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For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. System A few moles of carbon dioxide (CO₂) gas. A few moles of carbon dioxide (CO₂) gas. A few grams of liquid water (H₂O). Change The carbon dioxide expands from a volume of 1.0 L to a volume of 3.0 L while the temperature is held constant at 82.0 °C. The carbon dioxide is cooled from 77.0 °C to 8.0 °C and is also expanded from a volume of 2.0 L to a volume of 12.0 L. The water is heated from -12.0 °C to 63.0 °C. AS AS < 0 OAS = 0 OAS> 0 not enough. information OAS <0 AS = 0 O AS> 0 not enough. information Ο ΔS < 0 O AS = 0 OAS> 0 not enough information

For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. System A few moles of carbon dioxide (CO₂) gas. A few moles of carbon dioxide (CO₂) gas. A few grams of liquid water (H₂O). Change The carbon dioxide expands from a volume of 1.0 L to a volume of 3.0 L while the temperature is held constant at 82.0 °C. The carbon dioxide is cooled from 77.0 °C to 8.0 °C and is also expanded from a volume of 2.0 L to a volume of 12.0 L. The water is heated from -12.0 °C to 63.0 °C. AS AS < 0 OAS = 0 OAS> 0 not enough. information OAS <0 AS = 0 O AS> 0 not enough. information Ο ΔS < 0 O AS = 0 OAS> 0 not enough information

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy \( S \) of the system, decrease \( S \), or leave \( S \) unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. | System | Change | \( \Delta S \) | |-----------------------------------------------|------------------------------------------------------------------------------------------------------------------------------------------|-----------------------------------------| | A few moles of carbon dioxide (\( \text{CO}_2 \)) gas. | The carbon dioxide expands from a volume of 1.0 L to a volume of 3.0 L while the temperature is held constant at 82.0 °C. | ⬤ \( \Delta S > 0 \) | | A few moles of carbon dioxide (\( \text{CO}_2 \)) gas. | The carbon dioxide is cooled from 77.0 °C to 8.0 °C and is also expanded from a volume of 2.0 L to a volume of 12.0 L. | ⬤ \( \Delta S > 0 \) | | A few grams of liquid water (\( \text{H}_2\text{O} \)). | The water is heated from -12.0 °C to 63.0 °C. | ⬤ \( \Delta S > 0 \) | **Explanation:** 1. **First Scenario:** - **System:** Carbon dioxide gas. - **Change:** Expansion while temperature remains constant. - **Entropy Change (\( \Delta S \))**: Positive, since entropy increases with expansion at constant temperature. 2. **Second Scenario:** - **System:** Carbon dioxide gas. - **Change:** Cooled and expanded significantly. - **Entropy Change (\( \Delta S \))**: Positive, as the effect of expansion outweighs the entropy decrease due to cooling. 3. **Third Scenario:** - **System:** Liquid water. - **Change:** Water is heated. - **Entropy Change (\( \Delta S \))**: Positive, as heating increases entropy.
Transcribed Image Text:For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy \( S \) of the system, decrease \( S \), or leave \( S \) unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. | System | Change | \( \Delta S \) | |-----------------------------------------------|------------------------------------------------------------------------------------------------------------------------------------------|-----------------------------------------| | A few moles of carbon dioxide (\( \text{CO}_2 \)) gas. | The carbon dioxide expands from a volume of 1.0 L to a volume of 3.0 L while the temperature is held constant at 82.0 °C. | ⬤ \( \Delta S > 0 \) | | A few moles of carbon dioxide (\( \text{CO}_2 \)) gas. | The carbon dioxide is cooled from 77.0 °C to 8.0 °C and is also expanded from a volume of 2.0 L to a volume of 12.0 L. | ⬤ \( \Delta S > 0 \) | | A few grams of liquid water (\( \text{H}_2\text{O} \)). | The water is heated from -12.0 °C to 63.0 °C. | ⬤ \( \Delta S > 0 \) | **Explanation:** 1. **First Scenario:** - **System:** Carbon dioxide gas. - **Change:** Expansion while temperature remains constant. - **Entropy Change (\( \Delta S \))**: Positive, since entropy increases with expansion at constant temperature. 2. **Second Scenario:** - **System:** Carbon dioxide gas. - **Change:** Cooled and expanded significantly. - **Entropy Change (\( \Delta S \))**: Positive, as the effect of expansion outweighs the entropy decrease due to cooling. 3. **Third Scenario:** - **System:** Liquid water. - **Change:** Water is heated. - **Entropy Change (\( \Delta S \))**: Positive, as heating increases entropy.
