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7.46 The electromotive force of the cell Cd | CdCl2 2 H2O, sat. solution | AgCi...
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 –...
The standard electromotive force of the cell Pt/H2(g)/HC/// AgCl(s)/Ag has been determined from 0 - 90...
The standard electromotive force of the cell Pt/H2(g)/HC/// AgCl(s)/Ag has been determined from 0 - 90 °C. The potential in volts as function of temperature in °C is represented by the following linear equation (F = 96485 C/ mol) E°(T) = 0.24-3.9x10-4 T Determine AS° at 25° for 12 H2 (g) + AgCl(s) + HCl(aq) + Ag(s) Select one: a. 27.5 J/mol K b. -47.5 J/mol.k c. 47.6 J/mol K d. 37. e. -37. Ashwaq sent a photo
The standard electromotive force of the cell Pt/H2(g)/HC/// AgCl(s)/Ag has been determined from 0 to 90...
The standard electromotive force of the cell Pt/H2(g)/HC/// AgCl(s)/Ag has been determined from 0 to 90 °C. The potential in volts as function of temperature in °C is represented by the following linear equation (F = 96485 C/ mol) E°(T) = 0.24-3.9x10-4 T Determine AG° at 25° for 12 H2 (g) + AgCl(s) – HCl(aq) + Ag(s) Select one: a.-23.2 kJ/mol b. 21.2 kJ/mol C.-22.2 kJ/mol d. 23.2 kJ/mol e. 22.2 kJ/mol
Corrosion Problem: Electrode Electrode Pb (s) PbCh (s) HCl (aqueous) AgCI (s)Ag (s) The emf of...
Corrosion Problem: Electrode Electrode Pb (s) PbCh (s) HCl (aqueous) AgCI (s)Ag (s) The emf of the cell represented in the accompanying diagram is 0.490 V at 25°C and the temperature coefficient is-1.84 × 10-4 VpC. All the compo- nents are present as pure solids in contact with an HCl electrolyte. (a) Write the half-cell reactions. (b) Write the overall cell reaction (c) Calculate the Gibbs free energy change and the entropy change for this reaction.
Electrochemistry - Equilibrium 1. The electrochemical cell described by the balanced chemical equation has a standard...
Electrochemistry - Equilibrium 1. The electrochemical cell described by the balanced chemical equation has a standard emf (electromotive force) of -0.08 V. Calculate the value (J) for the Wmax that the cell can do under standard conditions. Round your answer to 3 significant figures. St. Red. Pot. (V) Faraday's Constant Hg2+/Hg +0.85 F = 96485 C Fe3+/Fe2+ +0.77 2Fe3+(aq) + Hg(l) → 2Fe2+(aq) + Hg2+(aq) 2. The voltaic cell described by the balanced chemical equation has a standard emf of...
please help, thanks! 7. What is the correct cell notation for the reaction below? Cd(aq)+Ni(s)-Cd(s)+ Ni(aq)...
please help, thanks!
7. What is the correct cell notation for the reaction below? Cd(aq)+Ni(s)-Cd(s)+ Ni(aq) a. Cd Cd| Ni | Ni d. Ni Cd I N | Ca b. Cd CdNi | Ni e. Cd |Cd Ni Ni 8. Calculate AS for the dissociation of dinitrogen tetraoxi de at 25°C NOdg) 2NO:(g) AG, J/mol)AH, J/mol) Substance NO) NOdg) +33.2 +51.3 +97.9 +9.2 d. +0.076 kJ K a.-2.10 kJ/K e +2.10kJ/K b. -0.550 kJ/K c.-0.208 kJ/K 9. Use the standard...
Consider the voltaic cell at 25 °C 21. Zn(s) | Zn2 (aq, 1.0 x 10 2...
Consider the voltaic cell at 25 °C 21. Zn(s) | Zn2 (aq, 1.0 x 10 2 mol L-1) I Ce (ag, 1.0 mol L-1), Ce (aq, 1.0 x 102 mol L-') | Pt(s) in which the compartments have equal volume. What is the electromotive force of the cell when the circuit is closed and the reaction has advanced to the point that [Ce3]-0.2 mol L12 A) 2.48 V B) 2.43 V C) 1.24 v D) 2.54 V E) 0.957 V
Consider a cell based on the following reaction: GeO(s) + H2O(l) + 2 Ag+(aq) → GeO2(s)...
Consider a cell based on the following reaction: GeO(s) + H2O(l) + 2 Ag+(aq) → GeO2(s) + 2 H+(aq) + 2 Ag(s) If [Ag+] = 1 M, at 25°C pH = (E - E°)/0.0592 V. pH = 2(E - E°)/0.0592 V. pH = 2(E° - E)/0.0592 V. pH = (E° - E)/0.0592 V.
