A student determines the value of the equilibrium constant to be 2.30 x 10¹6 for the following reaction. Ca(OH)2 (aq) + 2HCl(aq) → CaCl₂ (s) + 2H₂O(l) Based on this value of Keq AGO for this reaction is expected to be than zero. Calculate the free energy change for the reaction of 1.57 moles of Ca(OH)2 (aq) at standard conditions at 298 K. AGO kj Ixn
A student determines the value of the equilibrium constant to be 2.30 x 10¹6 for the following reaction. Ca(OH)2 (aq) + 2HCl(aq) → CaCl₂ (s) + 2H₂O(l) Based on this value of Keq AGO for this reaction is expected to be than zero. Calculate the free energy change for the reaction of 1.57 moles of Ca(OH)2 (aq) at standard conditions at 298 K. AGO kj Ixn
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter16: Thermodynamics: Directionality Of Chemical Reactions
Section: Chapter Questions
Problem 105QRT
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Transcribed Image Text:A student determines the value of the equilibrium constant to be 2.30 x 10¹6 for the following reaction.
Ca(OH)2 (aq) + 2HCl(aq) → CaCl₂ (s) + 2H₂O(1)
Based on this value of Keq
AGO for this reaction is expected to be
than zero.
Calculate the free energy change for the reaction of 1.57 moles of Ca(OH)2 (aq) at standard conditions at 298 K.
AGO
rxn
kJ
Transcribed Image Text:A student determines the value of the equilibrium constant to be 3.56×10-18 for the following reaction.
Fe3O4(s) + 4H₂(g) 3Fe(s) + 4H₂O(g)
Based on this value of Keqi
AGO for this reaction is expected to be (greater, less)
than zero.
Calculate the free energy change for the reaction of 1.84 moles of Fe3O4(s) at standard conditions at 298K.
AG° rxn=
kj
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