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
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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 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...
Using the Nernst equation, determine the concetration of Cu(II) needed to produce a concentration cell, in...
Using the Nernst equation, determine the concetration of Cu(II) needed to produce a concentration cell, in combination with the provided 0.10 M Cu(II) solution, that will have a measured cell potential of 0.030 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...
U could be 0++ slightly due monitor, or concentrations that were not liom, cell putu 2....
U could be 0++ slightly due monitor, or concentrations that were not liom, cell putu 2. (Part II) Use the Nernst equation to calcula 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. ESE
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
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
Use the Nernst euation and the cell potential for the Pb-PbI2 cell and the known [Pb2+] to calculate the [Pb2+] in equ...
Use the Nernst euation and the cell potential for the Pb-PbI2 cell and the known [Pb2+] to calculate the [Pb2+] in equilibrium with PbI2. The measured avgerage cell potential of Pb-PbI2 is 0.084 V the known [Pb2+] is 0.050 M Eo of Pb2+ (aq) + 2 e- --------> Pb(s) is -0.13 V 0.050 M KI Mixed 9 mL of 0.050 M KI with 3 mL of 0.050 M Pb(NO3)2 .
B1. Construction of Galvanic Cells a. For each galvanic cells you construct, calculate the theoretical cell...
B1. Construction of Galvanic Cells a. For each galvanic cells you construct, calculate the theoretical cell potential using the table of the Standard Electrode Potentials from the Chemistry 0130 data booklet. (3 marks) Measured Galvanic Cells Cathode reaction Anode reaction Voltage (V) Cu?*/Cu and Zn/Zn? 0.937 v Zn/Zn2+ and Ag /Ag 1.329v Ag"/Ag and Cu/Cu2+ 0.394v Electrochemistry 9 b. For each galvanic cells, write the overall cell reaction (balanced net ionic equation). • identify the oxidizing agent (OA) and reducing...
Prelab Questions: (PL1) For 6 galvanic cell combinations in part 1, write a chemical equation for each cell i...
Prelab Questions: (PL1) For 6 galvanic cell combinations in part 1, write a chemical equation for each cell in a direction that would be spontaneous and the overall cell potential (PL2) For part 2, what is the expected cell potential for that concentration cell? (PL3) Draw a data table you will be filling in during the lab. Include all the measurements that will be made in this lab and qualitative observation if needed. Procedure: Part 1) (1) Obtain copper strip,...
Prelab Activity: Electrochemical Cells To determine the solubility product of copper(II) carbonate, CuCO3 , a concentration...
Prelab Activity:
Electrochemical Cells
To determine the solubility product of copper(II) carbonate,
CuCO3 , a concentration cell as described on pages 71-72
of the lab handout is constructed. The temperature of the Galvanic
cell is measured to be 22.5°C, and the cell potential 282 mV (0.282
V). Using this data and Equation 8 in the lab manual, calculate the
Ksp for CuCO3 and report your answer with
three significant digits.
For the Galvanic cell you will construct in PART B,...
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...
U could be 0++ slightly due monitor, or concentrations that were not liom, cell putu 2. (Part II) Use the Nernst equation to calcula 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. ESE
B1. Construction of Galvanic Cells a. For each galvanic cells you construct, calculate the theoretical cell potential using the table of the Standard Electrode Potentials from the Chemistry 0130 data booklet. (3 marks) Measured Galvanic Cells Cathode reaction Anode reaction Voltage (V) Cu?*/Cu and Zn/Zn? 0.937 v Zn/Zn2+ and Ag /Ag 1.329v Ag"/Ag and Cu/Cu2+ 0.394v Electrochemistry 9 b. For each galvanic cells, write the overall cell reaction (balanced net ionic equation). • identify the oxidizing agent (OA) and reducing...
Prelab Questions: (PL1) For 6 galvanic cell combinations in part 1, write a chemical equation for each cell in a direction that would be spontaneous and the overall cell potential (PL2) For part 2, what is the expected cell potential for that concentration cell? (PL3) Draw a data table you will be filling in during the lab. Include all the measurements that will be made in this lab and qualitative observation if needed. Procedure: Part 1) (1) Obtain copper strip,...
Prelab Activity:
Electrochemical Cells
To determine the solubility product of copper(II) carbonate,
CuCO3 , a concentration cell as described on pages 71-72
of the lab handout is constructed. The temperature of the Galvanic
cell is measured to be 22.5°C, and the cell potential 282 mV (0.282
V). Using this data and Equation 8 in the lab manual, calculate the
Ksp for CuCO3 and report your answer with
three significant digits.
For the Galvanic cell you will construct in PART B,...
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