13. The cell SCE||Ag,CrO4(sat’d), CrO,²(x M)|Ag is used to determine the concentration of the chromate ion. Given that E°sCE (=E°left) = 0.244 V and that for Ag2CrO4(s) + 2 e-→ 2Ag(s) + CrO,²-(aq), E° (=E°right) = 0.446 V, calculate the concentration of CrO,²- when the cell potential is +0.366 V.

13. The cell SCE||Ag,CrO4(sat’d), CrO,²(x M)|Ag is used to determine the concentration of the chromate ion. Given that E°sCE (=E°left) = 0.244 V and that for Ag2CrO4(s) + 2 e-→ 2Ag(s) + CrO,²-(aq), E° (=E°right) = 0.446 V, calculate the concentration of CrO,²- when the cell potential is +0.366 V.

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 wishes to determine the chloride ion concentration in a water sample at 25 °C using a galvanic cell constructed with a graphite electrode and a half-cell of AgCl(s) + e → Ag(s) + Cl(aq) Eºred = 0.2223 V And a copper electrode with 0.500 M Cu²+ as the second half cell Cu²+ (aq) + 2 e → Cu(s) Eºred= 0.337 V The measured cell potential when the water sample was placed into the silver side of the cell was 0.0595 V. Write the balanced equation for the overall reaction in acidic solution.
For the following electrolyte-concentration cell consisting of two cells back to back by electrodes, What is the suitable Nernst Equation at 25 0C? Pt;H2,HCl(a1),AgCl(s),Ag,| Ag, AgCl(s),HCl(a2),H2;Pt
Consider the cell: Pt(s) | Sn2+, Sn4+ || Fe2+ | Fe(s). Starting with 1 M each of Sn²+, Sn4+ and Fe2+ Which of the following is correct when equilibrium is established? Eºred of Pt | Sn2+,Sn4+ = 0.15 V and εºred of Fe | Fe²+ = -0.45 V [Sn²+] > 1 M; [Fe²+] >> 1 M O [Sn²+] > 1 M; [Fe²+] > 1 M; [Sn4+] > 1 M; [Sn4+] > 1 M 00
In a certain zinc-copper cell, Zn(s) + Cu2*(aq) – Zn²*(aq) + Cu(s) the ion concentrations are [Cu2*] = 0.0346 M and [Zn2*] = 1.7 M. What is the cell potential at 25 °C? Ecell = i
Prepare a sketch and write the half-reactions and overall cell reaction for the electrochemical cell designated by: Pt(s) | Ag(s) |AgCl(s) | Cl-(a = 1) | Cl2(g, 1 bar)| C(graphite) | Pt(s)
9) At 25°C, what is the potential and the cell reaction for the following cell: Ni | Ni2+ (aq, 0010 M) || Cl(aq, 0.20M) | Cl2 (g, 1 atm) | Pt? What is the Keg at 298K?
A cell at 25oC is described by the following cell notationZn(s) | Zn2+(aq) || Zn2+(aq) | Zn(s)The concentration of zinc ions at the cathode is 0.50M while the concentration of zinc ions at the anode is 0.10M. Based on the given cell notation and concentrations, (show proper units and box final answers)A) Calculate the standard free energy change.B) Calculate the cell potential.C) If the given concentrations of zinc ions for anode and cathode are reversed, will the reaction proceed forward or backward?
In a certain zinc–copper cell, Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s) the ion concentrations are [Cu2+] = 0.0218 M and [Zn2+] = 1.3 M.What is the cell potential at 25 °C?
Calculate the cell potential of each of the following electrochemical cell at 25oC. a. Pt|H 2 (8.00 atm)|H + (1.00 x 10 -3 M)‖Ag + (0.00549 M)|Agb. Pt|H 2 (1.00 atm)| H + (pH = 5.97 ) ‖ H + (pH=3.47)|H 2 (1.00 atm)|Ptc. Pt|H 2 (0.0361 atm)|H + (0.0175 M)‖H + (0.0175 M)|H 2 (5.98 x 10 -4 atm)|Pt Please solve and give explanations steps.
Determine the cell potential for the following cell Zn(s) | Zn2+(aq), 0.500 M || Ag+(aq), 0.010 M | Ag(s) The standard reduction potentials of Zn2+(aq) and Ag+(aq) are –0.76 V and +0.80 V, respectively. A. 1.45 V B. 1.67 V C. 1.56 V D. 1.51 V E. 1.61 V
In a certain zinc-copper cell, Zn(s) + Cu2+(aq) → Zn2*(aq) + Cu(s) the ion concentrations are [Cu2+] = 0.0336 M and [Zn2+] = 1.8 M. What is the cell potential at 25 °C? Ecell = i V
(c) Consider the following cell: Ag(s)|AgCl(s)|Cl(aq, aci-= 0.00500) || Cd²+ (aq, aca²+ = 0.100)| Cd(s)