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**Entropy Changes in Systems** For each system listed in the table below, determine whether the change described will increase the entropy \(S\) of the system, decrease \(S\), or leave \(S\) unchanged. If there isn't enough information to decide, select the "not enough information" option. | **System** | **Change** | **\(\Delta S\)** | |--------------------------------------------|----------------------------------------------------------------------------------------------------------------------------------------------------------------|----------------------------| | A few moles of carbon dioxide \((\text{CO}_2)\) gas. | The carbon dioxide expands from a volume of 1.0 L to a volume of 3.0 L while the temperature is held constant at 82.0 °C. | ○ \(\Delta S < 0\) <br> ○ \(\Delta S = 0\) <br> ● \(\Delta S > 0\) <br> ○ not enough information | | A few moles of carbon dioxide \((\text{CO}_2)\) gas. | The carbon dioxide is cooled from 77.0 °C to 8.0 °C and is also expanded from a volume of 2.0 L to a volume of 12.0 L. | ○ \(\Delta S < 0\) <br> ○ \(\Delta S = 0\) <br> ● \(\Delta S > 0\) <br> ○ not enough information | | A few grams of liquid water \((\text{H}_2\text{O})\). | The water is heated from -12.0 °C to 63.0 °C. | ○ \(\Delta S < 0\) <br> ○ \(\Delta S = 0\) <br> ● \(\Delta S > 0\) <br> ○ not enough information | **Explanation of Selections:** - For the first system, expanding the gas at constant temperature typically increases the entropy. - For the second system, although the gas is cooled (which decreases entropy), the significant volume expansion can lead to an overall increase in entropy. - For the third system, heating the liquid water increases the entropy as thermal motion and disorder within the system rise.
Transcribed Image Text:**Entropy Changes in Systems** For each system listed in the table below, determine whether the change described will increase the entropy \(S\) of the system, decrease \(S\), or leave \(S\) unchanged. If there isn't enough information to decide, select the "not enough information" option. | **System** | **Change** | **\(\Delta S\)** | |--------------------------------------------|----------------------------------------------------------------------------------------------------------------------------------------------------------------|----------------------------| | A few moles of carbon dioxide \((\text{CO}_2)\) gas. | The carbon dioxide expands from a volume of 1.0 L to a volume of 3.0 L while the temperature is held constant at 82.0 °C. | ○ \(\Delta S < 0\) <br> ○ \(\Delta S = 0\) <br> ● \(\Delta S > 0\) <br> ○ not enough information | | A few moles of carbon dioxide \((\text{CO}_2)\) gas. | The carbon dioxide is cooled from 77.0 °C to 8.0 °C and is also expanded from a volume of 2.0 L to a volume of 12.0 L. | ○ \(\Delta S < 0\) <br> ○ \(\Delta S = 0\) <br> ● \(\Delta S > 0\) <br> ○ not enough information | | A few grams of liquid water \((\text{H}_2\text{O})\). | The water is heated from -12.0 °C to 63.0 °C. | ○ \(\Delta S < 0\) <br> ○ \(\Delta S = 0\) <br> ● \(\Delta S > 0\) <br> ○ not enough information | **Explanation of Selections:** - For the first system, expanding the gas at constant temperature typically increases the entropy. - For the second system, although the gas is cooled (which decreases entropy), the significant volume expansion can lead to an overall increase in entropy. - For the third system, heating the liquid water increases the entropy as thermal motion and disorder within the system rise.
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