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7. Electrochemical cell potentials can be used to determine equilibrium constants that would be otherwise difficult...
Name: Chem 1120 Electrochemical Potentials Perform each of the following calculations, showing all work. Use the...
Name: Chem 1120 Electrochemical Potentials Perform each of the following calculations, showing all work. Use the Electrochemical Potentials table provided on D2L if values are not provided. Standard State Electrochemical Cells 1. In each of the following systems two half-reactions are provided. For each system, a) write the balanced reaction occurring for a spontaneous system, and b) calculate the overall standard cell potential. a. Half Reaction Zn2+(aq) + 2e = Zn(s) Cr3+ (aq) + 38 = Cr(s) Eºred (V) -0.76...
Using the information in the table: Which combination of metals, if used to create an electrochemical...
Using the information in the table:
Which combination of metals, if used to create an
electrochemical cell, would produce the largest voltage?
Liu lur the reaction between Zn and Cu2+ ions is 1.1030 V, we can use the known value for the half-cell potential for zinc to determine the half-cell potential for copper: Zn(s) → Zn2+(aq) + 2e + Cu2+(aq) + 2e → Cu(s) Zn(s) + Cu2+ (aq) → Zn2+ (aq) + Cu(s) E half-cell = 0.7628 V Eºhalf-cell =...
30) Use the tabulated half-cell potentials below to calculate the equilibrium constant (K) for the following...
30) Use the tabulated half-cell potentials below to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. Pb2+(aq) + Cu(s) → Pb(s) + Cu2+(aq) Pb2+(aq) + 2e → Pb(s) Cu2+ (aq) +2e → Cu(s) E° = -0.13 V E = 0.34 V C) 7.9 x 1015 A) 7.9 x 10-8 D) 1.3 x 10-16 B) 8.9 x 107 E) 1.1 x 10-8
19. Calculate EceLL (in V to two decimal places) for an electrochemical cell based on the...
19. Calculate EceLL (in V to two decimal places) for an electrochemical cell based on the following half-reactions at equilibrium. In addition, determine ΔG° (in kJ mol-1 to two decimal places) for the reaction under standard conditions (i.e. all concentrations are 1.0 M) and predict the magnitude of K (e.g. very small, very large, etc.) E (o)0.34 V; E red) 0 9 = 1.68 V oxidation : Cu (s) → Cu2+ (aq, .010 M) + 2e- Reductin: MnO4 (aq, 2.0...
O H20 - 2.5 QUESTION 11 Use the standard half-cell potentials listed below to calculate the...
O H20 - 2.5 QUESTION 11 Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) Mg(s) + Cu2+(aq) Cu(s) + Mg2+(aq) E --238 V E° - +0.34 V Mg2(aq) + 2e - Mg() Cu2(aq) 2e-Cus) O A -2.04 V OB.-1.36 V OC. +2.04 V D. +2.72 V E. +1.36V Click Save and Submit to save and submit. Click Save All Answers...
Scores A Review | Constants | Periodic Table e Text Standard Reduction Half-Cell Potentials at 25°C...
Scores A Review | Constants | Periodic Table e Text Standard Reduction Half-Cell Potentials at 25°C Assignments Half-Reaction Course Tools + Pb2+ (aq) + 2 H2O(l)| PbO2(s) + 4 H+ (aq) + 2 e Cl2 (9) +2 e +2 CT (aq) Pb2+ (aq) +2 e e → Pb(s) + Pb(s) E° (V) 1.46 1.36 -0.13 Part B Write a balanced equation for the overall reaction. Express your answer as a chemical equation. Identify all of the phases in your answer....
Review I Constants I Periodic Table The equilibrium constant, K, for a redox reaction is related...
Review I Constants I Periodic Table The equilibrium constant, K, for a redox reaction is related to the standard potential, E°, by the equation Standard reduction potentials nFE RT In K E° (V) Reduction half-reaction Agt(aq)eAg(s) Cu2+(aq)2eCu(s) 0.80 where n is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mol e), R (the gas constant) is equal to 8.314 J/(mol - K) , and T is the Kelvin temperature. 0.34 Sn4t (aq)4eSn(s) 0.15...
An electrochemical cell was designed in order to determine the solubility product constant, Ksp for PbCO3....
An electrochemical cell was designed in order to determine the solubility product constant, Ksp for PbCO3. The cell uses the half reactions shown below to produce the overall dissociation reaction. cathode reaction: anode reaction: overall reaction: PbCO3(s) + 2e — Pb(s) + Coz- (aq) Ph(s) — Pb2+ (aq) + 2 e- PbCO,(s) — Pb2+ (aq) + CO2 (aq) Which equality correctly represents the relationship between the equilibrium constant expression for the overall reaction and the solubility product constant for PbCO,?...
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...
Consider a voltaic (galvanic) cell with the following metal electrodes. Identify which metal is the cathode...
