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how do i do nerst equation 1. Standard Cells Voltaie Cell Data Sheet Experimental Cell Potential,...
Table view List view Ecell (calculated) Ecell (calculated) 1.115 1.124 Table 1. Voltaic cells data table...
Table view List view Ecell (calculated) Ecell (calculated) 1.115 1.124 Table 1. Voltaic cells data table Ecell (measured) Reaction Quotient Q 1. Zn | Zn2(1.0M) || Cu2+(1.0 M) | Cu 2. Zn | Zn2+(1.0 M) || Cu2+(0.1 M) Cu 1.067 3. ZnZn2+(0.1 M) || Cu2+(1.0 M) | Cu 4. Zn | Zn2+(1.0 M) || Pb2+(1.0 M) | Pb 5. ZnZn2(1.0M) || Pb2+(0.1 M) | Pb 0.600 6. Zn | Zn2+(0.1 M) || Pb2+(1.0 M) I Pb 0.644 7. ZnZn2+(1.0 M)...
Calculate the theoretical cell potential for each of the following cells. Is the cell, as written,...
Calculate the theoretical cell potential for each of the following cells. Is the cell, as written, galvanic or electrolytic? a. Pb | PbSO_4 (sat'd), SO_4^2- (0.200 M) || Sn^2+ (0.150 M), Sn^4+ (0.250 M)|Pt b. Pt |Fe^3+ (0.0100M), Fe^2+ (0.00100M) || Ag^+ (0.200M), CuI (sat'd) |Cu d. Pt | UO_2^2+ (0.0100 M), U^4+ (0.0100 M), H^+ (1.00 times 10^-6 M) || AgClO (sat'd), KCI (1.00 times 10^-4 M) |Ag
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...
Data Analysis Questions Q1. Complete Table 8.2 below. Using a standard half-cell potential of 0.34 V...
Data Analysis Questions Q1. Complete Table 8.2 below. Using a standard half-cell potential of 0.34 V for Cu2*/Cu, calculate the experimental reduction potentials for Mg, Pb, Sn, and Zn half-cells. Obtain standard reduction potentials from a suitable reference source. Show all of your work below and RANK the metals in terms of oxidizing and reducing ability according to the experimental half-cell potentials. (3.0) Table 8.2 Half-cell reduction reaction (include phase labels) Calculated E (v) Literature E (V) Culaq) + 2e...
how do I solve this? 1. Use the Nernst equation to calculate the standard cell potential...
how
do I solve this?
1. Use the Nernst equation to calculate the standard cell potential for a voltaic cell of a Sn electrode in 0.10M Sn2(a) in one half-cell and Al in 0.10M AP) in the other. (EPe Eaode- Emode 1.52 V, Show your work. Hint: Check E values of the reduction haif reactions. Write the one with more negative E as oxidation half reaction (change the sign); ensure that equal number of electrons are exchanged ie. electrons cancel,...
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...
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...
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...
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...
Problem Set #34: Galvanic Cells & Standard Reduction Potential Practice Sheet Directions: (a) Sketch the galvanic...
Problem Set #34: Galvanic Cells & Standard Reduction Potential Practice Sheet Directions: (a) Sketch the galvanic cell based on the following overall reaction OR half- reactions. o Show the direction of electron flow o Identify the cathode and anode (b) Give the overall balanced reaction (c) Determine the Evalues for each of the galvanic cells. (d) Give the standard line notation for each cell. (Assume that all concentrations are 1.0M and that all partial pressures are 1.0 atm) 1. 103(aq)...
Table view List view Ecell (calculated) Ecell (calculated) 1.115 1.124 Table 1. Voltaic cells data table Ecell (measured) Reaction Quotient Q 1. Zn | Zn2(1.0M) || Cu2+(1.0 M) | Cu 2. Zn | Zn2+(1.0 M) || Cu2+(0.1 M) Cu 1.067 3. ZnZn2+(0.1 M) || Cu2+(1.0 M) | Cu 4. Zn | Zn2+(1.0 M) || Pb2+(1.0 M) | Pb 5. ZnZn2(1.0M) || Pb2+(0.1 M) | Pb 0.600 6. Zn | Zn2+(0.1 M) || Pb2+(1.0 M) I Pb 0.644 7. ZnZn2+(1.0 M)...
Calculate the theoretical cell potential for each of the following cells. Is the cell, as written, galvanic or electrolytic? a. Pb | PbSO_4 (sat'd), SO_4^2- (0.200 M) || Sn^2+ (0.150 M), Sn^4+ (0.250 M)|Pt b. Pt |Fe^3+ (0.0100M), Fe^2+ (0.00100M) || Ag^+ (0.200M), CuI (sat'd) |Cu d. Pt | UO_2^2+ (0.0100 M), U^4+ (0.0100 M), H^+ (1.00 times 10^-6 M) || AgClO (sat'd), KCI (1.00 times 10^-4 M) |Ag
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...
Data Analysis Questions Q1. Complete Table 8.2 below. Using a standard half-cell potential of 0.34 V for Cu2*/Cu, calculate the experimental reduction potentials for Mg, Pb, Sn, and Zn half-cells. Obtain standard reduction potentials from a suitable reference source. Show all of your work below and RANK the metals in terms of oxidizing and reducing ability according to the experimental half-cell potentials. (3.0) Table 8.2 Half-cell reduction reaction (include phase labels) Calculated E (v) Literature E (V) Culaq) + 2e...
how
do I solve this?
1. Use the Nernst equation to calculate the standard cell potential for a voltaic cell of a Sn electrode in 0.10M Sn2(a) in one half-cell and Al in 0.10M AP) in the other. (EPe Eaode- Emode 1.52 V, Show your work. Hint: Check E values of the reduction haif reactions. Write the one with more negative E as oxidation half reaction (change the sign); ensure that equal number of electrons are exchanged ie. electrons cancel,...
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...
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...
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...
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...
Problem Set #34: Galvanic Cells & Standard Reduction Potential Practice Sheet Directions: (a) Sketch the galvanic cell based on the following overall reaction OR half- reactions. o Show the direction of electron flow o Identify the cathode and anode (b) Give the overall balanced reaction (c) Determine the Evalues for each of the galvanic cells. (d) Give the standard line notation for each cell. (Assume that all concentrations are 1.0M and that all partial pressures are 1.0 atm) 1. 103(aq)...
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