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2. Identify whether the thermodynamic quantities will be negative, positive, or zero for the following spontaneous processes. Briefly explain your answer in each box (note: you may use equations as an explanation). Assume only expansion/compression work is possible. a. Two solid compounds react to form a liquid and gas at 1 bar, which decreases the temperature of the surroundings.

2. Identify whether the thermodynamic quantities will be negative, positive, or zero for the following spontaneous processes. Briefly explain your answer in each box (note: you may use equations as an explanation). Assume only expansion/compression work is possible. a. Two solid compounds react to form a liquid and gas at 1 bar, which decreases the temperature of the surroundings.

Introduction to Chemical Engineering Thermodynamics
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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**Problem Statement:** 2. Identify whether the thermodynamic quantities will be negative, positive, or zero for the following spontaneous processes. Briefly explain your answer in each box (note: you may use equations as an explanation). Assume only expansion/compression work is possible. a. Two solid compounds react to form a liquid and gas at 1 bar, which decreases the temperature of the surroundings. **Table with Thermodynamic Quantities:** | | | | | | | |------|------|------|------|--------|-------| | **q** | **w** | **ΔU** | **ΔH** | **ΔS_sys** | **ΔS_surr** | **Explanation:** - **q (Heat):** This will likely be negative because the reaction decreases the temperature of the surroundings, indicating an endothermic process. - **w (Work):** Since a gas is formed, expansion work is done, likely indicating a negative value (work done by the system). - **ΔU (Change in Internal Energy):** Considering the first law of thermodynamics (\(ΔU = q + w\)), we need specific values of q and w to determine the sign, but it suggests a variable outcome. - **ΔH (Change in Enthalpy):** For an endothermic reaction, ΔH is positive. - **ΔS_sys (Change in Entropy of the System):** Creating more disorder by forming gas, ΔS_sys is positive. - **ΔS_surr (Change in Entropy of the Surroundings):** As the surroundings decrease in temperature, ΔS_surr is negative.
Transcribed Image Text:**Problem Statement:** 2. Identify whether the thermodynamic quantities will be negative, positive, or zero for the following spontaneous processes. Briefly explain your answer in each box (note: you may use equations as an explanation). Assume only expansion/compression work is possible. a. Two solid compounds react to form a liquid and gas at 1 bar, which decreases the temperature of the surroundings. **Table with Thermodynamic Quantities:** | | | | | | | |------|------|------|------|--------|-------| | **q** | **w** | **ΔU** | **ΔH** | **ΔS_sys** | **ΔS_surr** | **Explanation:** - **q (Heat):** This will likely be negative because the reaction decreases the temperature of the surroundings, indicating an endothermic process. - **w (Work):** Since a gas is formed, expansion work is done, likely indicating a negative value (work done by the system). - **ΔU (Change in Internal Energy):** Considering the first law of thermodynamics (\(ΔU = q + w\)), we need specific values of q and w to determine the sign, but it suggests a variable outcome. - **ΔH (Change in Enthalpy):** For an endothermic reaction, ΔH is positive. - **ΔS_sys (Change in Entropy of the System):** Creating more disorder by forming gas, ΔS_sys is positive. - **ΔS_surr (Change in Entropy of the Surroundings):** As the surroundings decrease in temperature, ΔS_surr is negative.
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