A cell constructed in which one half-cell consists of a Zn wire dipped in a solution of Zn(NO3)2. The other half-cell is composed of an inert electrode in a solution containing a mixture of Fe and Fe* ions. What will the cell potential, Ecell, be if the soluble ions have the following concentrations at 25°C? [Zn**] = 0.49M; [Fe"] = 0.16 M; [Fe*] = 0.41 M Draw the complete galvanic cell set-up for this. Label each component. %3D

A cell constructed in which one half-cell consists of a Zn wire dipped in a solution of Zn(NO3)2. The other half-cell is composed of an inert electrode in a solution containing a mixture of Fe and Fe* ions. What will the cell potential, Ecell, be if the soluble ions have the following concentrations at 25°C? [Zn**] = 0.49M; [Fe"] = 0.16 M; [Fe*] = 0.41 M Draw the complete galvanic cell set-up for this. Label each component. %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...

See similar textbooks

Similar questions

Use the standard half cell potentials listed below to calculate the standard cell potential for the following reaction that occurs in an electochemical cell at 25 ° C.
A galvanic cell using Mg / Mg*" and Cu / Cu" half-cells operates under standard-state conditions at 25 °C, and each compartment has a volume of 227 mL. The cell delivers 0.31 A for 32.1 h. (a) How many grams of Cu are deposited? g Cu
Consider the same diagram of a galvanic cell as in previous question, where the half-cells are Ag|AgNO3(aq) and Ni|Ni(NO3)2(aq), and the electrode potentials are as follows: Ag+(aq) + e– --> Ag(s); Eo = 0.80 V Ni2+(aq) + 2e– --> Ni(s); Eo = – 0.23 V What is the Ecell at 25oC when the electrolyte concentrations are: [Ag+] = 1.3 x 10–5 M and [Ni2+] = 0.10 M. (A) 1.15 V (B) 1.30 V (C) 0.76 V (D) 0.91 V
what is the standard cell potential (in Volts) for a a galvanic cell that can do 567 kJ of work. The number of electrons tranferred in the rxn is 4.
For each cell at standard condtions calculate the cell potential, the free energy change and the equilibrium constant of the following reaction.
. Calculate the standard cell potential for the spontaneous redox reaction between Pb(s)/Pb(NO2)2(aq) half-cell and a Ag(s)/A£NO3(aq) half-cell. Which metal would be oxidized? a Which metal would be reduced?
Consider the following electrochemical cell notation with a cell potential of 0.300 V. Pt ∣Cr3+(aq, 0.015M) ∣ Cr2+(aq, 0.045M) ∣∣ H+(aq,?M) ∣ H2(g,1.0 atm) ∣ PtWrite the two half reactions (show the overall reaction) andCalculate the standard cell potential and determine if this cell is more or less spontaneous at the nonstandard conditions?
Calculate the non-standard cell potential (in V) for the following reaction at 160.73 ℃ with the following concentrations: [Mg^+2] = 1.00×10^−7 M; [Cu^+2] = 1.488 M Cu^+2(aq) + Mg(s) --> Cu(s) + Mg^+2(aq)
A galvanic (voltaic) cell consists of an inert platinum clectrode in a solution containing 1.0 M tin(IV) ion and 1.0M tin(II) ion, and another inert platinum clectrode in a solution containing 1.0 M iron(III) ion and 1.0M iron(II) ion, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Standard reduction potentials can be found in the standard reduction potentials table. E: cell V
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.
I have solved this equation and seen solutions to it. However, I keep seeing Pb2+ squared in the Nernst Equation (for Q) for the calcuation of the second part of this question. I do not understand why Pb2+ is squared. Can you explain that to me? Thank you.
Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Mg(s) ∣ Mg2+(aq, 1.74 M) || Cu2+(aq, 0.0053 M) ∣ Cu(s)