4.(a) Use the standard reduction potentials at 25° C in Table 18.1 in Tro, Fridgen and Shaw, andcalculate the standard emf E° of an electrochemical cell described by the following reaction:2 Na Ba Ba²+ + 2 Na(b) What is n?(c) What is AG° for this reaction at 25°?(d) What is the equilibrium constant for this reaction at 25°?

Answered: 4. (a) Use the standard reduction…

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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A copper, Cu(s), electrode is immersed in a solution that is 1.00 M in ammonia, NH3, and 1.00 M in tetraamminecopper(II), [Cu(NH3)4²+. If a standard hydrogen electrode is used Use the standard reduction potentials shown here to answer the questions. as the cathode, the cell potential, Ecell is found to be 0.080 V at 298 K. Reduction half-reaction E° (V) Cu2(aq) + 2e¬Cu(s) 0.337 Part A 2H+(aq) + 20¬H2(g) 0.000 Based on the cell potential, what is the concentration of Cu2+in this solution? Express your answer to one significant figure and include the appropriate units. Templates Symbols uado redo reset keyboard shortcuts help [Cu² = Value Units
Which statement is true regarding the galvanic cell in which an electric current is being produced? Zn²* + 2e¯→Zn E° = -0.76 V Cu2* + 2e¯→Cu E° = +0.34 V V Salt Bridge Zn - Cu ZnSO«(aq) CUSO:(aq) (A) Oxidation occurs at the copper electrode. (B) The mass of the copper electrode is increasing. (C) Zinc ions are produced at the copper electrode. (D) Copper ions are produced at the copper electrode.
A galvanic cell is constructed in which the overall reac- tion is Pb(s) + 2 H;O* (aq) → Pb²+ (aq) + H2 (g) + 2 H20(e) (a) Calculate AE° for this cell. (b) Chloride ions are added until PbCl, precipitates at the anode and [CI-] reaches 0.15 M. The cell potential is then measured to be 0.22 V at pH = 0 and PH, 1.0 atm. Calculate [Pb2+] under these conditions. (c) Calculate the solubility product constant Kp of PbCl2.
Enter electrons as e". Use smallest possible integer coefficients. States are not required. If a box is not needed, leave it blank. An aqueous ScCl3 solution is electrolyzed under 1 bar pressure using platinum electrodes. (a) Write the half-reactions predicted to occur at the anode and cathode, based on the standard cell potentials given below. Standard Reduction Potentials (Volts) at 25 °C Ch(g) + 2 e → 2 Cl'(aq) 1.360 02(g) + 4 H30*(aq) + 4 e» 6 H2O() 1.229 2 H2O(1) + 2 e– H2(g) + 2 OH (aq) -0.828 Sc*(aq) + 3 e - Sc(s) -2.080 Half-reaction at anode: Half-reaction at cathode: (b) What is the expected decomposition potential? V +

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