Ch.19 - Electrochemistry

McMurry8th EditionChemistryISBN: 9781292336145당신이 사용하는 게 아니라요?교과서 변경

McMurry 8th Edition

Ch.19 - Electrochemistry

문제 97

19장, 문제 97

A galvanic cell has an iron electrode in contact with 0.10 M FeSO4 and a copper electrode in contact with a CuSO4 solu-tion. If the measured cell potential at 25 °C is 0.67 V, what is the concentration of Cu2+ in the CuSO4 solution?

검증된 단계별 안내

Identify the half-reactions for the galvanic cell: Fe(s) \(\rightarrow\) Fe^{2+}(aq) + 2e^- and Cu^{2+}(aq) + 2e^- \(\rightarrow\) Cu(s).

Write the overall cell reaction by combining the half-reactions: Fe(s) + Cu^{2+}(aq) \(\rightarrow\) Fe^{2+}(aq) + Cu(s).

Use the Nernst equation to relate the cell potential to the concentrations: E_{cell} = E^\(\circ\)_{cell} - \(\frac{RT}{nF}\) \(\ln\) Q, where Q is the reaction quotient.

Calculate the standard cell potential, E^\(\circ\)_{cell}, using standard reduction potentials: E^\(\circ\)_{cell} = E^\(\circ\)_{Cu^{2+}/Cu} - E^\(\circ\)_{Fe^{2+}/Fe}.

Solve for the concentration of Cu^{2+} using the Nernst equation and the given cell potential, 0.67 V, by substituting known values and solving for the unknown concentration.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

주요 개념

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

Galvanic Cell

A galvanic cell is an electrochemical cell that converts chemical energy into electrical energy through spontaneous redox reactions. It consists of two electrodes, an anode and a cathode, immersed in electrolyte solutions. 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.

Nernst Equation

The Nernst equation relates the cell potential to the concentrations of the reactants and products in an electrochemical 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 allows for the calculation of cell potential under non-standard conditions.

Reaction Quotient (Q)

The reaction quotient (Q) is a measure of the relative concentrations of reactants and products in a chemical reaction at a given moment. It is calculated using the formula Q = [products]/[reactants], where the concentrations are raised to the power of their coefficients in the balanced equation. In the context of a galvanic cell, Q helps determine the direction of the reaction and the cell potential, especially when concentrations deviate from standard conditions.

관련 실천

교과서 질문

Consider a galvanic cell that uses the reaction Calculate the potential at 25 °C for a cell that has the following ion concentrations: [Ag+] = 0.010M, [Ni2+] = 0.100M.

1227

views

교과서 질문

Given the following half-reactions and E° values, write a balanced equation for the formation of Mn2+ and MnO2 from Mn3+, and calculate the value of E° for this reaction. Is the reaction spontaneous under standard-state conditions?

1214

views

교과서 질문

The Nernst equation applies to both cell reactions and half-reactions. For the conditions specified, calculate the potential for the following half-reactions at 25 °C. (b)

Consider a galvanic cell that uses the following half-reactions: (b) What is the oxidizing agent, and what is the reducing agent?.

872

views

교과서 질문

What is the Fe2+: Sn2+ concentration ratio in the following cell at 25 °C if the measured cell potential is 0.35 V?

612

views

교과서 질문

When suspected drunk drivers are tested with a Breathalyzer, the alcohol (ethanol) in the exhaled breath is oxidized to acetic acid with an acidic solution of potassium dichromate: The color of the solution changes because some of the orange Cr₂O₇^2-is converted to the green Cr³⁺ The Breathalyzer measures the color change and produces a meter reading calibrated in blood alcohol content. (a) What is E° for the reaction if the standard half-cell potential for the reduction of acetic acid to ethanol is 0.058 V?

801

views