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a) Build a schematic diagram of an electrochemical cell
b) Calculate...
The following figure represents an electrochemical cell at 25.00C with aqueous solutions that behave ideally: electro...
The following figure represents an electrochemical cell at
25.00C with aqueous solutions that behave ideally:
electro sal bridge incions surate ions copper electrode coccer 0p ne sulfate wade dation + cathode reduction 1 and 0.20 M, respectively. (a) Represent the electrochemical cell using cell notation, taking into account that concentrations of the ZnSO4 and CuSO4 solutions are 0.15 M and 0.20 M, respectively. (b) Calculate the standard potential of the cell, E'cell. (c) Calculate the potential of the cell, E...
6. Consider the following electrochemical cell: Write electrode half-reactions and the cell reaction. Determine the standard...
6. Consider the following electrochemical cell: Write electrode half-reactions and the cell reaction. Determine the standard emf E for this cell from standard potential data in the Data Section of your textbook. Calculate the standard Gibbs energy and the equilibrium constant for the cell reaction at 25°C. Write the Nernst equation for the cell and calculate its emf E given that the pressure of H:(g) p = 1 bar, the molality of HCI(aq) b = 0.01 mol kg.. and the...
1) Calculate the cell potential, E°cell, for the following electrochemical reaction. Cu(s) + I2(g) → Cu+2(aq)...
1) Calculate the cell potential, E°cell, for the following electrochemical reaction. Cu(s) + I2(g) → Cu+2(aq) + 2I-1(aq) E = ? a.-0.87 V b.-0.19 V c.0.19 V d.0.87 V 2) Calculate the equilibrium constant (Keq) for the following reaction at 25 °C? (Faraday's Constant = 96,500 J / V · mol) & (R = 8.314 J / mol · K) 2Fe+3(aq) + Sn+2(aq) → 2Fe+2(aq) + Sn+4(aq) K = ? a. 4.04 x 107 b. 3.44 x 1018 c. 4.48...
An electrochemical cell was designed in order to determine the solubility product constant, Ksp for PbCO2....
An electrochemical cell was designed in order to determine the solubility product constant, Ksp for PbCO2. The cell uses the half reactions shown below to produce the overall dissociation reaction. cathode reaction: anode reaction: overall reaction: PbCO2 (s) + 2e → Pb(s) + CO - (aq) Pb(s) + Pb2+ (aq) + 2 e- PbCO3(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...
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,?...
4) Using the information in the electrochemical cell diagram below, calculate the Kup of Ni(OH)2(s). Note...
4) Using the information in the electrochemical cell diagram below, calculate the Kup of Ni(OH)2(s). Note that the voltage listed is the voltage measured for the cell in its current state. e flew 0.17 V Ni(s) Ni(s) 10 M Ni solution agar plug (salt bridge) pH 10.00 Ni(OH)2(s)
An Ag-Cd electrochemical cell is written as Cd (s) CdCl2 (0.010 M) || AgCl (s) CI-...
An Ag-Cd electrochemical cell is written as Cd (s) CdCl2 (0.010 M) || AgCl (s) CI- (0.50 M) | Ag E°Cd2+/Ca = 0.403 V and EºACIJAg = 0.222 V 1. Write the half-cell reactions at anode and at cathode. 2. Which is oxidant and which is reductant? 3. Calculate the half-cell potentials at both anode and cathode. 4. Calculate the cell potential. 5. Write the whole-cell reaction. 6. Calculate the equilibrium constant for the whole-cell reaction. For the half –...
An electrochemical cell is expressed as Cu(s) | Cu^2+ (0.20 M) || I^- (0.10 M) |...
An electrochemical cell is expressed as Cu(s) | Cu^2+ (0.20 M) || I^- (0.10 M) | I_3^- (0.20 M) | Pt. I_3^- + 2e^- rightarrow 3I^-, E^0 = 0.535 V Cu^2+ + 2e^- rightarrow Cu(s) E^0 = 0.339 V Please answer the following questions: a. Write half-cell reactions at anode and at cathode. b. Write whole-cell reaction. c. Calculate the potential/voltage of the cell. d. Calculate equilibrium constant for this whole-cell reaction.
