E The saturated calomel electrode, abbreviated SCE, is often used as a reference electrode in making electrochemical measurements. The SCE is composed of mercury in contact with a saturated solution of calomel (Hg₂Cl₂). The electrolyte solution is saturated KCI. SCE is +0.242 V relative to the standard hydrogen electrode. Calculate the potential for each of the following galvanic cells containing a saturated calomel electrode and the given half-cell components at standard conditions. In each case, indicate whether the SCE is the cathode or the anode. Standard reduction potentials are found in the Standard Reduction Potentials table. (a) AuCl + 3 e → Au + 4 CI ४० 1.278 X V SCE role: O cathode O anode

E The saturated calomel electrode, abbreviated SCE, is often used as a reference electrode in making electrochemical measurements. The SCE is composed of mercury in contact with a saturated solution of calomel (Hg₂Cl₂). The electrolyte solution is saturated KCI. SCE is +0.242 V relative to the standard hydrogen electrode. Calculate the potential for each of the following galvanic cells containing a saturated calomel electrode and the given half-cell components at standard conditions. In each case, indicate whether the SCE is the cathode or the anode. Standard reduction potentials are found in the Standard Reduction Potentials table. (a) AuCl + 3 e → Au + 4 CI ४० 1.278 X V SCE role: O cathode O anode

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

A student constructs an electrochemical cell with a half-cell composed of a nickel anode in a 0.10 M Ni2+(aq) solution, and another composed of a silver cathode in a 0.10 M Ag+(aq) solution. The Ecell at 20.0oC is measured as +1.03 V. experimental standard cell potential, Eocell, for the reaction=1.06 experimental standard state free energy change, ΔGo, for the reaction =2.69e35 Calculate the experimental equilibrium constant, K, for the reaction Your answer should have 3 sig figs
Write the cell notation for an electrochemical cell consisting of an anode where H, (g) is oxidized to Ht (aq) at a platinum electrode and a cathode where Ag* (aq) is reduced to Ag (s) . Assume all aqueous solutions have a concentration of 1 mol/L and gases have a pressure of 1 bar.
What is the Eθ cell value for a galvanic cell constructed using aluminium and nickel electrodes.
A student constructs an electrochemical cell with a half-cell composed of a nickel anode in a 0.10 M Ni2+(aq) solution, and another composed of a silver cathode in a 0.10 M Ag+(aq) solution. The Ecell at 20oC (293K) is measured as +1.03 V. Calculate the experimental standard cell potential, Eocell, for the reaction
Calculate the cell potential for the galvanic cell (in volts) in which the following reaction occurs at 25.0∘C, given than [Ti2+] = 2.773 M and [Au3+] = 0.582 M. Use Standard reduction potentials
Two half-reactions are shown with their standard cell potentials. If a galvanic cell is constructed using them, which electrode would be the anode, and what would the cell potential be? Cd2* (aq) + 2e – Cd(s); E=-0.40 V Cr3+ (aq) + 3e → Cr(s); E=-0.74 V Oa. Cadmium, -0.34 V Ob. None of the other options Oc. Cadmium, -1.14 V Od. Chromium, -1.14 V Oe. Chromium, 0.34 V
Calculate the AG° (in kJ) for the reaction of elemental chlorine with the bromide ion at 298K. Refer to | the standard cell potentials on the last page of the note packet. Selected Answer: -54 A Calculate the AG° (in kJ) for the reaction of elemental chlorine with the bromide ion at 298K. Refer to the standard X cell potentials on the last page of the note packet. Selected Answer: 27.0
A standard hydrogen electrode has a half-cell reduction potential of zero at 25 C. Calculate the potential of the half-cell when the pH is 3.8 and the pressure of H2 is 4.6 bar.
The saturated calomel electrode, abbreviated SCE, is often used as a reference electrode in making electrochemical measurements. The SCE is composed of mercury in contact with a saturated solution of calomel (Hg₂Cl₂). The electrolyte solution is saturated KCI. SCE is +0.242 V relative to the standard hydrogen electrode. Calculate the potential for each of the following galvanic cells containing a saturated calomel electrode and the given half-cell components at standard conditions. In each case, indicate whether the SCE is the cathode or the anode. Standard reduction potentials are found in the Standard Reduction Potentials table. (a) AgCl + e → Ag + CI V SCE role: O cathode anode (b) Zn2+ + 2e → Zn SCE role: O cathode Oanode (c) Fe³+ + e→→ Fe²+ 8⁰ SCE role: O cathode O anode V V
A galvanic cell was constructed with a nickel electrode that was dipped into 1.1 M NiSO4 solution and a chromium electrode that was immersed into a solution containing Cr3+ at an unknown concentration. The potential of the cell was measured to be 0.557 V, with the chromium serving as the anode. The standard cell potential for this system was determined to be 0.487 V. What was the concentration of Cr3+ in the solution of unknown concentration?
Please don't provide handwritten solution...
Calculate the cell potential for the galvanic cell (in volts) in which the following reaction occurs at 25.0∘C, given than [Ti2+] = 0.602 M and [Au3+] = 0.276 M. use standard reduction potentials