Enter electrons as e".A voltaic cell is constructed in which the anode is a Ag Ag" half cell and the cathode is a Hg Hg* half cell. The half-cell compartments are connected by a salt bridge.(Use the lowest possible coeficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.)The anode reaction is:The cathode reaction is:The net cell reaction is:In the external circuit, electrons migratelthe AgAg" electrodev the Hg Hg* electrode.In the salt bridge, anions migrate|v the Hg|Hg" compartment|v the AgAg" compartment.+

Given : Anodic half cell reaction: Ag ---> Ag+ +e- Cathodic half cell reaction: Hg2+ + 2e-…

A voltaic cell is constructed in which the anode is a Ag Ag" half cell and the cathode is a Hg Hg" half cell. The half-cell compartments are connected by a salt i Use the lowest possible coefficients. Be sure to specify states such as (ag) or (3). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction is: The net cell reaction is:

A voltaic cell is constructed in which the anode is a Ag Ag" half cell and the cathode is a Hg Hg" half cell. The half-cell compartments are connected by a salt i Use the lowest possible coefficients. Be sure to specify states such as (ag) or (3). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction is: The net cell reaction is:

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 135CWP: Consider a galvanic cell based on the following half-reactions: a. What is the expected cell...

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Consider a voltaic cell in which the following reaction occurs. Zn(s)+Sn2+(aq)Zn2+(aq)+Sn(s) (a) Calculate E° for the cell. (b) When the cell operates, what happens to the concentration of Zn2+? The concentration of Sn2+? (c) When the cell voltage drops to zero, what is the ratio of the concentration of Zn2+ to that of Sn2+? (d) If the concentration of both cations is 1.0 M originally, what are the concentrations when the voltage drops to zero?
Consider a voltaic cell in which the following reaction takes place in basic medium at 25°C. 2NO3-(aq)+3S2(aq)+4H2O3S(s)+2NO(g)+8OH(aq) (a) Calculate E°. (b) Write the Nernst equation for the cell E. (c) Calculate E under the following conditions: PNO=0.994atm,ph=13.7,[S2]=0.154M,[NO3-]=0.472M, .
Consider a salt bridge cell in which the anode is a manganese rod immersed in an aqueous solution of manganese(II) sulfate. The cathode is a chromium strip immersed in an aqueous solution of chromium(III) sulfate. Sketch a diagram of the cell, indicating the flow of the current throughout. Write the half-equations for the electrode reactions, the overall equation, and the abbreviated notation for the cell.
Consider a galvanic cell based on the following half-reactions: a. What is the expected cell potential with all components in their standard states? b. What is the oxidizing agent in the overall cell reaction? c. What substances make up the anode compartment? d. In the standard cell, in which direction do the electrons flow? e. How many electrons are transferred per unit of cell reaction? f. If this cell is set up at 25C with [Fe2+] = 2.00 104 M and [La3+] = 3.00 103 M, what is the expected cell potential?
The half-cells Ag+(aq. 1.0 M)|Ag(s) and H+(aq, ? M)|H2(1.0 bar) are linked by a salt bridge to create a voltaic cell. With the silver electrode as the cathode, a value of 0.902 V is recorded tor kcell at 298 K. Determine the concentration of H+ and the pH of the solution.
Determine the standard cell potential and the cell potential under the stated conditions for the electrochemical reactions described here. State whether each is spontaneous or nonspontaueous under each set of conditions at 293.15 K. (a) Hg(l)+S2(aq,0.10M)+2Ag+(aq,0.25M)2Ag(s)+HgS(s) (b) The galvanic cell made from a half-cell consisting of an aluminum electrode in 0.015 M aluminum nitrate solution and a half—cell consisting of a nickel electrode in 025 M nickel(l) nitrate solution. (c) The cell made of a half-cell in which 1.0 M aqueous bromide is oxidized to 0.11 M bromine ion and a half-cell in which aluminum ion at 0.023 M is reduced to aluminum metal. Assume the standard reduction potential for Br2(l) is the same as that of Br2(aq).
For each reaction listed, determine its standard cell potential at 25 C and whether the reaction is spontaneous at standard conditions. (a) Mn(s)+Ni2+(aq)Mn2+(aq)+Ni(s) (b) 3Cu2+(aq)+2Al(s)2Al3+(aq)+3Cu(s) (c) Na(s)+LiNO3(aq)NaNO3(aq)+Li(s) (d) Ca(NO3)2(aq)+Ba(s)Ba(NO3)2(aq)+Ca(s)
Is it reasonable to conclude that a potential could be assigned to each half-cell in a voltaic cell, based on these data for three voltaic cells? Explain. Zn(s)|Zn2+(aq)||Cu2+(aq)|Cu(s) cell potential=1.10 V Zn(s)|Zn2+(aq)||Ag+(aq)|Ag(s) cell potential=1.56 V Cu(s)|Cu2+(aq)||Ag+(aq)|Ag(s) cell potential=0.46 V
Consider the voltaic cell 2 Ag+(aq) + Cd(s) 2 Ag(s) + Cd2+(aq) operating at 298 K. (a) Calculate the Ecell for this cell. (b) If (cone. Cd2+) = 2.0 M and (cone. Ag+) = 0.25 M, calculate Ecell. (c) If Ecell = 1.25 V and (cone. Cd2+) = 0.100 M, calculate(cone. Ag+).
Sketch a galvanic cell, and explain how it works. Look at Figs. 17-1 and 17-2. Explain what is occurring in each container and why the cell in Fig. 17-2 works but the one in Fig. 17-1 does not.