Consider a voltaic (galvanic) cell with the following metal electrodes. Identify which metal is the cathode and which is the anode, and calculate the cell potential. (Use the table of Standard Electrode Potentials.) (a) Ca(II) and Sc(III) Cathode: . Ca(II) Sc(III) Anode: Ca(II) Sc(III) Ecell = 0.0591 x V (b) Pb(II) and In(III) Cathode: . Pb(II) In(III) Anode: Pb(II) In(III) Ecell - (c) Ni(II) and Zr(IV) Cathode: NI(II) Zr(IV) Anode: Ni(II) Zr(IV) Ecell - V Supporting Materials Periodic Table Supplemental...
Name: Chem 1120 Electrochemical Potentials Perform each of the following calculations, showing all work. Use the Electrochemical Potentials table provided on D2L if values are not provided. Standard State Electrochemical Cells 1. In each of the following systems two half-reactions are provided. For each system, a) write the balanced reaction occurring for a spontaneous system, and b) calculate the overall standard cell potential. a. Half Reaction Zn2+(aq) + 2e = Zn(s) Cr3+ (aq) + 38 = Cr(s) Eºred (V) -0.76...
Using the information in the table:
Which combination of metals, if used to create an
electrochemical cell, would produce the largest voltage?
Liu lur the reaction between Zn and Cu2+ ions is 1.1030 V, we can use the known value for the half-cell potential for zinc to determine the half-cell potential for copper: Zn(s) → Zn2+(aq) + 2e + Cu2+(aq) + 2e → Cu(s) Zn(s) + Cu2+ (aq) → Zn2+ (aq) + Cu(s) E half-cell = 0.7628 V Eºhalf-cell =...
30) Use the tabulated half-cell potentials below to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. Pb2+(aq) + Cu(s) → Pb(s) + Cu2+(aq) Pb2+(aq) + 2e → Pb(s) Cu2+ (aq) +2e → Cu(s) E° = -0.13 V E = 0.34 V C) 7.9 x 1015 A) 7.9 x 10-8 D) 1.3 x 10-16 B) 8.9 x 107 E) 1.1 x 10-8
19. Calculate EceLL (in V to two decimal places) for an electrochemical cell based on the following half-reactions at equilibrium. In addition, determine ΔG° (in kJ mol-1 to two decimal places) for the reaction under standard conditions (i.e. all concentrations are 1.0 M) and predict the magnitude of K (e.g. very small, very large, etc.) E (o)0.34 V; E red) 0 9 = 1.68 V oxidation : Cu (s) → Cu2+ (aq, .010 M) + 2e- Reductin: MnO4 (aq, 2.0...
O H20 - 2.5 QUESTION 11 Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) Mg(s) + Cu2+(aq) Cu(s) + Mg2+(aq) E --238 V E° - +0.34 V Mg2(aq) + 2e - Mg() Cu2(aq) 2e-Cus) O A -2.04 V OB.-1.36 V OC. +2.04 V D. +2.72 V E. +1.36V Click Save and Submit to save and submit. Click Save All Answers...
Scores A Review | Constants | Periodic Table e Text Standard Reduction Half-Cell Potentials at 25°C Assignments Half-Reaction Course Tools + Pb2+ (aq) + 2 H2O(l)| PbO2(s) + 4 H+ (aq) + 2 e Cl2 (9) +2 e +2 CT (aq) Pb2+ (aq) +2 e e → Pb(s) + Pb(s) E° (V) 1.46 1.36 -0.13 Part B Write a balanced equation for the overall reaction. Express your answer as a chemical equation. Identify all of the phases in your answer....
Review I Constants I Periodic Table The equilibrium constant, K, for a redox reaction is related to the standard potential, E°, by the equation Standard reduction potentials nFE RT In K E° (V) Reduction half-reaction Agt(aq)eAg(s) Cu2+(aq)2eCu(s) 0.80 where n is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mol e), R (the gas constant) is equal to 8.314 J/(mol - K) , and T is the Kelvin temperature. 0.34 Sn4t (aq)4eSn(s) 0.15...
An electrochemical cell was designed in order to determine the solubility product constant, Ksp for PbCO3. The cell uses the half reactions shown below to produce the overall dissociation reaction. cathode reaction: anode reaction: overall reaction: PbCO3(s) + 2e — Pb(s) + Coz- (aq) Ph(s) — Pb2+ (aq) + 2 e- PbCO,(s) — Pb2+ (aq) + CO2 (aq) Which equality correctly represents the relationship between the equilibrium constant expression for the overall reaction and the solubility product constant for PbCO,?...
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...
Consider a voltaic (galvanic) cell with the following metal electrodes. Identify which metal is the cathode and which is the anode, and calculate the cell potential. (Use the table of Standard Electrode Potentials.) (a) Ca(II) and Sc(III) Cathode: . Ca(II) Sc(III) Anode: Ca(II) Sc(III) Ecell = 0.0591 x V (b) Pb(II) and In(III) Cathode: . Pb(II) In(III) Anode: Pb(II) In(III) Ecell - (c) Ni(II) and Zr(IV) Cathode: NI(II) Zr(IV) Anode: Ni(II) Zr(IV) Ecell - V Supporting Materials Periodic Table Supplemental...
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