Ch.19 - Electrochemistry

Problem 160

Chapter 19, Problem 160

The nickel–iron battery has an iron anode, an NiO(OH) cathode, and a KOH electrolyte. This battery uses the follow-ing half-reactions and has an E° value of 1.37 V at 25 °C. (b) Calculate ∆G° (in kilojoules) and the equilibrium con-stant K for the cell reaction at 25 °C.

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Identify the relationship between the standard cell potential (E°), the change in Gibbs free energy (∆G°), and the equilibrium constant (K). The relevant equations are: ∆G° = -nFE° and ∆G° = -RTlnK.

Determine the number of moles of electrons (n) transferred in the balanced overall cell reaction. This requires writing and balancing the half-reactions for the nickel–iron battery.

Use the equation ∆G° = -nFE° to calculate ∆G°, where F is the Faraday constant (approximately 96485 C/mol). Substitute the known values of n, F, and E° (1.37 V) into the equation.

Use the calculated ∆G° value in the equation ∆G° = -RTlnK to solve for the equilibrium constant K. Here, R is the universal gas constant (8.314 J/mol·K) and T is the temperature in Kelvin (25 °C = 298 K).

Rearrange the equation to solve for K: K = e^(-∆G°/RT). Substitute the values of ∆G°, R, and T to find the equilibrium constant K.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Gibbs Free Energy (∆G°)

Gibbs Free Energy (∆G°) is a thermodynamic potential that measures the maximum reversible work obtainable from a thermodynamic system at constant temperature and pressure. It is calculated using the equation ∆G° = -nFE°, where n is the number of moles of electrons transferred, F is the Faraday constant, and E° is the standard cell potential. A negative ∆G° indicates a spontaneous reaction.

Standard Cell Potential (E°)

The standard cell potential (E°) is the measure of the voltage produced by an electrochemical cell under standard conditions (1 M concentration, 1 atm pressure, and 25 °C). It is determined by the difference in reduction potentials of the cathode and anode. A higher E° value indicates a greater tendency for the cell reaction to occur spontaneously.

Equilibrium Constant (K)

The equilibrium constant (K) is a dimensionless value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given reaction. It can be related to Gibbs Free Energy by the equation ∆G° = -RT ln(K), where R is the universal gas constant and T is the temperature in Kelvin. A larger K value indicates a reaction that favors product formation at equilibrium.

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Related Practice

Textbook Question

A concentration cell has the same half-reactions at the anode and cathode, but a voltage results from different concentrations in the two electrode compartments. (b) A similar cell has 0.10 M Cu2+ in both compartments. When a stoichiometric amount of ethylenediamine (NH2CH2CH2NH2) is added to one compartment, the measured cell potential is 0.179 V. Calculate the formation constant Kf for the complex ion Cu(NH2CH2CH2CH2)22+. Assume there is no volume change.

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Textbook Question

Consider the redox titration (Section 4.13) of 120.0 mL of 0.100 M FeSO4 with 0.120 M K2Cr2O7 at 25 °C, assuming that the pH of the solution is maintained at 2.00 with a suitable buffer. The solution is in contact with a platinum electrode and constitutes one half-cell of an electrochemical cell. The other half-cell is a standard hydrogen electrode. The two half-cells are connected with a wire and a salt bridge, and the progress of the titration is monitored by measuring the cell potential with a voltmeter. (a) Write a balanced net ionic equation for the titration reaction, assuming that the products are Fe3+ and Cr3+.

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Textbook Question

Consider a galvanic cell that utilizes the following half-reactions:

(b) What are the values of E° and the equilibrium constant K for the cell reaction at 25 °C?

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Textbook Question

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Textbook Question

Experimental solid-oxide fuel cells that use butane (C₄H₁₀) as the fuel have been reported recently. These cells contain composite metal/metal oxide electrodes and a solid metal oxide electrolyte. The cell half-reactions are (c) How many grams of butane are required to produce a constant current of 10.5 A for 8.00 h? How many liters of gaseous butane at 20 °C and 815 mm Hg pressure are required?

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Textbook Question

The half-reactions that occur in ordinary alkaline batteries can be written as In 1999, researchers in Israel reported a new type of alkaline battery, called a 'super-iron' battery. This battery uses the same anode reaction as an ordinary alkaline battery but involves the reduction of FeO₄^2- ion (from K₂FeO₄) to solid Fe(OH)₃ at the cathode. (a) Use the following standard reduction potential and any data from Appendixes C and D to calculate the standard cell potential expected for an ordinary alkaline battery:

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