[References]A constant current of 2.20 amp is passed through an electrolytic cell containing a 0.100 M solution of AgNO, and a silver anode and a platinum cathode until 2.48 g of silver isdeposited.a. How long does the current flow to obtain this deposit?Sb. What mass of chromium would be deposited in a similar cell containing 0.100 M Cr+ if the same amount of current were used? [References]An electrochemical cell is made by placing an iron electrode in 1.00 L of 0.29 MFESO4 solution and a copper electrode in 1.00 L of6.80 x 10-2 MCUSO4 solution.Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°CCathode (Reduction)StandardHalf-ReactionPotential, E° (V)Fe?+ (aq) + 2e Fe(s)-0.41Cu?+(ag) + 2e = Cu(s)0.34a. What is the initial voltage of this cell when it is properly constructed?Initial voltageVb. Calculate the final concentration of Cu?+ in this cell if it is allowed to produce an average current of 1.22 amp for 289 s.Final concentration of Cu2+M

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A constant current of 2.20 amp is passed through an electrolytic cell containing a 0.100 M solution of AgN0, and a silver anode and a platinum cathode until 2.48 g of silver is deposited. a. How long does the current flow to obtain this deposit? b. What mass of chromium would be deposited in a similar cell containing 0.100 M Cr+ if the same amount of current were used? g

A constant current of 2.20 amp is passed through an electrolytic cell containing a 0.100 M solution of AgN0, and a silver anode and a platinum cathode until 2.48 g of silver is deposited. a. How long does the current flow to obtain this deposit? b. What mass of chromium would be deposited in a similar cell containing 0.100 M Cr+ if the same amount of current were used? g

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

[References]
A constant current of 2.20 amp is passed through an electrolytic cell containing a 0.100 M solution of AgNO, and a silver anode and a platinum cathode until 2.48 g of silver is
deposited.
a. How long does the current flow to obtain this deposit?
S
b. What mass of chromium would be deposited in a similar cell containing 0.100 M Cr+ if the same amount of current were used?

[References]
An electrochemical cell is made by placing an iron electrode in 1.00 L of 0.29 M
FESO4 solution and a copper electrode in 1.00 L of
6.80 x 10-2 M
CUSO4 solution.
Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C
Cathode (Reduction)
Standard
Half-Reaction
Potential, E° (V)
Fe?+ (aq) + 2e Fe(s)
-0.41
Cu?+
(ag) + 2e = Cu(s)
0.34
a. What is the initial voltage of this cell when it is properly constructed?
Initial voltage
V
b. Calculate the final concentration of Cu?+ in this cell if it is allowed to produce an average current of 1.22 amp for 289 s.
Final concentration of Cu2+
M

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