20. Electrochemistry

Cell Potential: The Nernst Equation

객관식
Using the Nernst equation, calculate the concentration of Cu^2+ ions given the cell potential is 0.5540 V and the standard cell potential is 0.4260 V. The equation is: 0.5540 V = 0.4260 V - (0.0592/2) log ([Cu^2+]/[1]^2). What is the concentration of Cu^2+?
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객관식
Calculate the ΔE°cell for the following concentration cell: Cu(s) | Cu2+(aq, 0.049M) || Cu2+(aq, 0.231M) | Cu(s). Cu2+(aq) + 2e- → Cu(s), E° = 0.340V.
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객관식
Determine [Fe²⁺] for the following galvanic cell at 25ºC if given [Sn²⁺] = 0.072 M, [Fe³⁺] = 0.0219 M, and [Sn⁴⁺] = 0.00345 M.
Sn²⁺ (aq) + 2 Fe³⁺ (aq) ⇌. Sn⁴⁺ (aq) + 2 Fe²⁺ (aq) E_cell = + 0.68 V
Standard Reduction Potentials
Sn⁴⁺(aq) + 2 e^– →. Sn²⁺(aq) E°_red = + 0.151 V
Fe³⁺(aq) + e^– → Fe²⁺(aq) E°_red = + 0.771 V
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객관식
If [Br^–] = 0.010 M and [Al³⁺] = 0.022 M, predict whether the following reaction would proceed spontaneously as written at 25ºC:
Al (s) + Br₂ (l) ⇌ Al³⁺ (aq) + Br^– (aq)
Standard Reduction Potentials
Al³⁺(aq) + 3 e^– → Al (s) E°_red = –1.66 V
Br₂ (l) + 2 e^– → 2 Br^– (aq) E°_red = +1.09 V
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객관식
How do you calculate the electrode potential under nonstandard conditions using the Nernst equation?
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객관식
What is the change in the cell voltage when the ion concentrations in the cathode half-cell are increased by a factor of 10, according to the Nernst Equation?
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객관식
A voltaic cell is constructed with two Zn2+-Zn electrodes, where the half-reaction is Zn2+ + 2e- → Zn(s) with E° = -0.763 V. The concentrations of zinc ion in the two compartments are 5.50 M and 1.11 × 10^-2 M, respectively. What is the cell emf in volts?
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객관식
What is the emf of this cell when [Fe²⁺] = 1.5 M, [Fe³⁺] = 1.4 × 10⁻² M, P(O₂) = 0.56 atm, and the pH of the solution in the cathode compartment is 3.5, given that the standard cell potential (E°) is 1.23 V?
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객관식
Calculate the cell potential at 25°C for a galvanic cell with the following reaction: Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s), given that the concentrations are [Zn²⁺] = 0.010 M and [Cu²⁺] = 1.0 M. The standard cell potential (E°) is 1.10 V.
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미해결 질문
______________________ accelerates the rusting process.
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객관식
Using the Nernst equation, what is the concentration of Ag+ in the cathode half-cell if the cell potential is measured to be 0.70 V?
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객관식
Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: Cu(s) | Cu2+(aq, 3.2×10^(-3) mol L^-1) || Cu2+(aq, 4.48 mol L^-1) | Cu(s). Given E°(Cu2+/Cu) = +0.34 V, express your answer to two significant figures.
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객관식
At 25°C, E° = +1.88 V for a cell based on the reaction 3 AgCl(s) + Al(s) → 3 Ag(s) + Al³⁺(aq) + 3 Cl⁻(aq). Find the cell potential E if [Al³⁺] = 0.20 M and [Cl⁻] = 0.010 M using the Nernst equation.
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