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Chapter 19: Problem 12

Why doesn't the evolution of human civilization violate the second law of thermodynamics?

Short Answer

Expert verified
The evolution of human civilization doesn't violate the second law of thermodynamics because Earth is not a closed system but an open one receiving energy from the Sun. This energy can be transformed and stored to decrease entropy (increase order) locally on Earth, while the overall entropy of the universe increases, keeping in line with the second law of thermodynamics.

Step by step solution

01

Understanding The Second Law of Thermodynamics

The First step to understanding why the evolution of human civilization does not violate the second law of thermodynamics is understanding the law itself. The Second Law of Thermodynamics states that the total entropy or disorder of a closed system cannot decrease over time. This is to say that things tend to move towards a state of maximum disorder.
02

Understanding the Evolution of Human Civilization

Human civilization has evolved over time, becoming more sophisticated and complex. This seems to suggest an increase in order, which seems to contradict the second law of thermodynamics. However, remember that the second law of thermodynamics refers to closed systems.
03

Recognizing Earth as an Open System

It's important to recognize that Earth is not a closed system. It continuously receives sunlight, which is a source of energy. This energy from the sun allows processes to take place on Earth that can result in a local decrease in entropy (increase in order).
04

Connecting Energy Input to Decrease in Entropy

The energy from the sun is converted into various forms of stored energy on Earth – in plants via photosynthesis, in fossil fuels, etc. This stored energy can then be harnessed by humans to create order (i.e. decrease entropy) - build buildings, create societies, advance technology, etc. While these processes decrease entropy on Earth, they increase the total entropy of the universe, thus not violating the Second Law of Thermodynamics.
05

Understanding the Overall Increase in Entropy

While the energy from the sun allows for a relative decrease in entropy or increase in order on Earth, it contributes to an overall increase in entropy in the universe. This is because the energy from the sun that reaches the earth is a small fraction of the total energy the sun radiates into space. The majority of it is radiated into space where it increases the universe's overall entropy. Therefore, even while processes on Earth may locally decrease entropy, the total entropy of the universe still increases, staying consistent with the second law of thermodynamics.

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Most popular questions from this chapter

Problem 74 of Chapter 16 provided an approximate expression for the specific heat of copper at low absolute temperatures: \(c=31(T / 343 \mathrm{K})^{3} \mathrm{J} / \mathrm{kg} \cdot \mathrm{K} .\) Use this to find the entropy change when \(40 \mathrm{g}\) of copper are cooled from \(25 \mathrm{K}\) to \(10 \mathrm{K}\). Why is the change negative?

Consider a gas containing an even number \(N\) of molecules, distributed among the two halves of a closed box. Find expressions for (a) the total number of microstates and (b) the number of microstates with half the molecules on each side of the box. (You can either work out a formula, or explore the term "combinations" in a math reference source.) (c) Use these results to find the ratio of the probability that all the molecules will be found on one side of the box to the probability that there will be equal numbers on both sides. (d) Evaluate for \(N=4\) and \(N=100\).

An object's heat capacity is inversely proportional to its absolute temperature: \(C=C_{0}\left(T_{0} / T\right),\) where \(C_{0}\) and \(T_{0}\) are constants. Find the entropy change when the object is heated from \(T_{0}\) to \(T_{1}\).

Energy is conserved, so why can't we recycle it as we do materials?

Find an expression for the entropy gain when hot and cold water are irreversibly mixed. A corresponding reversible process you can use to calculate this change is to bring each water sample slowly to their common final temperature \(T_{\mathrm{f}}\) and then mix them. Express your answer in terms of the initial temperatures \(T_{\mathrm{h}}\) and \(T_{\mathrm{c}} .\) Assume equal masses of hot and cold water, with constant specific heat \(c .\) What's the sign of your answer?
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