Ch.20 - Electrochemistry

Tro - Chemistry: A Molecular Approach 5th Edition

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Tro 5th Edition

Ch.20 - Electrochemistry

Problema 77c

Capitolo 20, Problema 77c

A voltaic cell consists of a Zn/Zn²⁺ half-cell and a Ni/Ni²⁺ half-cell at 25 °C. The initial concentrations of Ni²⁺ and Zn²⁺ are 1.50 M and 0.100 M, respectively. c. What are the concentrations of Ni²⁺ and Zn²⁺ when the cell potential falls to 0.45 V?

Guida verificata passo dopo passo

Identify the half-reactions for the voltaic cell: Zn -> Zn^{2+} + 2e^- and Ni^{2+} + 2e^- -> Ni.

Write the Nernst equation for the cell: E = E^0 - (RT/nF) * ln(Q), where Q is the reaction quotient.

Calculate the standard cell potential (E^0) using standard reduction potentials: E^0 = E^0_{cathode} - E^0_{anode}.

Set up the expression for the reaction quotient Q: Q = [Zn^{2+}]/[Ni^{2+}].

Substitute the given cell potential (0.45 V) and solve the Nernst equation for the concentrations of Ni^{2+} and Zn^{2+}.

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Electrochemical Cells

Electrochemical cells, such as voltaic cells, convert chemical energy into electrical energy through redox reactions. In a voltaic cell, oxidation occurs at the anode (where Zn is oxidized to Zn2+) and reduction occurs at the cathode (where Ni2+ is reduced to Ni). Understanding the flow of electrons and the role of each half-cell is crucial for analyzing cell behavior and potential.

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02:46

Electrochemical Cells

Nernst Equation

The Nernst equation relates the cell potential to the concentrations of the reactants and products in a redox reaction. It is expressed as E = E° - (RT/nF) ln(Q), where E° is the standard cell potential, R is the gas constant, T is the temperature in Kelvin, n is the number of moles of electrons transferred, F is Faraday's constant, and Q is the reaction quotient. This equation is essential for calculating the cell potential at non-standard conditions.

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01:17

The Nernst Equation

Reaction Quotient (Q)

The reaction quotient (Q) is a measure of the relative concentrations of products and reactants at any point in a reaction. For the voltaic cell in question, Q is calculated using the concentrations of Zn2+ and Ni2+ ions. As the reaction proceeds, the concentrations change, affecting Q and consequently the cell potential, which is critical for determining the concentrations when the potential drops to a specific value.

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00:49

Reaction Quotient Q

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An electrochemical cell is based on these two half-reactions:

Ox: Sn(s) → Sn²⁺(aq, 2.00 M) + 2 e^–

Red: ClO₂(g, 0.100 atm) + e^– → ClO₂^–(aq, 2.00 M)

Calculate the cell potential at 25 °C.

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A voltaic cell consists of a Pb/Pb²⁺ half-cell and a Cu/Cu²⁺ half-cell at 25°C. The initial concentrations of Pb²⁺ and Cu²⁺ are 0.0500 M and 1.50 M, respectively. b. What is the cell potential when the concentration of Cu²⁺ has fallen to 0.200 M?

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A voltaic cell consists of a Zn/Zn²⁺ half-cell and a Ni/Ni²⁺ half-cell at 25 °C. The initial concentrations of Ni²⁺ and Zn²⁺ are 1.50 M and 0.100 M, respectively. b. What is the cell potential when the concentration of Ni²⁺ has fallen to 0.500 M?

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A voltaic cell consists of a Pb/Pb²⁺ half-cell and a Cu/Cu²⁺ half-cell at 25°C. The initial concentrations of Pb²⁺ and Cu²⁺ are 0.0500 M and 1.50 M, respectively. a. What is the initial cell potential?

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A voltaic cell consists of a Pb/Pb²⁺ half-cell and a Cu/Cu²⁺ half-cell at 25°C. The initial concentrations of Pb²⁺ and Cu²⁺ are 0.0500 M and 1.50 M, respectively. c. What are the concentrations of Pb²⁺ and Cu²⁺ when the cell potential falls to 0.35 V?

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A voltaic cell consists of a Zn/Zn²⁺ half-cell and a Ni/Ni²⁺ half-cell at 25 °C. The initial concentrations of Ni²⁺ and Zn²⁺ are 1.50 M and 0.100 M, respectively. a. What is the initial cell potential?

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A voltaic cell consists of a Zn/Zn2+ half-cell and a Ni/Ni2+ half-cell at 25 °C. The initial concentrations of Ni2+ and Zn2+ are 1.50 M and 0.100 M, respectively. c. What are the concentrations of Ni2+ and Zn2+ when the cell potential falls to 0.45 V?

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Concetti chiave

Electrochemical Cells

Nernst Equation

Reaction Quotient (Q)

A voltaic cell consists of a Zn/Zn²⁺ half-cell and a Ni/Ni²⁺ half-cell at 25 °C. The initial concentrations of Ni²⁺ and Zn²⁺ are 1.50 M and 0.100 M, respectively. c. What are the concentrations of Ni²⁺ and Zn²⁺ when the cell potential falls to 0.45 V?