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Ch.19 - Electrochemistry
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Tro 4th EditionCh.19 - Electrochemistry문제 77a
19장, 문제 77a

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?

검증된 단계별 안내
1
Identify the half-reactions for the voltaic cell: Zn -> Zn^{2+} + 2e^- and Ni^{2+} + 2e^- -> Ni.
Look up the standard reduction potentials (E°) for each half-reaction: E°(Zn^{2+}/Zn) and E°(Ni^{2+}/Ni).
Calculate the standard cell potential (E°_{cell}) using the formula: E°_{cell} = E°(cathode) - E°(anode).
Use the Nernst equation to calculate the initial cell potential (E_{cell}): E_{cell} = E°_{cell} - (RT/nF) * ln(Q), where Q is the reaction quotient.
Substitute the given concentrations into the reaction quotient Q = [Zn^{2+}]/[Ni^{2+}] and solve for E_{cell} using the Nernst equation.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Voltaic Cell

A voltaic cell, also known as a galvanic cell, is an electrochemical cell that converts chemical energy into electrical energy through spontaneous redox reactions. It consists of two half-cells, each containing an electrode and an electrolyte. The flow of electrons from the anode to the cathode generates an electric current, and the cell potential is determined by the difference in reduction potentials of the two half-reactions.
추천 영상:
가이드 코스
01:21
The Electrolytic Cell

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 universal 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 allows for the calculation of the cell potential under non-standard conditions.
추천 영상:
가이드 코스
01:17
The Nernst Equation

Standard Reduction Potentials

Standard reduction potentials are measured voltages that indicate the tendency of a species to gain electrons and be reduced, measured under standard conditions (1 M concentration, 1 atm pressure, and 25 °C). Each half-reaction has a specific standard reduction potential, and the overall cell potential can be calculated by subtracting the anode potential from the cathode potential. These values are crucial for determining the feasibility and strength of electrochemical reactions.
추천 영상:
가이드 코스
01:10
Standard Reduction Potentials
관련 실천
교과서 질문

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

Ox: Pb(s) → Pb2+(aq, 0.10 M) + 2 e–

Red: MnO4–(aq, 1.50 M) + 4 H+(aq, 2.0 M) + 3 e– → MnO2(s) + 2 H2O(l)

Calculate the cell potential at 25 °C.

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교과서 질문

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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교과서 질문

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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교과서 질문

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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교과서 질문

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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