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Homework answers / question archive / Electrochemical Cells Procedure Navigate to the following simulation: https://web
Electrochemical Cells Procedure
Navigate to the following simulation: https://web.mst.edu/~gbert/Electro/Electrochem.html
Level 0
e Use the simulations link to standard reduction potentials to answer the questions
Level 1
e Select Level 1 in the lower right corner of the simulation
e Indicate the electrode construction and concentration for the given Left and Right electrodes
e Measure the cell voltage and record the voltage reading
e Using the standard reduction potentials, show your work to calculate this voltage
e Select “New Problem” and repeat these steps for two additional combinations
Level 2
e Select Level 2 in the lower right corner of the simulation
e Place the fake element electrode Wd(s)|Wd?* on the Right at a concentration of 1.00M
e Chose any electrode material for the Left Electrode, but maintain a concentration of 1.00M
e Measure the cell voltage and record the voltage reading
e Using the known standard reduction potential, and the measured voltage, determine the
theoretical standard potential of the fake element
e Select “New Problem” and repeat these steps for two additional combinations
Level 3
e Select Level 3 in the lower right corner of the simulation
e Record the requested voltage
e Manipulate both the left and right electrode material to generate the indicated voltage
e Do NOT use the fake element electrode
e Select “New Problem” and repeat these steps for two additional combinations
Level 4
e Select Level 4 in the lower right corner of the simulation
e Record the given electrode materials and concentrations
e While unlikely, if the fake element is given, please choose a New Problem
e Using the standard reduction potentials, and the Nernst Equation, calculate the overall
electrochemical potential of the cell (USE 25°C as Temp in Nernst Equation)
e Select “New Problem” and repeat these steps for two additional combinations
Electrochemical Reactions over Time
e Select Level 0 in the lower right corner of the simulation
e Choose any combination of real element electrodes each at 1.00M concentration, so that the
voltage is positive
e Record the conditions and the voltage
e Lower the concentration of the Left electrode and record the new concentration and voltage
e Return the Left Electrode to a concentration of 1.00M and lower the concentration of the Right electrode and record the new voltage
Electrochemical Cells (Electrochem_Report_(Fillable)
Name:
Navigate to the following simulation: https://web.mst.edu/~gbert/Electro/Electrochem.html
Level 0
#1). What process occurs at the Anode? (Oxidation or Reduction?)
#2). What process occurs at the Cathode? (Oxidation or Reduction?)
#3). What direction do electrons travel in the wire of an Electrochemical Cell?
(Anode to Cathode, or Cathode to Anode?)
#4). What direction do anions travel in the Salt Bridge of an Electrochemical Cell?
(Anode to Cathode, or Cathode to Anode?)
#5). On a battery, or a voltmeter (such as in the simulation), what is the Negative (Black)
terminal (Anode or Cathode)
#6). On a battery, or a voltmeter (such as in the simulation), what is the Positive (Red)
terminal (Anode or Cathode)
Select the “Standard Potentials” link in the upper left of the simulation and use the reduction potentials
listed to answer the following questions.
#7).Is the reaction Ni2+
+ 2e-
? Ni(s) an oxidation or reduction?
#8).Which half reaction of the ones listed, has a potential of -0.402V?
#9).What is the potential of the half reaction Cu(s) ? Cu2+
+ 2e-
?
#10).Is the reaction Fe(s) ? Fe2+
+ 2e-
an oxidation or reduction?
#11). What is the potential of the half reaction Mg2+
+ 2e-
? Mg(s) ?
#12).Which half reaction of the ones listed, has a potential of 0.763V?
oxidation
reduction
anode to cathode
anode to cathode
anode
positive
reduction
Cd2^+(aq)+ 2e^—> Cd(s)
-.339V oxidation
Electrochemical Cells
#13). Level 1
Problem #1
Left Electrode
Electrode Material
Electrode Solution
Solution Concentration
Measured Cell Voltage: ____________
Use the standard reduction potentials for the half reactions to calculate the voltage. Show your work.
Problem #2
Left Electrode
Electrode Material
Electrode Solution
Solution Concentration
Measured Cell Voltage: ____________
Use the standard reduction potentials for the half reactions to calculate the voltage. Show your work.
Problem #3
Left Electrode
Electrode Material
Electrode Solution
Solution Concentration
Measured Cell Voltage: ____________
Use the standard reduction potentials for the half reactions to calculate the voltage. Show your work.
Right Electrode
Electrode Material
Electrode Solution
Solution Concentration
Right Electrode
Electrode Material
Electrode Solution
Solution Concentration
Right Electrode
Electrode Material
Electrode Solution
Solution Concentration
Zinc
Zinc (II) Nitrate
.0001moles/liter
copper
copper(II) Nitrate
.0001moles/liter
[Zn (s)—> Zn^2+(aq)+2e^- anode rxn] [Cu2+(aq)+2e^-->Cu (s)] cathode rxn] Volts
from simulation=.513V -.76V+.339
Electrochemical Cells
#14). Level 2
Problem #1
Left Electrode
Electrode Material
Electrode Solution
Solution Concentration
Measured Cell Voltage: ____________
Use the standard reduction potential for the left solution, and the measured voltage to calculate the
standard reduction potential of Wd(s)|Wd2+
Show your work.
