zn ls) 2 ทั้า(o.1o)11 Fe2+Co.10m) 1 Fecz) Fe (0.10 MyFe -0.35V Calculation Pb (0.10 M)/Pb Calculation Unk2 (0.10 MyUnk Calculation Dilutions of 0.10 M Cu(NO3)2 solution Solution Ecell Eces(calculated) Number . 84 0.8& 0.64 V 0.42V 2 Calculation of [Cu"] in solutions 2, 3, and 4: Calculation of theoretical Ecel for the coupling of Zine with solutions 1,2, 3, and 4
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Mcasured Cell Potentials of Redo x Couples from cells A1. A2, Bl. B2, and Unknown #1 Redox Measur...
Mcasured Cell Potentials of Redo x Couples from cells A1. A2, Bl. B2, and Unknown #1...
Mcasured Cell Potentials of Redo x Couples from cells A1. A2, Bl. B2, and Unknown #1 Redox Measured Anode Anode Reaction Cathode Cathode Reaction CouplePotential Cu-Zn 10.qqv|Zn |2n→ (Al-B2) Cu-Pb Pb-Zn (BI-B2) 0-46V Fe-Pb Fe-Zn Cu-Fe (AI-A2) Zn-Unk#1 (B2-A3) 0.3Iv Unkel Assuming that the reduction potential for Zn2 (0.10 M/Zn is equal to -0.79 V, calculate the reduction potentials for the remaining cells: Cu (0.10 M/Cu 0.2ov Calculation: 95 0- 0.71-0.20V zn ls) 2 ทั้า(o.1o)11 Fe2+Co.10m) 1 Fecz) Fe (0.10...
Separate galvanic cells are made from the following half-cells: cell 1: H+(aq)/H2(g) and Pb2+(aq)/Pb(s) cell 2:...
Separate galvanic cells are made from the following half-cells: cell 1: H+(aq)/H2(g) and Pb2+(aq)/Pb(s) cell 2: Fe2+(aq)/Fe(s) and Zn2+(aq)/Zn(s) Which of the following is correct for the working cells? Standard reduction potentials, 298 K, Aqueous Solution (pH = 0): Cl2(g) + 2e --> 2C1-(aq); E° = +1.36 V Fe3+(aq) + e --> Fe2+(aq); E° = +0.77 V Cu2+(aq) + 2e --> Cu(s); E° = +0.34 V 2H+(aq) + 2e --> H2(g); E° = 0.00 V Pb2+(aq) + 2e --> Pb(s);...
Chem 1212 Lab Report on electrochemistry Electrochemistry When electrons transfer between reaction components in a redox...
Chem 1212 Lab Report on electrochemistry
Electrochemistry When electrons transfer between reaction components in a redox reaction, we can harness the motion of the electrons to create a potential. Electrochemistry revolves around the separation of the two half-reactions in a redox reaction and establishing two different electrodes. This might involve physically separating the half-reactions or including a separator, such as a semi-permeable membrane or plastic dividers. With the reactions separated, the electrons will need to flow through the wire connecting...
need help with the rest of the table EXPERIMENT 10 DETERMINATION OF THE ELECTROCHEMICAL SERIES PURPOSE...
need help with the rest of the table
EXPERIMENT 10 DETERMINATION OF THE ELECTROCHEMICAL SERIES PURPOSE To determine the standard cell potential values of several electrochemical coll INTRODUCTION The basis for an electrochemical cell is an oxidation reduction Corredor be divided into two half reactions reaction. This reaction can Oxidation half reaction Gloss of electrons) takes place at the anode, which is the positive electrode that the anions migrate to Chence the name anode) Reduction half reaction (gain of electrons)...
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...
need help for half cell potentials pls calculate step by step (NOTE - Remember that the...
need help for half cell potentials pls calculate step by step
(NOTE - Remember that the positive electrode is attached to the red wire and the negative electrode is attached to the black wire.) Electrode Systems Used Anode (oxidation) Negative Cathode (reduction) Positive Measured Potential (V) Positive (Ecu) Copper and silver Cu() - Cu2+ + 2e" Ag+ +1e Ag) 0.432 V Zinc + Silver Zn cs + 2n**+ Zé dat + leº nAg (s) 1.484 V Copper & Zinc Zn(s)...
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...
Standard reduction potentials are listed for reactions under standard conditions. Standard conditions are 1 M concentrations of ions, 1 atm (or 1 bar) partial pressures for gases, and a tem...
