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: McGraw-Hill Education
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Question
**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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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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