Problem #2
Left Electrode
Electrode Material
Electrode Solution
Solution Concentration
Measured Cell Voltage: ____________
Use the standard reduction potential for the left solution, and the measured voltage to calculate the
standard reduction potential of Wd(s)|Wd2+
Show your work.
Problem #3
Left Electrode
Electrode Material
Electrode Solution
Solution Concentration
Measured Cell Voltage: ____________
Use the standard reduction potential for the left solution, and the measured voltage to calculate the
standard reduction potential of Wd(s)|Wd2+ Show your work.
Right Electrode Electrode Material Whodatium
Electrode Solution Whodatium (II) Nitrate
Solution Concentration 1.00M
Right Electrode
Electrode Material Whodatium
Electrode Solution Whodatium (II) Nitrate
Solution Concentration 1.00M
Right Electrode
Electrode Material Whodatium Electrode Solution Whodatium (II) Nitrate
Solution Concentration 1.00M
Electrochemical Cells
#15). Level 3
Problem #1
What is the voltage requested in the simulation? ____________
Prepare the electrochemical cell. Do NOT use the fake element.
Left Electrode (Anode)
Electrode Material
Electrode Solution
Solution Concentration
Problem #2
What is the voltage requested in the simulation? ____________
Prepare the electrochemical cell. Do NOT use the fake element.
Left Electrode
Electrode Material
Electrode Solution
Solution Concentration
Problem #3
What is the voltage requested in the simulation? ____________
Prepare the electrochemical cell. Do NOT use the fake element.
Left Electrode
Electrode Material
Electrode Solution
Solution Concentration
Right Electrode (Cathode)
Electrode Material
Electrode Solution
Solution Concentration
Right Electrode
Electrode Material
Electrode Solution
Solution Concentration
Right Electrode
Electrode Material
Electrode Solution
Solution Concentration
Electrochemical Cells
#16). Level 4
Problem #1
Prepare the electrochemical cell. Do NOT use the fake element.
Left Electrode
Electrode Material
Electrode Solution
Solution Concentration
Use the standard reduction potentials for the half reactions to calculate and the Nernst Equation to
calculate the voltage. Show your work.
Problem #2
Prepare the electrochemical cell. Do NOT use the fake element.
Left Electrode
Electrode Material
Electrode Solution
Solution Concentration
Use the standard reduction potentials for the half reactions to calculate and the Nernst Equation to
calculate the voltage. Show your work.
Problem #3
Prepare the electrochemical cell. Do NOT use the fake element.
Left Electrode
Electrode Material
Electrode Solution
Solution Concentration
Use the standard reduction potentials for the half reactions to calculate and the Nernst Equation to
calculate the voltage. Show your work.
Right Electrode
Electrode Material
Electrode Solution
Solution Concentration
Right Electrode
Electrode Material
Electrode Solution
Solution Concentration
Right Electrode
Electrode Material
Electrode Solution
Solution Concentration
Electrochemical Cells
#17). Electrochemical Reactions over Time
Move back to Level 0 and select any combination of real element electrodes each at 1.00M
concentration, so that the voltage is positive
Left Electrode
Electrode Material
Electrode Solution
Solution Concentration
a). What is the reduction half reaction?
b). What is the oxidation half reaction?
c). What is the Cell Voltage?
d). Over time, as the reaction progresses, what will happen to the concentration of Left Electrode
Solution?
e). Over time, as the reaction progresses, what will happen to the concentration of Right Electrode
Solution?
Lower the concentration of Left Solution only
f). What is the new Left Solution Concentration?
g). What is the Cell Voltage?
Bring the concentration of Left Solution back to 1.00M and lower the concentration of Right Solution
h). What is the new Right Solution Concentration?
i). What is the Cell Voltage?
j). Over time, what will happen to the overall voltage of the cell?
Right Electrode
Electrode Material
Electrode Solution
Solution Concentration
Electrochemical Cells
#18). Car Batteries
The lecture example gives the chemistry of a standard alkali battery, but Car Batteries have a different chemistry and are Lead-Acid batteries. In a Lead-Acid battery, solid Lead is oxidized to Pb2+ and Lead (IV)
Oxide is reduced to Pb2+
. For this battery, indicate which fully balanced half reaction occurs at the
Anode, which fully balanced half reaction occurs at the cathode, the full balanced electrochemical reaction, and show your work for determining the Electrochemical Potential of this reaction.
a). Anode Reaction:
b). Cathode Reaction:
c). Full Balanced Reaction:
d). Show your work to determine the theoretical voltage
