   Chapter 18, Problem 43PS

Chapter
Section
Textbook Problem

The ionization constant, Ka, for acetic acid is 1.8 × 10−5 at 25 °C. What is the value of ΔrG° for this reaction? Is this reaction product- or reactant-favored at equilibrium?

Interpretation Introduction

Interpretation:

The value of ΔrG for the given process should be calculated.

Concept introduction:

The Gibbs free energy or the free energy change is a thermodynamic quantity represented by ΔrG. It is related to the equilibrium constant K by the equation,

ΔrG=RTlnK.

Explanation

The ΔrG value for the ionization of acetic acid is calculated below.

Given:

For the reaction of ionization of acetic acid the value of equilibrium constant K is 1.8×105

at 25 C.

Now, The Gibbs free energy is related to the equilibrium constant K by the equation,

ΔrG=RTlnK

Substitute the value of K, T and R

Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started 