QUESTION 8 Refer to the data you obtained in the simulation for the concentration cells. Select...
QUESTION 8
-
Refer to the data you obtained in the simulation for the concentration cells.
Select the correct statements that describe the concentration cell with half cells containing 0.01 M Cu2+ and 0.10 M Cu2+ respectively
The voltage is 29.6 mV
The voltage is 59.2 mV
The solution containing 0.1 M Cu2+ is at the cathode
The solution containing 1.0 M Cu2+ is at the cathode
The solution containing 0.1 M Cu2+ is at the anode
The solution containing 0.01 M Cu2+ is at the anode
The equation for the reaction is
Cu2+ (aq, 0.1 M) + Cu(s) --> Cu2+ (aq, 0.01 M) + Cu(s)
The equation for the reaction is
Cu2+ (aq, 0.01 M) + Cu(s) --> Cu2+ (aq, 0.1 M) + Cu(s)
8 points
QUESTION 9
-
Refer to the data you obtained in the simulation for the concentration cells.
Select the correct statements that describe the concentration cell with half cells containing 0.01 M Cu2+ and 1.0 M Cu2+ respectively
The voltage is 29.6 mV
The voltage is 59.2 mV
The solution containing 0.1 M Cu2+ is at the cathode
The solution containing 1.0 M Cu2+ is at the cathode
The solution containing 0.1 M Cu2+ is at the anode
The solution containing 0.01 M Cu2+ is at the anode
The equation for the reaction is
Cu2+ (aq, 0.01 M) + Cu(s) --> Cu2+ (aq, 1.0 M) + Cu(s)
The equation for the reaction is
Cu2+ (aq, 1.0 M) + Cu(s) --> Cu2+ (aq, 0.01 M) + Cu(s)
8 points
QUESTION 10
-
Refer to the data you obtained in the simulation for the concentration cells.
Select the correct statements that describe the concentration cell with half cells containing 0.1 M Cu2+ and 1.0 M Cu2+ respectively
The voltage is 29.6 mV
The voltage is 59.2 mV
The solution containing 0.1 M Cu2+ is at the cathode
The solution containing 1.0 M Cu2+ is at the cathode
The solution containing 0.1 M Cu2+ is at the anode
The solution containing 0.01 M Cu2+ is at the anode
The equation for the reaction is
Cu2+ (aq, 0.1 M) + Cu(s) --> Cu2+ (aq, 1.0 M) + Cu(s)
The equation for the reaction is
Cu2+ (aq, 1.0 M) + Cu(s) --> Cu2+ (aq, 0.1 M) + Cu(s)
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QUESTION 8
Refer to the data you obtained in the simulation for the
concentration cells.
Select...
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,...
In Part B we were going to construct concentration cells. In these galvanic cells, the driving...
In Part B we were going to construct concentration cells. In these galvanic cells, the driving force is the difference in concentration in the two half-cells. Write the anode and cathode reactions for a concentration cell which contains 0.1 M Cu2+ in one half-cell and 0.01 M Cu2+ in the other. (Be clear as to which [Cu2+] is being oxidized or reduced).
some questions are filled out but still need help woth the remainder of this assignment part...
some questions are filled out but still need help woth the
remainder of this assignment
part B and below needs to be answered.
Paragraph Styles . . Electrochemical Cells Objective: Investigate electrochemical potential using electrochemical cells. Information: Electric current is the flow of negatively charged particles. An electrochemical cell is a device that creates an electric current by converting chemical energy into electric current, or vice versa. Voltaic cells are electrochemical cells that produce current spontaneously by converting chemical energy...
A concentration cell composed of Cu(s)/Cu2+(aq, 0.10M)||Cu2+(aq, 1.0M)| Cu(s) is connected to a voltmeter. Initially a...
A concentration cell composed of Cu(s)/Cu2+(aq, 0.10M)||Cu2+(aq, 1.0M)| Cu(s) is connected to a voltmeter. Initially a reading of 29.6 mV was obtained. The cell was left sitting for a few minutes. How has the voltage change compared to the initial reading? Why did this change occur?
14.__/15 pts) In a concentration cell, a voltage can be created when one compartment has a...
14.__/15 pts) In a concentration cell, a voltage can be created when one compartment has a concentrated solution while the other has a dilute solution. • Let's build one out of the Cu?"(aq) + 2e → Cu(s) half reaction, using 1.00 M Cu?"(aq) in one half cell and 1.58 x 10 M Cu?"(aq) in the other half cell. A) Label the diagram below; identify the copper electrodes and the [Cu?") in each half-cell along with the anode, cathode, and direction...
looking for help for question 1 please Experiment 23 Electrochemical Cells Postlaboratory Questions Lell potentials are...
looking for help for question 1 please
Experiment 23 Electrochemical Cells Postlaboratory Questions Lell potentials are state functions so the cell potential for Zn (s)[Zn- (aq) Fe (aq me added to the cell potential for Fe+ (aq) Fe (s) Cu²+ (aq)Cu (s) should equal the cell potential of Zn (s)IZn2+ (aq)||Cu2+ (aq) Cu (s). a. Does this hold using the theoretical cell potentials? b. Does this hold using the experimentally determined cell potentials? c. Why might the two differ? 2....