Standard reduction potentials are listed for reactions under standard conditions. Standard conditions are 1 M concentrations of ions, 1 atm (or 1 bar) partial pressures for gases, and a temperature of 298 K a. In Part I, you were asked to compare your measured cell potential to a calculated standard cell 3. potential. The cell potential you measured was for a galvanic cell you prepared using 0.10 M solutions of Pb and Cu, not 1.0 M solutions. Write out the...
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?...
ANSWER ALL 3 QUESTIONS AND ALL PARTS Question 1 Using the standard reduction potentials on page 127, draw a compl...
ANSWER ALL 3 QUESTIONS AND ALL PARTS
Question 1 Using the standard reduction potentials on page 127, draw a complete galvanic cell in the space below for Fe Ag a) Clearly label the electrodes, the solutions and the salt bridge. Clearly label which metal is the cathode and anode and a chemical you might use for the salt bridge. b) Give the half-reaction that occurs at the cathode and the half-reaction that occurs at the anode and indicate the direction...
Mcasured Cell Potentials of Redo x Couples from cells A1. A2, Bl. B2, and Unknown #1 Redox Measured Anode Anode Reaction Cathode Cathode Reaction CouplePotential Cu-Zn 10.qqv|Zn |2n→ (Al-B2) Cu-Pb Pb-Zn (BI-B2) 0-46V Fe-Pb Fe-Zn Cu-Fe (AI-A2) Zn-Unk#1 (B2-A3) 0.3Iv Unkel Assuming that the reduction potential for Zn2 (0.10 M/Zn is equal to -0.79 V, calculate the reduction potentials for the remaining cells: Cu (0.10 M/Cu 0.2ov Calculation: 95 0- 0.71-0.20V zn ls) 2 ทั้า(o.1o)11 Fe2+Co.10m) 1 Fecz) Fe (0.10...
Separate galvanic cells are made from the following half-cells: cell 1: H+(aq)/H2(g) and Pb2+(aq)/Pb(s) cell 2: Fe2+(aq)/Fe(s) and Zn2+(aq)/Zn(s) Which of the following is correct for the working cells? Standard reduction potentials, 298 K, Aqueous Solution (pH = 0): Cl2(g) + 2e --> 2C1-(aq); E° = +1.36 V Fe3+(aq) + e --> Fe2+(aq); E° = +0.77 V Cu2+(aq) + 2e --> Cu(s); E° = +0.34 V 2H+(aq) + 2e --> H2(g); E° = 0.00 V Pb2+(aq) + 2e --> Pb(s);...
Chem 1212 Lab Report on electrochemistry
Electrochemistry When electrons transfer between reaction components in a redox reaction, we can harness the motion of the electrons to create a potential. Electrochemistry revolves around the separation of the two half-reactions in a redox reaction and establishing two different electrodes. This might involve physically separating the half-reactions or including a separator, such as a semi-permeable membrane or plastic dividers. With the reactions separated, the electrons will need to flow through the wire connecting...
need help with the rest of the table
EXPERIMENT 10 DETERMINATION OF THE ELECTROCHEMICAL SERIES PURPOSE To determine the standard cell potential values of several electrochemical coll INTRODUCTION The basis for an electrochemical cell is an oxidation reduction Corredor be divided into two half reactions reaction. This reaction can Oxidation half reaction Gloss of electrons) takes place at the anode, which is the positive electrode that the anions migrate to Chence the name anode) Reduction half reaction (gain of electrons)...
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...
need help for half cell potentials pls calculate step by step
(NOTE - Remember that the positive electrode is attached to the red wire and the negative electrode is attached to the black wire.) Electrode Systems Used Anode (oxidation) Negative Cathode (reduction) Positive Measured Potential (V) Positive (Ecu) Copper and silver Cu() - Cu2+ + 2e" Ag+ +1e Ag) 0.432 V Zinc + Silver Zn cs + 2n**+ Zé dat + leº nAg (s) 1.484 V Copper & Zinc Zn(s)...
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...
Standard reduction potentials are listed for reactions under standard conditions. Standard conditions are 1 M concentrations of ions, 1 atm (or 1 bar) partial pressures for gases, and a temperature of 298 K a. In Part I, you were asked to compare your measured cell potential to a calculated standard cell 3. potential. The cell potential you measured was for a galvanic cell you prepared using 0.10 M solutions of Pb and Cu, not 1.0 M solutions. Write out the...
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?...
ANSWER ALL 3 QUESTIONS AND ALL PARTS
Question 1 Using the standard reduction potentials on page 127, draw a complete galvanic cell in the space below for Fe Ag a) Clearly label the electrodes, the solutions and the salt bridge. Clearly label which metal is the cathode and anode and a chemical you might use for the salt bridge. b) Give the half-reaction that occurs at the cathode and the half-reaction that occurs at the anode and indicate the direction...
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