i) Consider an electrochemical cell involving Nickel and Copper. Ni2- (aq) + 2e- - Nia E° = -0.25 V Cu2- (aq) + 2e- - Cu(s) E° = +0.34 V a) What is the standard reduction potential of anode? b) What is the standard reduction potential of cathode? c) Calculate the potential of this cell under standard conditions(E°cell). ii) How many amperes of current needs to be passed through molten Sodium chloride (NaCl) to produce 1.5 g of Sodium (Na) metal at the cathode in 35 minutes during electrolysis of molten Sodium chloride? ii) Calculate the charge in coulomb passed through the solution in part (ii). iv) Calculate the charge in Faraday passed through the solution in part (ii). Reduction Potential of Anode Reduction Potential of Cathode Cell Potential Current Charge in Coulomb Charge in Faraday

i) Consider an electrochemical cell involving Nickel and Copper. Ni2- (aq) + 2e- - Nia E° = -0.25 V Cu2- (aq) + 2e- - Cu(s) E° = +0.34 V a) What is the standard reduction potential of anode? b) What is the standard reduction potential of cathode? c) Calculate the potential of this cell under standard conditions(E°cell). ii) How many amperes of current needs to be passed through molten Sodium chloride (NaCl) to produce 1.5 g of Sodium (Na) metal at the cathode in 35 minutes during electrolysis of molten Sodium chloride? ii) Calculate the charge in coulomb passed through the solution in part (ii). iv) Calculate the charge in Faraday passed through the solution in part (ii). Reduction Potential of Anode Reduction Potential of Cathode Cell Potential Current Charge in Coulomb Charge in Faraday

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 the following standard reduction potentials: Tl+(aq)+eTl(s)Ered=0.34VTl3+(aq)+3eTl(s)Ered=0.74VTl3+(aq)+2eTl+(aq)Ered=1.28V and the following abbreviated cell notations: (1) Tl|Tl+Tl3+,Tl+|Pt (2) Tl|Tl3+Tl3+,Tl+|Pt (3) Tl|Tl+Tl3+|Tl (a) Write the overall equation for each cell. (b) Calculate E° for each cell. (c) Calculate G° for each overall equation. (d) Comment on whether G° and/or E° are state properties. (Hint: A state property is path-independent.)
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 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?
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).
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, .
In biological systems, acetate ion is converted to ethyl alcohol in a two-step process: CH3COO(aq)+3H+(aq)+2eCH3CHO(aq)+H2OE=0.581V CH3CHO(aq)+2H+(aq)+2eC2H5OH(aq)E=0.197V (E°' is the standard reduction voltage at 25°C and pH of 7.00.) (a) Calculate G°' for each step and for the overall conversion. (b) Calculate E°' for the overall conversion.
A metallurgist wants to gold-plate an object with a surface area of 17.21 in2. The gold plating must be 0.00200 in. thick (assume uniform thickness). (a) How many grams of gold (d=10.5g/cm3) are required? (b) How many minutes will it take to plate the object from a solution of AuCN using a current of 7.00 A? Assume 100% efficiency.
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.
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Consider the standard galvanic cell based on the following half-reactions: Cu2++2eCuAg++eAg The electrodes in this cell are Ag(s) and Cu(s). Does the cell potential increase. decrease. or remain the same when the following changes occur to the standard cell? a. CuSO4(s) is added to the copper half-cell compartment (assume no volume change). b. NH3(aq) is added to the copper half-cell compartment (Hint: Cu2+ reacts with NH3, to form Cu(NH3)42+(aq).] c. NaCl(s) is added to the silver half .cell compartment (Hint: Ag+ reacts with Cl to form AgCl(s).] d. Water is added to both half-cell compartments until the volume or solution is doubled. e. The silver electrode is replaced with a platinum electrode
Calculate the theoretical potential of each of the following cells.Is the cell reaction spontaneous as written or spontaneous in the opposite direction? (a) Bi|BiO+ (0.0300 M),H+ (0.100 M)||I- (0.100 M), AgI(sat’d)|Ag (b) Zn|Zn2+(5.75 10-4M)||Fe(CN)64-(530 10-2 M),Fe(CN)63-(6.75 10-2M)|Pt (c) Pt,H2O (0.200 atm)|HCI(8.25 10-4M), AgCI(sat’d)| Ag
Calculate the standard free energy change for the following reactions using the standard cell potentials for the half-reactions that are involved. (a) Fe(s)+Hg22+(aq)Fe2+(aq)+2Hg(l) (b Fe3+(aq)+Ag(s)+Cl-(aq)Fe2+(aq)+AgCl(s) (c) 2MnO4(aq)+5Zn(s)+16H3O+(aq)2Mn2+(aq)+5Zn2+(aq)+24H2O(l)