Use the Nernst equation to calculate the concentration of the unknown solution. Base this on your...
Use the Nernst equation to calculate the concentration of the unknown solution. Base this on your experimental voltage of 0.4410 V for the galvanic cell with silver combined with your copper half-cell.
Use the unrounded [Cu2+] value of 0.04969 M and the unrounded value of the constants.
E(cell) = 0.462 V
| Ag+ + e- → Ag(s) | E(knot)= 0.799V | |||||
| Cu2+ + 2e- → Cu(s) | E(knot)=0.337V | |||||
Homework Answers
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Use the Nernst equation to calculate the concentration
of the unknown solution. Base this on your...
Use the Nernst equation to calculate the theoretical value of E of th copper-concentration cell and compare this value...
Use the Nernst equation to calculate the theoretical value of E of th copper-concentration cell and compare this value with th cell potential you measured. E = E* - 0.0592 / n * logQ **So I believe this is the equation that I would use. However, i'm don't know what E* is suppose to be...** The my electrochemistry experiment the cell potential that i measured were: 0.130V, 0.115V, and 0.110V (average cell potential = 0.118V) The concentration of the copper...
Instead of using zinc, a student accidentally used a 1 M solution of silver (Ag). Based...
Instead of using zinc, a student accidentally used a 1 M solution of silver (Ag). Based on the information in the table below, what would be the theoretical cell voltage, Eocell, when it is used in a galvanic cell with copper? Electrode Eo Ag+ + e- à Ag +0.80 V Cu2+ + 2e- à Cu +0.34 V Pb2+ + 2e- à Pb -0.13 V Zn2+ + 2e- à Zn -0.76 V Al3+ + 3e- à Al -1.66 V
Use the table of Standdard Reduction Potentials and the Nernst Equation to calculate the concentration of...
Use the table of Standdard Reduction Potentials and the Nernst
Equation to calculate the concentration of Cu2+ present in the
Cu/Cu2+ half-cell after the addition NH3 (aq) while it was coupled
with
a) Zn/Zn2+
b) Ag/Ag+
Table 2 has your measured voltages for these cells. SHOW YOUR
SETUP OF THE NERST EQUATION WITH ALL VARIABLES FILLED IN. SHOW THE
CALCULATED [Cu2+] CONCENTRATION.
Table 2:
METAL
Mg
Ag
Ni
Zn
Pb
Cu
1.230 V
0.642 V
0.030 V
0.648 V
0.256...
use the nernst equation to calculate the theoretical value of E of the copper concentration cell...
use the nernst equation to calculate the theoretical
value of E of the copper concentration cell and compare this value
with the cell potential that you measured
DATA TABLE Results of Parts I and II Cu/Pb X/Pb Y/Pb 0.431 0.172 0.581 Average cell potential (V) Results of Part III Cu concentration 0.042 Average cell potential (V)
Find the best combination of half-cell pair from the following list, which will give the highest...
Find the best combination of half-cell pair from the following list, which will give the highest voltage. What is the voltage for that Galvanic cell? Given that Reduction Half-reaction Standard Potential (Eredo) Zn2+(aq) + 2e– → Zn(s) -0.763 (V) Fe2+(aq) + 2e– → Fe(s) -0.44 (V) Cu2+(aq) + 2e– → Cu(s) +0.34 (V) Sn2+(aq) + 2e– → Sn(s) -0.14 (V) Cu2+(aq) + e– → Cu+(aq) + 0.153 (V) Ag+(aq) + e– → Ag(s) + 0.80 (V) Cu+(aq) + e– →...
Use the Nernst equation to calculate the expected voltage of the concentration cell before the addition...
Use the Nernst equation to calculate the expected voltage of the concentration cell before the addition of the 10 extra drops of 0.10 M copper(II) nitrate solution. Use your experimental temperature. How did the addition of 10 drops of 0.10 M cupric nitrate affect the concentration cells voltage? Why? Temp. 21C E=91V 10 drops 75.8V
9. Copper and silver are in contact with an aqueous solution at 25°C containing Cu2+ and...
9. Copper and silver are in contact with an aqueous solution at 25°C containing Cu2+ and Ag+ ions setting up a corrosion cell. a) Show the anode and cathode reactions. b) Now show the overall cell reaction. c) If [Cu2+] = 10-M and (Ag*] -0.5M, calculate the cell voltage. Except for sign, standard electrode potentials are absolute. They do not change if you change the stoichiometry of the reaction. Electrode Reaction E° (V) Cu2+ + 2e = Cu Ag+ +e...
I just want to double check my work for Q1, 2, 3 in the blank spaces and the Nernst equations. Concentration Cells 1) C...
