You dissolve 2.000 g of KCl (s) with 48.000 g of water (resulting in a solution with a total mass of 50.000 g) in an insulated container. This results in a change in temperature of the solution of – 2.1 °C. Assume that the specific heat capacity of this solution is 4.184 J/ (g °C). Please calculate the change in entropy (AS) for this reaction at 298 K using the AGf values listed below: KCI (s) AGf = - 408.3 kJ / mol K+ (aq) AG = - 283.2 kJ / mol CI (aq) AGfº = – 131.2 kJ / mol + 44000 kJ / (K mol) + 16 kJ / (K · mol) + 330 kJ / (K · mol) + 2.8 kJ / (K · mol) + 0.074 kJ / (K• mol)
You dissolve 2.000 g of KCl (s) with 48.000 g of water (resulting in a solution with a total mass of 50.000 g) in an insulated container. This results in a change in temperature of the solution of – 2.1 °C. Assume that the specific heat capacity of this solution is 4.184 J/ (g °C). Please calculate the change in entropy (AS) for this reaction at 298 K using the AGf values listed below: KCI (s) AGf = - 408.3 kJ / mol K+ (aq) AG = - 283.2 kJ / mol CI (aq) AGfº = – 131.2 kJ / mol + 44000 kJ / (K mol) + 16 kJ / (K · mol) + 330 kJ / (K · mol) + 2.8 kJ / (K · mol) + 0.074 kJ / (K• mol)
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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Transcribed Image Text:You dissolve 2.000 g of KCl (s) with 48.000 g of water (resulting in a solution with a total mass of 50.000 g) in an
insulated container.
This results in a change in temperature of the solution of – 2.1 °C.
Assume that the specific heat capacity of this solution is 4.184 J/ (g °C).
Please calculate the change in entropy (AS) for this reaction at 298 K using the AGf values listed below:
KCI (s) AGfº =- 408.3 kJ / mol
K+
(aq) AGFº = - 283.2 kJ / mol
CI
(aq) AGf = – 131.2 kJ / mol
--
+ 44000 kJ / (K · mol)
+ 16 kJ / (K · mol)
+ 330 kJ / (K · mol)
+ 2.8 kJ / (K · mol)
+ 0.074 kJ / (K · mol)
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