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Part B. Data for voltaic cells Calculatedbserved Electrodes Cathode Half ReactionTAnode Half-Reaction Voltage 2+ 1.530 uH...
predicted voltage 1,2,3? ulations Part I: Voltaic Cells A. Cell Potentials Using a Zn(s)/Zn (aq) Reference...
predicted voltage 1,2,3?
ulations Part I: Voltaic Cells A. Cell Potentials Using a Zn(s)/Zn (aq) Reference Electrode Complete the following table using your mean values for PartI A, and assigning a reference voltage of 0.00 volts for the reduction of Zn2 to Zn. Put the voltages in increasing order Half-Reaction Standard Reduction Potential at 25 °C, Volts Zn (aq) + 2e Zn (s) 0.00 Fers +7 0.30 0.5 Phess B.Cell Potentials Using the Table Above Redox Couple predicted voltage observed...
Part I: Voltaic Cells Use your textbook or other resource to complete the following table: Half-Reaction...
Part I: Voltaic Cells Use your textbook or other resource to complete the following table: Half-Reaction Zn2 ag)2eZn Fe (a)2e Fe (s) Standard Reduction Potential at 25 °C, Volts 0.76 13 34 Cu2+ (aq) +2e- Cu (s) → Use the table above to predict voltlages for the redox couples studied in Part L, sections A and B. Redox Couple predicted voltage observed voltage 1. Zn/Cu 2. Zn/Pb 3. Pb/Cu 4. Fe/Cu 87 405
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...
Lab11_PP_147-156... * 5 79 Calculations Part I:Voltaic Cells A. Cell Potentials Using a Zn(s)[Zn2+ (aq) Reference...
Lab11_PP_147-156... * 5 79 Calculations Part I:Voltaic Cells A. Cell Potentials Using a Zn(s)[Zn2+ (aq) Reference Electrode Complete the following table using your mean values for Part 1 A, and assigning a reference voltage of 0.00 volts for the reduction of Zn?t to Zn. Put the voltages in increasing order. Half-Reaction Standard Reduction Potential at 25 °C, Volts Zn2+ (aq) + 2e → Zn (s) 0.00 0.328 0.443 0.907 observed voltage 0.469 percent error B. Cell Potentials Using the Table...
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,...
can someone help me write the half reactions for part A and B. 2. Electrolytic Cells...
can someone help me write the half reactions for part A and
B.
2. Electrolytic Cells A. In a small beaker, mix 1 mL of 0.1 M sodium iodide solution, 9 mL of water, 1 mL of fresh starch solution, and two drops of phenolphthalein indicator. Lead wires from a dry cell or storage battery into this solution and observe the region around each wire (9). Write half- reaction equations for the reactions (10). What would happen if the reaction...
please help answer question 4, a-f please using the data below from chart 1 objectives from...
please help answer question 4, a-f please
using the data below from chart 1
objectives from lab, thank you
DATA:CA y 3 Ay No3 Part I: Cell Potential of voltaic cells under standard conditions: cell CU CND2 #27 14.0m Give the half Half cell reaction at Combinations Oxidation Reduction E the anode and with [ion] takes place Theoretical takes place cathode. Write in M here here (V) above the arrow E c (V) if it is oxidation or reduction. |-0.340...
please help fill out chart 1 by using the data belowed thank you! DATA:Cag] "Ay No₃...
please help fill out chart 1 by using the data belowed thank
you!
DATA:Cag] "Ay No₃ cell cell CUCNO3)27144-1.0m AgNO3 ! Agu = 10M Part I: Cell Potential of voltaic cells under standard conditions: Give the half Half cell reaction at Oxidation Combinations Reduction E the anode and Theoretical with [ion] takes place takes place cathode. Write in M here here (V) above the arrow if it is oxidation or reduction. -0.340 Ag - Cu Cucs) Agters oxi Anode: 0.3440.00...
5. What was the purpose of the NaNO3 solution in this experiment? 6. Could a solution...
5. What was the purpose of the NaNO3 solution in this experiment? 6. Could a solution of NaCl be used instead of NaNO3? 7. What was the purpose of FeSO4 solution in this experiment? 8. Could a solution of FeCl, be used instead of FeSO4? 9. Could a solution of NaSO4 be used instead of FeSO4? 10. Calculate the standard cell potential for the spontaneous redox reaction between a Pb(s)/Pb(NO3)2(aq) half-cell and a Ag(s)/AgNO3(aq) half-cell. Which metal would be oxidized?...
Page 1 and 2 are instructions. Please help me solve K for page 3 and page...