I just want to double check my work for Q1, 2, 3 in the blank
spaces and the Nernst equations.
Concentration Cells 1) Concentration cell #1 : Which solution is being reduced, the IM Cu2 or the 0.001M Cu? VE 90 What was the measured cell potential for the 1M Cu/0.001 M Cu concentration cell? 14,S mV Measured Ecel= Use the Nernst equation to calculate the expected cell potential for the 1M Cu/0.001M Cu concentration cell; refer to the experimental...
Using the table below: 19. Three combinations of metals are listed below, which combination would produce...
Using the table below:
19. Three combinations of metals are listed below, which
combination would produce the largest voltage if they were used to
construct an electrochemical cell?
Copper (Cu) with zinc (Zn)
Lead (Pb) with zinc (Zn)
Lead (Pb) with cadmium (Cd)
Liu lur the reaction between Zn and Cu2+ ions is 1.1030 V, we can use the known value for the half-cell potential for zinc to determine the half-cell potential for copper: Zn(s) → Zn2+(aq) + 2e +...
Using the information in the table: Which combination of metals, if used to create an electrochemical...
Using the information in the table:
Which combination of metals, if used to create an
electrochemical cell, would produce the largest voltage?
Liu lur the reaction between Zn and Cu2+ ions is 1.1030 V, we can use the known value for the half-cell potential for zinc to determine the half-cell potential for copper: Zn(s) → Zn2+(aq) + 2e + Cu2+(aq) + 2e → Cu(s) Zn(s) + Cu2+ (aq) → Zn2+ (aq) + Cu(s) E half-cell = 0.7628 V Eºhalf-cell =...
Use the table of Standdard Reduction Potentials and the Nernst
Equation to calculate the concentration of Cu2+ present in the
Cu/Cu2+ half-cell after the addition NH3 (aq) while it was coupled
with
a) Zn/Zn2+
b) Ag/Ag+
Table 2 has your measured voltages for these cells. SHOW YOUR
SETUP OF THE NERST EQUATION WITH ALL VARIABLES FILLED IN. SHOW THE
CALCULATED [Cu2+] CONCENTRATION.
Table 2:
METAL
Mg
Ag
Ni
Zn
Pb
Cu
1.230 V
0.642 V
0.030 V
0.648 V
0.256...
use the nernst equation to calculate the theoretical
value of E of the copper concentration cell and compare this value
with the cell potential that you measured
DATA TABLE Results of Parts I and II Cu/Pb X/Pb Y/Pb 0.431 0.172 0.581 Average cell potential (V) Results of Part III Cu concentration 0.042 Average cell potential (V)
9. Copper and silver are in contact with an aqueous solution at 25°C containing Cu2+ and Ag+ ions setting up a corrosion cell. a) Show the anode and cathode reactions. b) Now show the overall cell reaction. c) If [Cu2+] = 10-M and (Ag*] -0.5M, calculate the cell voltage. Except for sign, standard electrode potentials are absolute. They do not change if you change the stoichiometry of the reaction. Electrode Reaction E° (V) Cu2+ + 2e = Cu Ag+ +e...
I just want to double check my work for Q1, 2, 3 in the blank
spaces and the Nernst equations.
Concentration Cells 1) Concentration cell #1 : Which solution is being reduced, the IM Cu2 or the 0.001M Cu? VE 90 What was the measured cell potential for the 1M Cu/0.001 M Cu concentration cell? 14,S mV Measured Ecel= Use the Nernst equation to calculate the expected cell potential for the 1M Cu/0.001M Cu concentration cell; refer to the experimental...
Using the table below:
19. Three combinations of metals are listed below, which
combination would produce the largest voltage if they were used to
construct an electrochemical cell?
Copper (Cu) with zinc (Zn)
Lead (Pb) with zinc (Zn)
Lead (Pb) with cadmium (Cd)
Liu lur the reaction between Zn and Cu2+ ions is 1.1030 V, we can use the known value for the half-cell potential for zinc to determine the half-cell potential for copper: Zn(s) → Zn2+(aq) + 2e +...
Using the information in the table:
Which combination of metals, if used to create an
electrochemical cell, would produce the largest voltage?
Liu lur the reaction between Zn and Cu2+ ions is 1.1030 V, we can use the known value for the half-cell potential for zinc to determine the half-cell potential for copper: Zn(s) → Zn2+(aq) + 2e + Cu2+(aq) + 2e → Cu(s) Zn(s) + Cu2+ (aq) → Zn2+ (aq) + Cu(s) E half-cell = 0.7628 V Eºhalf-cell =...
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