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Chapter 5: Problem 21

(a) Which of the following cannot leave or enter a closed system: heat, work, or matter? (b) Which cannot leave or enter an isolated system? (c) What do we call the part of the universe that is not part of the system?

Short Answer

Expert verified
(a) Matter cannot leave or enter a closed system; (b) Neither heat, work, nor matter can leave or enter an isolated system; (c) The part of the universe not part of the system is called the surroundings.

Step by step solution

01

Understanding a Closed System

In a closed system, matter cannot enter or leave the system boundary. However, energy in the form of heat or work can be exchanged across the boundary.
02

Analyzing an Isolated System

In an isolated system, neither matter nor energy (in the form of heat or work) can cross the system boundary. The system is completely isolated from its surroundings without any exchange of matter or energy.
03

Defining Surroundings

The part of the universe that is not part of the system is called the surroundings. In thermodynamics, the system is typically isolated for analysis, and everything outside is considered the surroundings that may interact with the system.

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Key Concepts

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

Closed Systems
A closed system is a fundamental concept in thermodynamics. In such systems, matter cannot enter or exit through the system's boundary.
However, energy is not as restricted. Energy, in the form of heat or work, can flow across the boundary of a closed system. This means that although the mass remains constant, the energy levels within the system can change.
For instance, consider a sealed pot on a stove. The water inside won't leave the pot unless the lid is moved, but the heat from the stove can still enter the pot to increase the temperature of the water.
  • This allows for various changes within the system as long as they don't involve a shift in matter.
It's crucial to note the difference between energy and matter in these contexts, as it dictates what types of processes can occur within the system.
Isolated Systems
An isolated system takes the idea of a closed system a step further. In an isolated system, not only is matter unable to move across the system's boundary, but energy in any form (such as heat or work) also cannot cross that boundary.
This means these systems are entirely closed off from interactions with their surroundings.
Imagine a vacuum flask or thermos that is perfectly sealed. In this scenario, no heat escapes or enters, and no matter can be exchanged with the surroundings.
  • This makes isolated systems ideal for studying reactions or processes that need no external interference.
Thus, isolated systems are rare in everyday applications but are useful concepts for theoretical scenarios.
System and Surroundings
In thermodynamics, distinguishing between a system and its surroundings is essential. The system comprises the part of the universe that is being studied or analyzed. Everything outside this boundary is termed the surroundings.
Understanding the interaction between these two is key to understanding thermodynamic processes. It's the surroundings that the system exchanges heat, work, or other forms of energy with, except in the case of isolated systems.
  • For practical purposes, defining the system clearly at the beginning of any analysis is necessary to set up the scope of observations.
For example, when observing a chemical reaction in a beaker, the chemicals and the beaker constitute the system, while everything else is the surroundings.

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Most popular questions from this chapter

The heat of combustion of ethanol, \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(t),\) is -1367 \(\mathrm{kJ} / \mathrm{mol}\). A bottle of stout (dark beer) contains up to \(6.0 \%\) ethanol by mass. Assuming the density of the beer to be \(1.0 \mathrm{~g} / \mathrm{mL},\) what is the caloric content due to the alcohol (ethanol) in a bottle of beer (500 mL)?

Indicate which of the following is independent of the path by which a change occurs: (a) the change in potential energy when a book is transferred from table to shelf, \((\mathbf{b})\) the heat evolved when a cube of sugar is oxidized to \(\mathrm{CO}_{2}(g)\) and \(\mathrm{H}_{2} \mathrm{O}(g),(\mathbf{c})\) the work accomplished in burning a gallon of gasoline.

Given the data $$ \begin{aligned} \mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) & \longrightarrow 2 \mathrm{NO}(g) & & \Delta H=+180.7 \mathrm{~kJ} \\ 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) & \longrightarrow 2 \mathrm{NO}_{2}(g) & \Delta H=-113.1 \mathrm{~kJ} \\ 2 \mathrm{~N}_{2} \mathrm{O}(g) & \longrightarrow 2 \mathrm{~N}_{2}(g)+\mathrm{O}_{2}(g) & \Delta H &=-163.2 \mathrm{~kJ} \end{aligned} $$ use Hess's law to calculate \(\Delta H\) for the reaction $$ \mathrm{N}_{2} \mathrm{O}(g)+\mathrm{NO}_{2}(g) \longrightarrow 3 \mathrm{NO}(g) $$

A \(2.20-g\) sample of phenol \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{OH}\right)\) was burned in a bomb calorimeter whose total heat capacity is \(11.90 \mathrm{~kJ} /{ }^{\circ} \mathrm{C} .\) The temperature of the calorimeter plus contents increased from 21.50 to \(27.50^{\circ} \mathrm{C}\). (a) Write a balanced chemical equation for the bomb calorimeter reaction. (b) What is the heat of combustion per gram of phenol and per mole of phenol?

Both oxyhydrogen torches and fuel cells use the following reaction to produce energy: $$ 2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l) $$ Both processes occur at constant pressure. In both cases the change in state of the system is the same: the reactant is oxyhydrogen ("Knallgas") and the product is water. Yet, with an oxyhydrogen torch, the heat evolved is large and with a fuel cell it is small. If heat at constant pressure is considered to be a state function, why does it depend on path?
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