Question 8Given:ΔGAGO =Determine the value of the standard Gibbs free energy change for this reaction at 67.2 °C.H₂ONH4Cl(s) →kJK=NH(aq) + Cl(aq)Jwith ΔΗ° = 14.7 kJ and ASO = 75.3/1Determine the value of the equilibrium constant for this reaction at 67.2 °C.

Answered: Image /qna-images/answer/3f94eeec-9be2-4f02-bc80-2bddd4c4435a.jpg

Question 8 Given: AGO H₂O → NH(aq) + Cl(aq) kJ K = NH4Cl(s) with AH = 14.7 kJ and AS Determine the value of the standard Gibbs free energy change for this reaction at 67.2 °C. = J 75.3 K Determine the value of the equilibrium constant for this reaction at 67.2 °C.

Question 8 Given: AGO H₂O → NH(aq) + Cl(aq) kJ K = NH4Cl(s) with AH = 14.7 kJ and AS Determine the value of the standard Gibbs free energy change for this reaction at 67.2 °C. = J 75.3 K Determine the value of the equilibrium constant for this reaction at 67.2 °C.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 38P

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Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

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