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Chapter 5: Problem 19

(a) What is meant by the term system in thermodynamics? (b) What is a closed system? (c) What do we call the part of the universe that is not part of the system?

Short Answer

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(a) In thermodynamics, a "system" refers to a specific portion of the universe being observed or studied, surrounded by a boundary separating it from its surroundings. (b) A "closed system" is a type of thermodynamic system that can exchange energy with its surroundings but does not exchange matter. (c) The part of the universe not part of the system being studied is called the "surroundings."

Step by step solution

01

(a) Definition of System in Thermodynamics

In thermodynamics, a "system" is a specific portion of the universe that is being observed or studied. It can be any specific region or object, like a container of gas, a metal, or a chemical reaction. The system is surrounded by a boundary that separates it from its surroundings (the rest of the universe). The boundary could be physical or imaginary. The main focus of the thermodynamic analysis is on the internal processes and properties of the system.
02

(b) Definition of Closed System

A "closed system" is a type of thermodynamic system that can exchange energy (in the form of work and heat) with its surroundings but does not exchange matter. In other words, no mass or particles can move across the boundary, and the total amount of matter within the closed system remains constant during the process.
03

(c) Name for the Part of the Universe Not Part of the System

The part of the universe that is not part of the system being studied is called the "surroundings." In thermodynamic analysis, the surroundings include everything that is outside the system, encompassing the rest of the universe. Both the system and its surroundings together constitute the "universe" in a thermodynamic context.

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Key Concepts

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

Thermodynamic System
In thermodynamics, the term "system" refers to a specific part of the universe that is under study or consideration. It can be anything from a container of gas to a piece of metal or a chemical reaction. The system includes all the components or substances being analyzed, and is separated from its surroundings by a boundary. This boundary can be either physically tangible, like the walls of a container, or simply an imaginary demarcation used for theoretical purposes.

The concept of a system is crucial because it allows scientists and engineers to focus on the internal processes and transformations that occur within it. This focus is essential for analyzing how energy is transferred and transformed within the system, as well as how it interacts with the surroundings.
Closed System
A closed system in thermodynamics is one that can exchange energy in the form of heat or work with its surroundings, but does not allow the transfer of matter. In simpler terms, the amount of substance or material within the system stays constant over time. This feature makes closed systems particularly interesting when examining energy conversions and transfers.

A familiar example of a closed system could be a sealed container of gas where no particles enter or leave, but the container itself can be heated from outside or exert force against a piston. Because mass remains unchanged in closed systems, these models help us understand processes where conservation of energy is key.
Surroundings in Thermodynamics
In the context of thermodynamics, the "surroundings" represent everything outside of the system being studied. Essentially, it is the remainder of the universe that interacts with the system across its boundary. The surroundings play a vital role because they are where exchanges of energy and sometimes matter occur.

When a system undergoes a thermodynamic process, energy (in various forms) can cross the boundary, influencing both the system and its surroundings. Understanding this interaction is crucial for analyzing energy efficiency, predicting system behavior, and designing practical systems in engineering. It's important to note that in a thermodynamic framework, the system and its surroundings together form what is referred to as the "universe."

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Most popular questions from this chapter

In a thermodynamic study a scientist focuses on the properties of a solution in an apparatus as illustrated. A solution is continuously flowing into the apparatus at the top and out at the bottom, such that the amount of solution in the apparatus is constant with time. (a) Is the solution in the apparatus a closed system, open system, or isolated system? Explain your choice. (b) If it is not a closed system, what could be done to make it a closed system?

Consider the following reaction: \(2 \mathrm{CH}_{3} \mathrm{OH}(g) \longrightarrow 2 \mathrm{CH}_{4}(g)+\mathrm{O}_{2}(g) \quad \Delta H=+252.8 \mathrm{~kJ}\) (a) Is this reaction exothermic or endothermic? (b) Calculate the amount of heat transferred when \(24.0 \mathrm{~g}\) of \(\mathrm{CH}_{3} \mathrm{OH}(g)\) is decomposed by this reaction at constant pressure. (c) For a given sample of \(\mathrm{CH}_{3} \mathrm{OH},\) the enthalpy change during the reaction is \(82.1 \mathrm{~kJ}\). How many grams of methane gas are produced? (d) How many kilojoules of heat are released when \(38.5 \mathrm{~g}\) of \(\mathrm{CH}_{4}(g)\) reacts completely with \(\mathrm{O}_{2}(g)\) to form \(\mathrm{CH}_{3} \mathrm{OH}(g)\) at constant pressure?

The automobile fuel called E85 consists of \(85 \%\) ethanol and \(15 \%\) gasoline. \(\mathrm{E} 85\) can be used in so-called "flex-fuel" vehicles (FFVs), which can use gasoline, ethanol, or a mix as fuels. Assume that gasoline consists of a mixture of octanes (different isomers of \(\mathrm{C}_{8} \mathrm{H}_{18}\) ), that the average heat of combustion of \(\mathrm{C}_{8} \mathrm{H}_{18}(l)\) is \(5400 \mathrm{~kJ} / \mathrm{mol}\), and that gasoline has an average density of \(0.70 \mathrm{~g} / \mathrm{mL}\). The density of ethanol is \(0.79 \mathrm{~g} / \mathrm{mL}\). (a) By using the information given as well as data in Appendix C, compare the energy produced by combustion of \(1.0 \mathrm{~L}\) of gasoline and of \(1.0 \mathrm{~L}\) of ethanol. (b) Assume that the density and heat of combustion of \(\mathrm{E} 85\) can be obtained by using \(85 \%\) of the values for ethanol and \(15 \%\) of the values for gasoline. How much energy could be released by the combustion of \(1.0 \mathrm{~L}\) of E85? (c) How many gallons of E85 would be needed to provide the same energy as 10 gal of gasoline? (d) If gasoline costs \(\$ 3.10\) per gallon in the United States, what is the break-even price per gallon of \(\mathrm{E} 85\) if the same amount of energy is to be delivered?

Consider two solutions, the first being \(50.0 \mathrm{~mL}\) of \(1.00 \mathrm{M} \mathrm{CuSO}_{4}\) and the second \(50.0 \mathrm{~mL}\) of \(2.00 \mathrm{MKOH}\). When the two solutions are mixed in a constant-pressure calorimeter, a precipitate forms and the temperature of the mixture rises from \(21.5^{\circ} \mathrm{C}\) to \(27.7^{\circ} \mathrm{C}\). (a) Before mixing, how many grams of Cu are present in the solution of \(\mathrm{CuSO}_{4} ?\) (b) Predict the identity of the precipitate in the reaction. (c) Write complete and net ionic equations for the reaction that occurs when the two solutions are mixed. (d) From the calorimetric data, calculate \(\Delta H\) for the reaction that occurs on mixing. Assume that the calorimeter absorbs only a negligible quantity of heat, that the total volume of the solution is 100.0 \(\mathrm{mL},\) and that the specific heat and density of the solution after mixing are the same as that of pure water.

(a) Why are fats well suited for energy storage in the human body? (b) A particular chip snack food is composed of \(12 \%\) protein, \(14 \%\) fat, and the rest carbohydrate. What percentage of the calorie content of this food is fat? (c) How many grams of protein provide the same fuel value as \(25 \mathrm{~g}\) of fat?
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