4.In a electrochemical cell consisting of a silver electrode in a solution of AgNO3 and a...
4.In a electrochemical cell consisting of a silver electrode in a solution of AgNO3 and a gold electrode in a solution of Au(NO3)3 at standard conditions, the correct cell potential is 0.70 V b. 2.30 V 0.90 V d. -0.90 V 5. Predict which of the following reactions would exhibit an increase in entropy based on the nature of the reactants and products. 2H2(g) + O2(g) → 2H2O(g) 2NO2(g) → N2O4(g) H+(aq) + F-(aq) → HF(aq) BaF2(s) → Ba2+(aq) +...
NUEL UILCO CHM 112 Lab Analysis 1 CHE [References Use the References to access important values...
NUEL UILCO CHM 112 Lab Analysis 1 CHE [References Use the References to access important values if needed for this question. Enter electrons as c Use smallest possible integer coefficients. If a box is not needed, leave it blank. A voltaic cell is constructed from a standard Co2"Co half cell (Erod - -0.280V) and a standard APAl half cell (Ered -- 1.660V). The anode reaction is: + The cathode reaction is: + + The spontaneous cell reaction is: + The...
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 –...
The standard electromotive force of the cell Pt/H2(g)/HC/// AgCl(s)/Ag has been determined from 0 - 90 °C. The potential in volts as function of temperature in °C is represented by the following linear equation (F = 96485 C/ mol) E°(T) = 0.24-3.9x10-4 T Determine AS° at 25° for 12 H2 (g) + AgCl(s) + HCl(aq) + Ag(s) Select one: a. 27.5 J/mol K b. -47.5 J/mol.k c. 47.6 J/mol K d. 37. e. -37. Ashwaq sent a photo
The standard electromotive force of the cell Pt/H2(g)/HC/// AgCl(s)/Ag has been determined from 0 to 90 °C. The potential in volts as function of temperature in °C is represented by the following linear equation (F = 96485 C/ mol) E°(T) = 0.24-3.9x10-4 T Determine AG° at 25° for 12 H2 (g) + AgCl(s) – HCl(aq) + Ag(s) Select one: a.-23.2 kJ/mol b. 21.2 kJ/mol C.-22.2 kJ/mol d. 23.2 kJ/mol e. 22.2 kJ/mol
Corrosion Problem: Electrode Electrode Pb (s) PbCh (s) HCl (aqueous) AgCI (s)Ag (s) The emf of the cell represented in the accompanying diagram is 0.490 V at 25°C and the temperature coefficient is-1.84 × 10-4 VpC. All the compo- nents are present as pure solids in contact with an HCl electrolyte. (a) Write the half-cell reactions. (b) Write the overall cell reaction (c) Calculate the Gibbs free energy change and the entropy change for this reaction.
please help, thanks!
7. What is the correct cell notation for the reaction below? Cd(aq)+Ni(s)-Cd(s)+ Ni(aq) a. Cd Cd| Ni | Ni d. Ni Cd I N | Ca b. Cd CdNi | Ni e. Cd |Cd Ni Ni 8. Calculate AS for the dissociation of dinitrogen tetraoxi de at 25°C NOdg) 2NO:(g) AG, J/mol)AH, J/mol) Substance NO) NOdg) +33.2 +51.3 +97.9 +9.2 d. +0.076 kJ K a.-2.10 kJ/K e +2.10kJ/K b. -0.550 kJ/K c.-0.208 kJ/K 9. Use the standard...
Consider the voltaic cell at 25 °C 21. Zn(s) | Zn2 (aq, 1.0 x 10 2 mol L-1) I Ce (ag, 1.0 mol L-1), Ce (aq, 1.0 x 102 mol L-') | Pt(s) in which the compartments have equal volume. What is the electromotive force of the cell when the circuit is closed and the reaction has advanced to the point that [Ce3]-0.2 mol L12 A) 2.48 V B) 2.43 V C) 1.24 v D) 2.54 V E) 0.957 V
NUEL UILCO CHM 112 Lab Analysis 1 CHE [References Use the References to access important values if needed for this question. Enter electrons as c Use smallest possible integer coefficients. If a box is not needed, leave it blank. A voltaic cell is constructed from a standard Co2"Co half cell (Erod - -0.280V) and a standard APAl half cell (Ered -- 1.660V). The anode reaction is: + The cathode reaction is: + + The spontaneous cell reaction is: + The...
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