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Chapter 2: Problem 19

What are the differences between an open, a closed, and an isolated system? Describe an example of each.

Short Answer

Expert verified
An open system exchanges energy and matter, a closed system exchanges only energy, and an isolated system exchanges neither. Examples: boiling pot (open), sealed container (closed), thermos (isolated).

Step by step solution

01

Understanding System Types

Systems in thermodynamics are classified based on their interaction with the surroundings in terms of energy and matter transfer. An open system can exchange both energy and matter with its surroundings. A closed system can exchange only energy but not matter with its surroundings. An isolated system cannot exchange either energy or matter with its surroundings.
02

Example of an Open System

An open system allows for the transfer of both energy and matter. For example, a boiling pot of water without a lid is an open system because steam (matter) can escape, and heat (energy) is transferred between the water and the surrounding environment.
03

Example of a Closed System

A closed system permits only the exchange of energy, not matter. For instance, a sealed container of soup that is heated from the outside is a closed system. The container prevents the soup (matter) from escaping, although heat (energy) can still be transferred into or out of the container.
04

Example of an Isolated System

An isolated system does not allow the transfer of either energy or matter. The best practical example is a thermos bottle or a Dewar flask, which is designed to minimize heat transfer, thus trying to keep its contents at a constant temperature without exchanging energy or matter with the environment.

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Key Concepts

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

Open System
In thermodynamic terms, an open system is a system that freely exchanges both energy and matter with its surroundings. This means anything within this type of system can be influenced by the external environment. For example, consider a steaming cup of coffee. The steam rising represents the matter (water in gas form) leaving the system, while heat energy dissipates into the cooler surrounding air.

Here are key characteristics of an open system:
  • Energy exchange: Energy can be added or removed from the system, usually in the form of heat.
  • Matter exchange: Matter can move in and out of the system, such as gases or liquids.
  • Example: Beyond a boiling pot of water, other examples include human bodies or open bottles of soda.
Open systems are common in nature, as well as in industrial applications where inputs and outputs are constant.
Closed System
A closed system is defined by its ability to exchange energy but not matter with its surroundings. This characteristic makes it crucial for processes where maintaining the amount of matter is essential, while energy transformations are allowed. For instance, a sealed pressure cooker exemplifies a closed system. It can transfer heat (energy) to the contents while preventing any escape of steam (matter).

Important aspects of a closed system include:
  • No matter transfer: Matter within the system stays constant unless the system barrier is breached.
  • Energy transfer possible: Heat or other forms of energy can still cross the system's boundaries.
  • Example: Engines or refrigeration cycles often operate as closed systems during a specific phase of their functionality.
Such systems are essential in applications where preserving the mass of substances is necessary, while their energy states can vary.
Isolated System
An isolated system is one that does not engage in either energy or matter exchange with its environment. It is essentially "closed off" to outside influences. In reality, no system can be perfectly isolated; however, certain setups like a well-insulated thermos bottle come close by minimizing both heat and substance loss to its surroundings.

Key elements of an isolated system include:
  • Complete isolation: Neither matter nor energy are allowed to enter or leave.
  • Purpose: Ideal for maintaining a constant system state without external interference.
  • Example: The universe itself can be considered as an isolated system. Practically, vacuum flasks and ultra-insulated containers are designed to act similarly.
Isolated systems are theoretically indispensable for studying thermodynamic laws in a controlled environment, free from external variables that may disrupt data.

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Most popular questions from this chapter

A 7.50-g piece of iron at \(100.0^{\circ} \mathrm{C}\) is dropped into \(25.0 \mathrm{~g}\) of water at \(22.0^{\circ} \mathrm{C}\). Assuming that the heat lost by the iron equals the heat gained by the water, determine the final temperature of the iron/water system. Assume a heat capacity of water at \(4.18 \mathrm{~J} / \mathrm{g} \cdot \mathrm{K}\) and of iron at \(0.452 \mathrm{~J} / \mathrm{g} \cdot \mathrm{K}\).

True or false: Any process for which \(\Delta H\) is negative is exothermic. Explain your answer.

A \(244 \mathrm{~g}\) amount of coffee in an open plastic cup cools from \(80.0^{\circ} \mathrm{C}\) to \(20.0^{\circ} \mathrm{C}\). Assuming no loss of mass and a heat capacity of liquid water, determine \(w, q, \Delta U\), and \(\Delta H\) for the process. The densities of water are \(d\left(\mathrm{H}_{2} \mathrm{O}, 80.0^{\circ} \mathrm{C}\right)=0.9718 \mathrm{~g} / \mathrm{cm}^{3}\) and \(d\left(\mathrm{H}_{2} \mathrm{O}, 20.0^{\circ} \mathrm{C}\right)=0.9982 \mathrm{~g} / \mathrm{cm}^{3}\).

A piston reversibly and adiabatically contracts \(3.88\) moles of ideal gas to one-tenth of its original volume, then expands back to the original conditions. It does this a total of five times. If the initial and final temperatures both are \(27.5^{\circ} \mathrm{C}\), calculate (a) the total work and (b) the total \(\Delta U\) for the overall process.

A bottle of soda has a head space containing \(25.0 \mathrm{~mL}\) of \(\mathrm{CO}_{2}\) gas at \(4.2\) atm pressure when the soda is at \(4.4^{\circ} \mathrm{C}\). The bottle is opened slowly, letting the excess pressure escape. How much work does the escaping \(\mathrm{CO}_{2}\) do if the ambient pressure is \(1.0 \mathrm{~atm}\) ? Assume that the temperature remains constant.
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