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 grams of ammonia vapor (NH\(_3\)). | The ammonia condenses to a liquid at a constant temperature of -8.0°C. | ○ \(\Delta S < 0\) (Selected) || | | ○ \(\Delta S = 0\) || | | ○ \(\Delta S > 0\) || | | ○ not enough information || A few moles of nitrogen (N\(_2\)) gas. | The nitrogen is cooled from 78.0°C to 3.0°C while the volume is held constant at 2.0 L. | ○ \(\Delta S < 0\) || | | ○ \(\Delta S = 0\) || | | ○ \(\Delta S > 0\) || | | ○ not enough information (Selected) || A few moles of nitrogen (N\(_2\)) gas. | The nitrogen is heated from -16.0°C to 12.0°C and also expands from a volume of 1.0 L to a volume of 10.0 L. | ○ \(\Delta S < 0\) || | | ○ \(\Delta S = 0\) || | | ○ \(\Delta S > 0\) || | | ○ not enough information (Selected) |

Answered: For each system listed in the first…

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 grams of ammonia vapor (NH\(_3\)). | The ammonia condenses to a liquid at a constant temperature of -8.0°C. | ○ \(\Delta S < 0\) (Selected) |
| | | ○ \(\Delta S = 0\) |
| | | ○ \(\Delta S > 0\) |
| | | ○ not enough information |

| A few moles of nitrogen (N\(_2\)) gas. | The nitrogen is cooled from 78.0°C to 3.0°C while the volume is held constant at 2.0 L. | ○ \(\Delta S < 0\) |
| | | ○ \(\Delta S = 0\) |
| | | ○ \(\Delta S > 0\) |
| | | ○ not enough information (Selected) |

| A few moles of nitrogen (N\(_2\)) gas. | The nitrogen is heated from -16.0°C to 12.0°C and also expands from a volume of 1.0 L to a volume of 10.0 L. | ○ \(\Delta S < 0\) |
| | | ○ \(\Delta S = 0\) |
| | | ○ \(\Delta S > 0\) |
| | | ○ not enough information (Selected) |

Expert Solution

Step 1

Entropy is the degree of disorderness or degree of randomness. As Temperature increases, entropy increases. As volume increases entropy also increases, because the molecules has more space to move.

Thus, when both Temperature and Volume is increased entropy increases, ∆S > 0.

When both Temperature and Volume is decreased, entropy decreases, ∆S < 0.

When The temperature is increased ( ∆S > 0 )and volume is decreased (∆S < 0 ) or vice versa we cannot predict the sign of overall entropy.

Entropy of gas > Entropy of liquid > Entropy of solid

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