I need the answers for 1 and 2 2. Electrochemical cell #1: Select the followingRed Wire-Metal: SilverSolution: 1.0 M AGNO3(aq)Black Wire-Metal: CopperSolution: 1.0 M Cu(NO3)2(aq):Label the diagram below showing the followingelectrochemical cell that you built andobserved:• label electrode with the metals;show direction of electron flow;show electrode polarity;• record standard potential for the cell; andlabel the bridge and show direction of ionmovement in the bridge.Electrochemical Cell #1externalcircuitvoltmeterelectrodeelectrodeKNO3internalcircuitNONO33. Electrochemical cell #2: Select the followingRed Wire-Metal: SilverSolution: 1.0 M AGNO3(aq)Black Wire-Metal: ZincSolution: 1.0 M Zn(NO3)2(aq):Label the diagram below showing the followingelectrochemical cell that you built andobserved:label electrode with the metals;• show direction of electron flow;show electrode polarity;record standard potential for the cell; andlabel the bridge and show direction of ionmovement in the bridge.Electrochemical Cell #2externalcircuitvoltmeterelectrodeelectrodeKNO3internalcircuitNONO Data Analysis and Discussion1. For each electrochemical cell, show the half-cell reactions and using the "StandardReduction Potentials For Half-Reactionscalculate the standard potential for the cell andcompare it to the recorded potential from thesimulation.2. Which cell combination is a morespontaneous reaction? Explain.

The electrochemical cell can be denoted with the help of their Standard reduction potential(SRP).…

Data Analysis and Discussion 1. For each electrochemical cell, show the half- cell reactions and using the "Standard Reduction Potentials For Half-Reactions calculate the standard potential for the cell and compare it to the recorded potential from the simulation. 2. Which cell combination is a more spontaneous reaction? Explain.

Data Analysis and Discussion 1. For each electrochemical cell, show the half- cell reactions and using the "Standard Reduction Potentials For Half-Reactions calculate the standard potential for the cell and compare it to the recorded potential from the simulation. 2. Which cell combination is a more spontaneous reaction? Explain.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 77AP

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Consider the following galvanic cell: A 15 0-mole sample of NH is added to the Ag compartment (assume 1.00 L of total solution after the addition). The silver ion reacts with ammonia to form complex ions as shown: Ag+(aq)+NH3(aq)AgNH3+(aq)K1=2.1103AgNH3+(aq)+NH3(aq)Ag(NH3)2+(aq)K2=8.2103 Calculate the cell potential after the addition of 15.0 moles of NH3.
A galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.
Assume the following electrochemical cell simulates the galvanic cell formed by copper and zinc in seawater at pH 7.90 and 25 C. Zn | Zn(OH)2(s) | OH(aq) || Cu(OH)2(s) | Cu(s) a. Write a balanced equation for the reaction that occurs at the cathode. b. Write a balanced equation for the reaction that occurs at the anode. c. Write a balanced chemical equation for the overall reaction. d. Determine the potential (in volts) of the cell.
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.
A voltaic cell is constructed in which one half-cell consists of a silver wire in an aqueous solution of AgNO3.The other half cell consists of an inert platinum wire in an aqueous solution containing Fe2+(aq) and Fe3+(aq). (a) Calculate the cell potential, assuming standard conditions. (b) Write the net ionic equation for the reaction occurring in the cell. (c) Which electrode is the anode and which is the cathode? (d) If [Ag+] is 0.10 M, and [Fe2+] and [Fe3+] are both 1.0 M, what is the cell potential? Is the net cell reaction still that used in part (a)? If not, what is the net reaction under the new conditions?
An electrochemical cell consists of a silver metal electrode immersed in a solution with [Ag+] = 1.0 M separated by a porous disk from a copper metal electrode. If the copper electrode is placed in a solution of 5.0 M NH3 that is also 0.010 M in Cu(NH3)42+, what is the cell potential at 25C? Cu2+(aq)+4NH3(aq)Cu(NH3)42+(aq)K=1.01013
An alloy made up of tin and copper is prepared by simultaneously electroplating the two metals from a solution containing Sn(NO3)2 and Cu(NO3)2.If 20.0% of the total current is used to plate tin, while 80.0% is used to plate copper, what is the percent composition of the alloy?
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
Calculate the cell potential of a cell operating with the following reaction at 25C, in which [Cr2O32] = 0.020 M, [I] = 0.015 M, [Cr3+] = 0.40 M, and [H+] = 0.60 M. Cr2O72(aq)+6I(aq)+14H+(aq)2Cr3+(aq)+3I2(s)+7H2O(l)