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224 Experiment 25/An lavestigatios of Veitaie Cells-The Nerast Equation Section Report B. Cell Vo...
cell voltages/ net ionic equation 224 Experiment 25/An lavestigatios of Veitaie Cells-The Nerast Equation Section Report...
cell voltages/ net ionic equation
224 Experiment 25/An lavestigatios of Veitaie Cells-The Nerast Equation Section Report B. Cell Voltages For each cell you constructed, record (a) the potential (voltage) of the cell, (b) the polarity of the copper electrode, and (c) the net ionic equation for the reaction that occurred Copper Polarity Average Net Ionic Equation Cell Potential + or- 0.350-35/05 1.3414 1.34 0.50 0.504 0.50v 0.301 0.305 -0.30 v C. Effect of Concentration For each part, record the potential...
We created a Cu/Zn cell by placing 0.10 M ZnSO4 in to a porous cup and...
We created a Cu/Zn cell by placing 0.10 M ZnSO4 in to
a porous cup and poured 0.10 M CuSO4 in to a beaker
surrounding the porous cup. We placed a Zn electrode in to the Zn
solution and a copper electrode in the Cu solution.
a) Calculate the expected potential V (our measured potential V was
around 1.09 so it should be around there I believe)
b) The e- flow from which electrode?
c) The e- flow to which...
A student measures the potential of a cell m in the other. There is a copper...
A student measures the potential of a cell m in the other. There is a copper electrode in the CuSO, and a silver electro student finds the potential of the cell, Ecall to be 0. e potential of a cell made up with 1 M Cuso, in one solution and 1 M AgNO, the Cuso, and a silver electrode in the AgNO,. The otential of the cell, E., to be 0.47 V, and that the copper electrode is negative. 1....
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...
First fill in your half cell and cell reactions. F in standard cell potentials as you...
First fill in your half cell and cell reactions. F in standard cell potentials as you calculate them. Oxidation at the Anode: The black (.) lead is attached to the electrode, which is the source of electrons. Write the anode half reaction: Reduction at the Cathode: The red lead (+) is attached to the electrode. Write the cathode half reaction: E degree - V. Overall Cell Reaction (Net Ionic equation): Write the overall cell reaction (balance electrons and add together):...
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,...
V-25 OBSERVATIONS SHEET - EXPERIMENT V Voltaic Cell and the Nernst Equation Part I: Electrode Potentials...
V-25 OBSERVATIONS SHEET - EXPERIMENT V Voltaic Cell and the Nernst Equation Part I: Electrode Potentials You only have to record positive readings. If reading is negative, reverse the leads. The zero point value was out byvolts Electrode A Electrode B AglAg AglAg Ecel Which is the positive electrode? 1S.D 0.1у ver Cu Cu2 CulCu2 ZniZn2 Zn Zn2 Coppe odine Part II. Halgen Disnlacemant Units Show your work - answers without supporting work will get zero marks. and the correct...
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)...
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?...
cell voltages/ net ionic equation
224 Experiment 25/An lavestigatios of Veitaie Cells-The Nerast Equation Section Report B. Cell Voltages For each cell you constructed, record (a) the potential (voltage) of the cell, (b) the polarity of the copper electrode, and (c) the net ionic equation for the reaction that occurred Copper Polarity Average Net Ionic Equation Cell Potential + or- 0.350-35/05 1.3414 1.34 0.50 0.504 0.50v 0.301 0.305 -0.30 v C. Effect of Concentration For each part, record the potential...
We created a Cu/Zn cell by placing 0.10 M ZnSO4 in to
a porous cup and poured 0.10 M CuSO4 in to a beaker
surrounding the porous cup. We placed a Zn electrode in to the Zn
solution and a copper electrode in the Cu solution.
a) Calculate the expected potential V (our measured potential V was
around 1.09 so it should be around there I believe)
b) The e- flow from which electrode?
c) The e- flow to which...
A student measures the potential of a cell m in the other. There is a copper electrode in the CuSO, and a silver electro student finds the potential of the cell, Ecall to be 0. e potential of a cell made up with 1 M Cuso, in one solution and 1 M AgNO, the Cuso, and a silver electrode in the AgNO,. The otential of the cell, E., to be 0.47 V, and that the copper electrode is negative. 1....
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...
First fill in your half cell and cell reactions. F in standard cell potentials as you calculate them. Oxidation at the Anode: The black (.) lead is attached to the electrode, which is the source of electrons. Write the anode half reaction: Reduction at the Cathode: The red lead (+) is attached to the electrode. Write the cathode half reaction: E degree - V. Overall Cell Reaction (Net Ionic equation): Write the overall cell reaction (balance electrons and add together):...
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,...
V-25 OBSERVATIONS SHEET - EXPERIMENT V Voltaic Cell and the Nernst Equation Part I: Electrode Potentials You only have to record positive readings. If reading is negative, reverse the leads. The zero point value was out byvolts Electrode A Electrode B AglAg AglAg Ecel Which is the positive electrode? 1S.D 0.1у ver Cu Cu2 CulCu2 ZniZn2 Zn Zn2 Coppe odine Part II. Halgen Disnlacemant Units Show your work - answers without supporting work will get zero marks. and the correct...
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)...
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?...
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