Show your work please, thank you! 9. For the following galvanic cellI (expressed in cell notation), how will the voltage, E, change if Fe(NO3)2was added to the cathode compartment? Assume that the cell was at equilibrium prior to the addition.X(s)|X*(aq)||Fe²2+(aq)|Fe(s)a. E > E°b. E = E°с.E < E°d. Need more information

Given cell : X | X+ || Fe 2+ | Fe Reaction at cathode: Fe 2+ + 2e --> FeReaction at anode: X…

For the following galvanic cell (expressed in cell notation), how will the voltage, E, change if Fe(N03)2 was added to the cathode compartment? Assume that the cell was at equilibrium prior to the addition. X(s)|X*(aq)||Fe²2+(aq)|Fe(s) a. E> E° b. E = E° C. E < E° d. Need more information

For the following galvanic cell (expressed in cell notation), how will the voltage, E, change if Fe(N03)2 was added to the cathode compartment? Assume that the cell was at equilibrium prior to the addition. X(s)|X*(aq)||Fe²2+(aq)|Fe(s) a. E> E° b. E = E° C. E < E° d. Need more information

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter18: Introduction To Electrochemistry

Section: Chapter Questions

Problem 18.18QAP

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Question

Show your work please, thank you!

9. For the following galvanic cellI (expressed in cell notation), how will the voltage, E, change if Fe(NO3)2
was added to the cathode compartment? Assume that the cell was at equilibrium prior to the addition.
X(s)|X*(aq)||Fe²2+(aq)|Fe(s)
a. E > E°
b. E = E°
с.
E < E°
d. Need more information

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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?
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.
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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.
Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
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At 298 K, the solubility product constant for Pb(IO3)2 is 2.6 1013, 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 Pb(IO3)2(s)+2ePb(s)+2IO3(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/Pb(IO3)2 electrode in a 3.5 103 M solution of NaIO3.
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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)?
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