Consider a ring which was electroplated with gold (Au, MM = 197 g/mol) using an Au(III) salt with a0.328-Ampere current for 4.00 min.R= 8.314 J/mol-K; F = 96,485 J/mol-V1. How much electric charge passed through the cell? [Select]VII. How many moles of electrons passed through the cell? [Select]III. How much gold were deposited onto the ring? [Select]VV Consider a voltaic cell at 25°C consisting of a Fe(s) electrode immersed in a 1.0 M Fe(NO3)3 solutionand a Pb(s) electrode immersed in a 1.0 M Pb(NO3)2 solution, linked by a KCI bridge. Refer to thehalf-reactions and standard potentials below:Pb2+ + 2e → Pb-0.13 VFe³+ + 3e → Fe-0.04 V1. Which is the reduction half reaction and potential? [Select]A. Fe3+ + 3e → Fe-0.04 VB. Fe Fe³+ + 3e+0.04 VC. Pb2+ + 2e →→ Pb-0.13 VD. Pb→ Pb2+ + 2e+0.13 VII. Which is the oxidation half reaction and potential? [Select]A. Fe3+ + 3e → Fe-0.04 VB. Fe Fe3+ + 3e¯+0.04 VC. Pb2+ + 2e →→ Pb-0.13 VD. Pb→ Pb2+ + 2e+0.13 VIII. Which is the net cell reaction and potential? [Select]A. 3Fe + 2Pb²+ →3Fe³+ + 2Pb-0.09 V-0.09 VB. 2Fe +3Pb2+→2Fe³+ + 3PbC. 3Fe3+ + 2Pb →3Fe + 2Pb²++0.09 VD. 2Fe³+ + 3Pb →→2Fe +3Pb2++0.09 VIV. What is the cell notation? [Select]A. Pb2+ (aq)|Pb(s)||Fe(s)| Fe³+ (aq)B. Pb(s) Pb2+ (aq)||Fe3+ (aq)| Fe(s)C. Fel Fe3+llPb2+Ph

The electric charge carried by the electrolysis is determined by the amount of current flow and…

Consider a ring which was electroplated with gold (Au, MM = 197 g/mol) using an Au(III) salt with a 0.328-Ampere current for 4.00 min. R= 8.314 J/mol-K; F = 96,485 J/mol-V 1. How much electric charge passed through the cell? [Select] V II. How many moles of electrons passed through the cell? [Select] III. How much gold were deposited onto the ring? [Select] V

Consider a ring which was electroplated with gold (Au, MM = 197 g/mol) using an Au(III) salt with a 0.328-Ampere current for 4.00 min. R= 8.314 J/mol-K; F = 96,485 J/mol-V 1. How much electric charge passed through the cell? [Select] V II. How many moles of electrons passed through the cell? [Select] III. How much gold were deposited onto the ring? [Select] V

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 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?
You have 1.0 M solutions of Al(NO3)3 and AgNO3 along with Al and Ag electrodes to construct a voltaic cell. The salt bridge contains a saturated solution of KCl. Complete the picture associated with this problem by a writing the symbols of the elements and ions in the appropriate areas (both solutions and electrodes). b identifying the anode and cathode. c indicating the direction of electron flow through the external circuit. d indicating the cell potential (assume standard conditions, with no current flowing). e writing the appropriate half-reaction under each of the containers. f indicating the direction of ion flow in the salt bridge. g identifying the species undergoing oxidation and reduction. h writing the balanced overall reaction for the cell.
At 298 K, the solubility product constant for PbC2O4 is 8.5 1010, and the standard reduction potential of the Pb2+(aq) to Pb(s) is 0.126 V. (a) Find the standard potential of the half-reaction PbC2O4(s)+2ePb(s)+C2O42(aq) (Hint: The desired half-reaction is the sum of the equations for the solubility product and the reduction of Pb2+. Find G for these two reactions and add them to find G for their sum. Convert the G to the potential of the desired half-reaction.) (b) Calculate the potential of the Pb/PbC2O4 electrode in a 0.025 M solution of Na2C2O4.
An electrolysis experiment is performed to determine the value of the Faraday constant (number of coulombs per mole of electrons). In this experiment, 28.8 g of gold is plated out from a AuCN solution by running an electrolytic cell for two hours with a current of 2.00 A. What is the experimental value obtained for the Faraday Constant?
The half cells Sn2+(aq) |Sn(s) and Cl2(g) |Cl(aq) are linked to create a voltaic cell. (a) Write equations for the oxidation and reduction half-reactions and for the overall (cell) reaction. (b) Which half-reaction occurs in the anode compartment, and which occurs in the cathode compartment? (c) Complete the following sentences: Electrons in the external circuit flow from the ______ electrode to the ____ electrode. Negative ions move in the salt bridge from the _____ half-cell to the _____ half-cell.
Consider a voltaic cell with the reaction H2(g) + Sn4+(aq) 2 H+(aq) + Sn2+(aq) operating at 298 K. (a) Calculate the Ecell for this cell. (b) Calculate the Ecell for PH2 = 1.0 bar, (cone. Sn2+) = 6.0 104M, (cone. Sn4+) = 5.0 104M, and pH = 3.60.
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)
A half-cell that consists of a copper wire in a 1.00 M Cu(NO3)2 solution is connected by a salt bridge to a solution that is 1.00 M in both Pu3+ and Pu4+, and contains an inert metal electrode. The voltage of the cell is 0.642 V, with the copper as the negative electrode. (a) Write the half-reactions and the overall equation for the spontaneous chemical reaction. (b) Use the standard potential of the copper half-reaction, with the voltage of the cell, to calculate the standard reduction potential for the plutonium half-reaction.
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+).
It took 150. s for a current of 1.25 A to plate out 0.109 g of a metal from a solution containing its cations. Show that it is not possible for the cations to have a charge of 1+.