Page 1 and 2 are instructions. Please help me solve K for page 3
and page 4 and please check the other work on Page 3.
Thanyou very much. Will Rate!
CHM 112 Electrochemical Cells and Thermodynamics Section A. Constructing a Small-Scale Electrochemical Cell Woodbridge Campus Objective To construct a small-scale electrochemical cell using a redox system, to measure the cell potential and derive thermodynamic quantities. Procedures 1. Connect the red and black alligator clips to the multimeter to read...
predicted voltage 1,2,3?
ulations Part I: Voltaic Cells A. Cell Potentials Using a Zn(s)/Zn (aq) Reference Electrode Complete the following table using your mean values for PartI A, and assigning a reference voltage of 0.00 volts for the reduction of Zn2 to Zn. Put the voltages in increasing order Half-Reaction Standard Reduction Potential at 25 °C, Volts Zn (aq) + 2e Zn (s) 0.00 Fers +7 0.30 0.5 Phess B.Cell Potentials Using the Table Above Redox Couple predicted voltage observed...
Part I: Voltaic Cells Use your textbook or other resource to complete the following table: Half-Reaction Zn2 ag)2eZn Fe (a)2e Fe (s) Standard Reduction Potential at 25 °C, Volts 0.76 13 34 Cu2+ (aq) +2e- Cu (s) → Use the table above to predict voltlages for the redox couples studied in Part L, sections A and B. Redox Couple predicted voltage observed voltage 1. Zn/Cu 2. Zn/Pb 3. Pb/Cu 4. Fe/Cu 87 405
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...
Lab11_PP_147-156... * 5 79 Calculations Part I:Voltaic Cells A. Cell Potentials Using a Zn(s)[Zn2+ (aq) Reference Electrode Complete the following table using your mean values for Part 1 A, and assigning a reference voltage of 0.00 volts for the reduction of Zn?t to Zn. Put the voltages in increasing order. Half-Reaction Standard Reduction Potential at 25 °C, Volts Zn2+ (aq) + 2e → Zn (s) 0.00 0.328 0.443 0.907 observed voltage 0.469 percent error B. Cell Potentials Using the Table...
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,...
can someone help me write the half reactions for part A and
B.
2. Electrolytic Cells A. In a small beaker, mix 1 mL of 0.1 M sodium iodide solution, 9 mL of water, 1 mL of fresh starch solution, and two drops of phenolphthalein indicator. Lead wires from a dry cell or storage battery into this solution and observe the region around each wire (9). Write half- reaction equations for the reactions (10). What would happen if the reaction...
please help answer question 4, a-f please
using the data below from chart 1
objectives from lab, thank you
DATA:CA y 3 Ay No3 Part I: Cell Potential of voltaic cells under standard conditions: cell CU CND2 #27 14.0m Give the half Half cell reaction at Combinations Oxidation Reduction E the anode and with [ion] takes place Theoretical takes place cathode. Write in M here here (V) above the arrow E c (V) if it is oxidation or reduction. |-0.340...
please help fill out chart 1 by using the data belowed thank
you!
DATA:Cag] "Ay No₃ cell cell CUCNO3)27144-1.0m AgNO3 ! Agu = 10M Part I: Cell Potential of voltaic cells under standard conditions: Give the half Half cell reaction at Oxidation Combinations Reduction E the anode and Theoretical with [ion] takes place takes place cathode. Write in M here here (V) above the arrow if it is oxidation or reduction. -0.340 Ag - Cu Cucs) Agters oxi Anode: 0.3440.00...
5. What was the purpose of the NaNO3 solution in this experiment? 6. Could a solution of NaCl be used instead of NaNO3? 7. What was the purpose of FeSO4 solution in this experiment? 8. Could a solution of FeCl, be used instead of FeSO4? 9. Could a solution of NaSO4 be used instead of FeSO4? 10. Calculate the standard cell potential for the spontaneous redox reaction between a Pb(s)/Pb(NO3)2(aq) half-cell and a Ag(s)/AgNO3(aq) half-cell. Which metal would be oxidized?...
Page 1 and 2 are instructions. Please help me solve K for page 3
and page 4 and please check the other work on Page 3.
Thanyou very much. Will Rate!
CHM 112 Electrochemical Cells and Thermodynamics Section A. Constructing a Small-Scale Electrochemical Cell Woodbridge Campus Objective To construct a small-scale electrochemical cell using a redox system, to measure the cell potential and derive thermodynamic quantities. Procedures 1. Connect the red and black alligator clips to the multimeter to read...
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