Table provided below for context Please answer all parts that you can. 1. Which electrochemical cell...
Table provided below for context
Please answer all parts that you can.
1. Which electrochemical cell had the greatest voltage? Identify the anode and the cathode for this pair, the measured cell potential, and the calculated Eºcell- 2. Which electrochemical cell had the smallest voltage? Identify the anode and the cathode for this pair, the measured cell potential, and the calculated Eºcell- 3. If the oxidation and reduction half-reactions are separated in a battery, this means the oxidizing agent is...
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...
need help with last column on both charts art II-A - Effect of concentration pn the...
need help with last column on both charts
art II-A - Effect of concentration pn the voltage of voltaic cell: Onda ti on cauction At which Half cell At which electrode electrode Combinations E electrons are electrons are with lion) product? This reactant? This in M is anode or is anode or cathode? cathode? Give the half reaction and write above the arrow if it is oxidation or reduction. (V) Ag - Cu 7 Angezom This is cung) 0.1m Anode...
Equation 18: (didnt mean to attach equation 15 oops) V-13 EXPERIMENT V: VOLTAIC CELLS, AND THE...
Equation 18: (didnt mean to attach equation 15 oops)
V-13 EXPERIMENT V: VOLTAIC CELLS, AND THE NERNST EQUATION PRELAB ASSIGNMENT (CONTINUED) 5. In aqueous solution Cu* ions are more stable than Cu ions because 2 Cu* (aq) + Cu2+ (aq) + Cu (s) (a) Give an oxidation half-cell reaction and a reduction half-cell reaction that can be combined to form this overall reaction. (0.5 marks) (b) Use Eq. 18 with your answer to (a) to calculate the theoretical K for...
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,...
some questions are filled out but still need help woth the
remainder of this assignment
part B and below needs to be answered.
Paragraph Styles . . Electrochemical Cells Objective: Investigate electrochemical potential using electrochemical cells. Information: Electric current is the flow of negatively charged particles. An electrochemical cell is a device that creates an electric current by converting chemical energy into electric current, or vice versa. Voltaic cells are electrochemical cells that produce current spontaneously by converting chemical energy...
A concentration cell composed of Cu(s)/Cu2+(aq, 0.10M)||Cu2+(aq, 1.0M)| Cu(s) is connected to a voltmeter. Initially a reading of 29.6 mV was obtained. The cell was left sitting for a few minutes. How has the voltage change compared to the initial reading? Why did this change occur?
14.__/15 pts) In a concentration cell, a voltage can be created when one compartment has a concentrated solution while the other has a dilute solution. • Let's build one out of the Cu?"(aq) + 2e → Cu(s) half reaction, using 1.00 M Cu?"(aq) in one half cell and 1.58 x 10 M Cu?"(aq) in the other half cell. A) Label the diagram below; identify the copper electrodes and the [Cu?") in each half-cell along with the anode, cathode, and direction...
looking for help for question 1 please
Experiment 23 Electrochemical Cells Postlaboratory Questions Lell potentials are state functions so the cell potential for Zn (s)[Zn- (aq) Fe (aq me added to the cell potential for Fe+ (aq) Fe (s) Cu²+ (aq)Cu (s) should equal the cell potential of Zn (s)IZn2+ (aq)||Cu2+ (aq) Cu (s). a. Does this hold using the theoretical cell potentials? b. Does this hold using the experimentally determined cell potentials? c. Why might the two differ? 2....
Table provided below for context
Please answer all parts that you can.
1. Which electrochemical cell had the greatest voltage? Identify the anode and the cathode for this pair, the measured cell potential, and the calculated Eºcell- 2. Which electrochemical cell had the smallest voltage? Identify the anode and the cathode for this pair, the measured cell potential, and the calculated Eºcell- 3. If the oxidation and reduction half-reactions are separated in a battery, this means the oxidizing agent is...
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...
need help with last column on both charts
art II-A - Effect of concentration pn the voltage of voltaic cell: Onda ti on cauction At which Half cell At which electrode electrode Combinations E electrons are electrons are with lion) product? This reactant? This in M is anode or is anode or cathode? cathode? Give the half reaction and write above the arrow if it is oxidation or reduction. (V) Ag - Cu 7 Angezom This is cung) 0.1m Anode...
Equation 18: (didnt mean to attach equation 15 oops)
V-13 EXPERIMENT V: VOLTAIC CELLS, AND THE NERNST EQUATION PRELAB ASSIGNMENT (CONTINUED) 5. In aqueous solution Cu* ions are more stable than Cu ions because 2 Cu* (aq) + Cu2+ (aq) + Cu (s) (a) Give an oxidation half-cell reaction and a reduction half-cell reaction that can be combined to form this overall reaction. (0.5 marks) (b) Use Eq. 18 with your answer to (a) to calculate the theoretical K for...
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