothe chromium electrode. Write the cell half- reactions, overallreaction and cell notation. Calculate the following:A) Gibbs Free - EnergyB) Standard Gibbs Free – EnergyC) Electrode potential of the cell.5. Calculate the emf generated by the cell in the given notation:AlI Al e II I 2) II-When [Al*] = 4.0 x 10 * M and [I-]=0.010 M(aq)!!

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1. Calculate the emf generated, Gibbs Free-Energy and the standard Gibbs Free-Energy by the cell in the given notation: Zno IZn m) || H o) Hy) |Pto) When [Zn"] = 4.0 x 10 M, [H] = 0.010 M, [H'] = 1.0 M (ag) %3D

1. Calculate the emf generated, Gibbs Free-Energy and the standard Gibbs Free-Energy by the cell in the given notation: Zno IZn m) || H o) Hy) |Pto) When [Zn"] = 4.0 x 10 M, [H] = 0.010 M, [H'] = 1.0 M (ag) %3D

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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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?
A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AG". • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions E. His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 1. calculated quantities (Check the box next to any that are wrong.) cell n 46° K 1 - 124. kJ/mol 5.30 x 10 21 -1.28 V -18 4.53 x 10 B 1 - 99. kJ/mol -1.03 V -7 2.20 x 10 1 - 38. kJ/mol 0.39 V
What is the equilibrium constant K at 25 °C for an electrochemical cell when E° = +0.0235 V and n = 2?(F = 96,500 J/(V･mol), R = 8.314 J/(mol･K))
A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AGº. • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions E". His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 1. calculated quantities (Check the box next to any that are wrong.) cell n aG K E -21 1.42 x 10 A 1 119. kJ/mol O 1.23 V -- В - 51. kJ/mol 1.16 X 10 -0.53 V -11 2.06 X 10 1 -61. kJ/mol 0.63 V
A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AG⁰. • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions º His results are listed below. any. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 1. cell n A B C 1 calculated quantities (Check the box next to any that are wrong.) AGⓇ 37. kJ/mol - 66. kJ/mol -47. kJ/mol K 6 3.03 × 10 2.74 × 10 5.83 × 10 12 9 X 0 E -0.38 V 0.68 V -0.49 V S