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Chapter 6: Problem 15

Label each of the following systems as high or low entropy: 1\. perfume the instant after it is sprayed into the air 2\. an unmaintained 1950 s car compared with a brand new car 3\. a living cell compared with a dead cell a. \(1 .\) low 2\. high 3\. low b. \(1 .\) low 2\. high 3\. high C. \(1 .\) high 2\. low 3\. high d. \(1 .\) high 2.. low 3\. low

Short Answer

Expert verified
Option a is correct. The answers are: 1. high, 2. high, 3. low.

Step by step solution

01

Understand Entropy

Entropy is a measure of disorder or randomness in a system. High entropy means higher disorder and lower entropy means more order.
02

Analyze the Perfume

Perfume the instant after it is sprayed into the air is highly disordered because its molecules are spreading out randomly in all directions. Therefore, it has high entropy.
03

Analyze the Cars

An unmaintained 1950s car is likely more disordered compared to a brand new car due to rust, wear-and-tear, and general neglect. Therefore, the old car has high entropy.
04

Analyze the Cells

A living cell is highly organized and maintains various functions and structures, whereas a dead cell has lost this organization. Therefore, a living cell has low entropy compared to a dead cell.
05

Compare to Answers

The correct labeling should be: 1. high, 2. high, 3. low. This matches option a.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

entropy
Entropy is a fundamental concept in thermodynamics and statistical mechanics. It measures the amount of disorder or randomness within a system. In simpler terms, the higher the entropy, the more chaotic the system is. Conversely, the lower the entropy, the more ordered and structured the system. This concept helps explain why certain processes occur naturally, as most systems tend to move towards higher entropy or disorder.
disorder in systems
Disorder in systems can be easily understood with daily life examples. Imagine a clean, well-organized room versus a messy room with items scattered everywhere. The messy room represents high entropy, as everything is disordered and chaotic. On the other hand, the organized room represents low entropy, where items are systematically arranged. This demonstrates that systems with high entropy have elements that are spread out randomly, while systems with low entropy have a certain degree of organization.
living vs non-living cells
The difference in entropy between living and non-living cells is significant. A living cell is a highly complex and organized entity, maintaining specific functions and structures crucial for life. This high degree of organization translates to low entropy. In contrast, a dead cell has lost this organization, and its internal components start to degrade and disperse, leading to higher entropy. This shift from low to high entropy marks the transition from an organized, living state to a disorganized, non-living state.
comparison of entropy in objects
Comparing the entropy in different objects can help us understand their respective states of disorder. For instance, when perfume is freshly sprayed into the air, its molecules quickly disperse in various directions, increasing entropy. An old, unmaintained car from the 1950s, suffering from rust and wear, represents higher entropy compared to a new car, which is more ordered and structured. Similarly, the entropy in a living cell is lower because of its organized systems, whereas a dead cell has higher entropy due to the loss of this organization.
thermodynamics in biology
Thermodynamics, specifically the concept of entropy, plays a crucial role in biological systems. Living organisms maintain their organized state (low entropy) through various biological processes that require energy. For example, cells perform metabolic functions, synthesize proteins, and repair damage, all of which contribute to maintaining low entropy. When these processes stop, as in the death of a cell or organism, the system starts to degrade, leading to higher entropy, illustrating how biological systems adhere to the principles of thermodynamics.

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Most popular questions from this chapter

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Consider a simple process that illustrates the change in entropy when energy is transferred. 1\. Take a block of ice as a system with a temperature of \(0^{\circ} \mathrm{C}\) . This is water as a solid, so it has a high structural order. This means that the molecules are in a fixed position. As a result, the entropy of the system is low. 2\. Allow the ice to melt at room temperature. Describe changes in the motion and interactions of water molecules before and after melting. Explain where the energy came from whose transfer produced melting. Predict the effect of the energy transfer on the entropy on the system, and justify your prediction. 3\. Heat the water until the temperature reaches boiling point. Explain what happens to the entropy of the system when the water is heated. 4\. Continue to heat the water at the constant temperature of the boiling point. Describe changes in the motion and interactions of water molecules before and after boiling. Predict the effect of the energy transfer on the entropy of the system, and justify your prediction. 5\. [Extension/Connection] Molecules of water have simple responses to heating: The molecules move faster and interact less strongly with other neighboring molecules. Consider the primary producers of an aquatic ecosystem in summer. Describe the source of energy transfer to the system of photosynthetic plants and algae. Predict changes in the system in response. Explain what happens to the entropy of this trophic level when energy transfer occurs. Now consider the primary producers and their aqueous environment as the system. Explain what happens to the entropy of this system composed of photosynthetic organisms and their abiotic environment. 6\. Predict the change in entropy of the system when both autotrophs and their abiotic environment are considered. Justify your prediction. Predict the signs of the entropy changes in both biotic and abiotic components of this system. Predict the relative magnitudes of these entropy changes, and justify your prediction.
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