The dissociation of acetic acid has an equilibrium constant of1.75x10-5 at 25°C. What is the value of AG° for this reaction?A. 0.268 kJ mol-1B. 27.1 kJ mol-C. 2.28 kJ mol-1D. 11.8 kJ mol-1

The dissociation of acetic acid have the following equation. CH3COOH(aq)⇔CH3COO-(aq) + H+(aq) The…

Answered: The dissociation of acetic acid has an…

The dissociation of acetic acid has an equilibrium constant of 1.75×10-5 at 25°C. What is the value of AG° for this reaction? A. 0.268 kJ mol-1 B. 27.1 kJ mol-1 C. 2.28 kJ mol-1 D. 11.8 kJ mol-1

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 100CWP

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Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

The dissociation of acetic acid has an equilibrium constant of
1.75x10-5 at 25°C. What is the value of AG° for this reaction?
A. 0.268 kJ mol-1
B. 27.1 kJ mol-
C. 2.28 kJ mol-1
D. 11.8 kJ mol-1

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