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X After 2.00 × 10² g of gold (Cp,s = 0.131 J g-¹ K-¹) at 120.0 °C is dropped into 25.0 g of water (Cp,s = 4.184 J g-¹ K-¹) at 10.0 °C, the system is allowed to reach equilibrium. Calculate the entropy change (in J K-¹) for the system of gold + water. +1.19 +7.83 -6.64 0 +14.5

X After 2.00 × 10² g of gold (Cp,s = 0.131 J g-¹ K-¹) at 120.0 °C is dropped into 25.0 g of water (Cp,s = 4.184 J g-¹ K-¹) at 10.0 °C, the system is allowed to reach equilibrium. Calculate the entropy change (in J K-¹) for the system of gold + water. +1.19 +7.83 -6.64 0 +14.5

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 14.3QE: Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been...
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After 2.00 × 10² g of gold (Cp,s = 0.131 J g-¹ K-¹) at 120.0 °C is dropped into 25.0 g of water (Cp,s = 4.184 J g-¹ K-¹) at 10.0 °C, the system is allowed to reach equilibrium. Calculate the entropy change (in J K-1) for the system of gold + water. +1.19 +7.83 -6.64 0 +14.5
Transcribed Image Text:After 2.00 × 10² g of gold (Cp,s = 0.131 J g-¹ K-¹) at 120.0 °C is dropped into 25.0 g of water (Cp,s = 4.184 J g-¹ K-¹) at 10.0 °C, the system is allowed to reach equilibrium. Calculate the entropy change (in J K-1) for the system of gold + water. +1.19 +7.83 -6.64 0 +14.5
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