8. Consider the following electrochemical cell: Cd Cd? (0.20 M) // H (0.05 M), H2 (1...
8. Consider the following electrochemical cell: Cd Cd? (0.20 M) // H (0.05 M), H2 (1 atm) /Pt Given the following standard reduction potentials: Reaction 2 H+ (aq) + 2 Cd + (aq) + 2e H2 (aq) Cd (s) Eº (volts) 0.00 -0.40 (a) Write the equation for the overall cell reaction. (b) Calculate E' for the overall reaction. (c) Calculate the equilibrium constant for the overall reaction. (d) Calculate the actual value of E for the cell at the...
3. Consider the following electrochemical cell. Standard reduction potentials are given on the next page. Tl(s)...
3. Consider the following electrochemical cell. Standard reduction potentials are given on the next page. Tl(s) | Tl+(aq, 0.50 mol L−1) || H+(aq, x mol L−1) | H2(g, 1 atm) | Pt(s) The concentration of H+ is unknown and the pressure of H2 is kept constant at 1 atm. The cell voltage is initially measured as 0.139 V, with the Pt | H2 | H+ half-cell acting as the cathode. (a) (6 marks) Write out the oxidation and reduction half...
The following figure represents an electrochemical cell at
25.00C with aqueous solutions that behave ideally:
electro sal bridge incions surate ions copper electrode coccer 0p ne sulfate wade dation + cathode reduction 1 and 0.20 M, respectively. (a) Represent the electrochemical cell using cell notation, taking into account that concentrations of the ZnSO4 and CuSO4 solutions are 0.15 M and 0.20 M, respectively. (b) Calculate the standard potential of the cell, E'cell. (c) Calculate the potential of the cell, E...
6. Consider the following electrochemical cell: Write electrode half-reactions and the cell reaction. Determine the standard emf E for this cell from standard potential data in the Data Section of your textbook. Calculate the standard Gibbs energy and the equilibrium constant for the cell reaction at 25°C. Write the Nernst equation for the cell and calculate its emf E given that the pressure of H:(g) p = 1 bar, the molality of HCI(aq) b = 0.01 mol kg.. and the...
An electrochemical cell was designed in order to determine the solubility product constant, Ksp for PbCO2. The cell uses the half reactions shown below to produce the overall dissociation reaction. cathode reaction: anode reaction: overall reaction: PbCO2 (s) + 2e → Pb(s) + CO - (aq) Pb(s) + Pb2+ (aq) + 2 e- PbCO3(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...
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,?...
4) Using the information in the electrochemical cell diagram below, calculate the Kup of Ni(OH)2(s). Note that the voltage listed is the voltage measured for the cell in its current state. e flew 0.17 V Ni(s) Ni(s) 10 M Ni solution agar plug (salt bridge) pH 10.00 Ni(OH)2(s)
An Ag-Cd electrochemical cell is written as Cd (s) CdCl2 (0.010 M) || AgCl (s) CI- (0.50 M) | Ag E°Cd2+/Ca = 0.403 V and EºACIJAg = 0.222 V 1. Write the half-cell reactions at anode and at cathode. 2. Which is oxidant and which is reductant? 3. Calculate the half-cell potentials at both anode and cathode. 4. Calculate the cell potential. 5. Write the whole-cell reaction. 6. Calculate the equilibrium constant for the whole-cell reaction. For the half –...
An electrochemical cell is expressed as Cu(s) | Cu^2+ (0.20 M) || I^- (0.10 M) | I_3^- (0.20 M) | Pt. I_3^- + 2e^- rightarrow 3I^-, E^0 = 0.535 V Cu^2+ + 2e^- rightarrow Cu(s) E^0 = 0.339 V Please answer the following questions: a. Write half-cell reactions at anode and at cathode. b. Write whole-cell reaction. c. Calculate the potential/voltage of the cell. d. Calculate equilibrium constant for this whole-cell reaction.
8. Consider the following electrochemical cell: Cd Cd? (0.20 M) // H (0.05 M), H2 (1 atm) /Pt Given the following standard reduction potentials: Reaction 2 H+ (aq) + 2 Cd + (aq) + 2e H2 (aq) Cd (s) Eº (volts) 0.00 -0.40 (a) Write the equation for the overall cell reaction. (b) Calculate E' for the overall reaction. (c) Calculate the equilibrium constant for the overall reaction. (d) Calculate the actual value of E for the cell at the...
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