Ch. 5 - Chemical Reaction Analysis: Thermodynamics and Kinetics

Mullins - Organic Chemistry: A Learner Centered Approach 1st Edition

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Mullins 1st Edition

Ch. 5 - Chemical Reaction Analysis: Thermodynamics and Kinetics

Problem 24e

Chapter 4, Problem 24e

For the following acid–base reaction, (e) calculate ∆G° at 273 K.

Verified step by step guidance

Step 1: Identify the acid and base in the reaction. Determine the conjugate acid and conjugate base formed after the reaction. This will help in understanding the equilibrium of the reaction.

Step 2: Use the pKa values of the acid and conjugate acid to calculate the equilibrium constant (K). The relationship between pKa and K is given by \( K = 10^{\Delta pKa} \), where \( \Delta pKa = pKa_{acid} - pKa_{conjugate\ acid} \).

Step 3: Recall the relationship between the Gibbs free energy change (\( \Delta G^\circ \)) and the equilibrium constant (K). The formula is \( \Delta G^\circ = -RT \ln K \), where \( R \) is the gas constant (8.314 J/mol·K) and \( T \) is the temperature in Kelvin.

Step 4: Substitute the values for \( R \), \( T \), and \( K \) into the formula \( \Delta G^\circ = -RT \ln K \). Ensure that the temperature is given as 273 K and calculate \( \ln K \) using the equilibrium constant derived from \( \Delta pKa \).

Step 5: Perform the calculation to determine \( \Delta G^\circ \). Ensure units are consistent throughout the calculation (e.g., J/mol or kJ/mol). This will yield the Gibbs free energy change for the reaction at 273 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 a crucial concept in predicting the spontaneity of a reaction; a negative ∆G° indicates that a reaction can occur spontaneously, while a positive value suggests non-spontaneity.

Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H⁺ ions) between reactants. In these reactions, acids donate protons, while bases accept them. Understanding the strength of acids and bases, as well as their dissociation constants (Ka and Kb), is essential for calculating the equilibrium position and the Gibbs Free Energy change associated with the reaction.

Temperature and Reaction Quotient

Temperature plays a significant role in determining the Gibbs Free Energy of a reaction. The reaction quotient (Q) reflects the ratio of the concentrations of products to reactants at any point in time. At equilibrium, the relationship between Gibbs Free Energy, temperature, and the reaction quotient can be expressed using the equation ∆G° = ∆H° - T∆S°, where ∆H° is the change in enthalpy and ∆S° is the change in entropy.

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Related Practice

Textbook Question

Calculate ∆G°, ∆H°, and ∆S° for the following acid–base reactions. Rationalize the value of ∆H° based on the structure of the conjugate bases. [Assume T = 298 K.]

(b)

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Textbook Question

For the following acid–base reaction, (f) calculate ∆G° at 373 K.

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Textbook Question

Calculate ∆G°, ∆H°, and ∆S° for the following acid–base reactions. Rationalize the value of ∆H° based on the structure of the conjugate bases. [Assume T = 298 K.]

(a)

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Textbook Question

For the following acid–base reaction, (b) calculate the equilibrium constant.

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Textbook Question

For the following acid–base reaction, (c) calculate the ratio of butan-2-ol to 2-butoxide.

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Textbook Question

For the following acid–base reaction, (d) calculate ∆G° at 298 K.

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