Heat vs work - Revision history

Jmdonev: 1 revision imported

2018-07-21T01:12:59Z

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Jmdonev at 19:26, 17 July 2018

2018-07-17T19:26:26Z

← Older revision		Revision as of 19:26, 17 July 2018
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	[[Category:Done ~~2015~~-06-01]]		[[Category:Done 2018-07-20]]
	<onlyinclude>The ~~concept of~~ '''Heat vs Work''' is an important ~~one~~ in the field of [[thermodynamics]]. ~~The idea~~ of ~~how [[~~heat]] and [[work~~]] are distinct but interchangeable forms of energy~~ is crucial to how thermodynamic processes work. ~~Although heat~~ can be transformed into work and vice verse (see [[mechanical equivalent of heat]]), they aren't ~~necessarily~~ the same thing.</onlyinclude> The [[first law of thermodynamics]] states that heat and work both contribute to the total internal energy of a system, but the [[second law of thermodynamics]] limits the ~~relationship between~~ work ~~and heat~~.		<onlyinclude>[[Heat]] and [[work]] are two different ways of transferring [[energy]] from one [[system]] to another. The the distinction between '''Heat and Work''' is important in the field of [[thermodynamics]]. Heat is the transfer of thermal energy between systems, while work is the transfer of mechanical energy between two systems. This distinction between the microscopic motion (heat) and macroscopic motion (work) is crucial to how thermodynamic processes work. Heat can be transformed into work and vice verse (see [[mechanical equivalent of heat]]), but they aren't the same thing.</onlyinclude> The [[first law of thermodynamics]] states that heat and work both contribute to the total internal energy of a system, but the [[second law of thermodynamics]] limits the amount of heat that can be turned into work.

	===Main Differences===		===Main Differences===
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	* The Second Law allows work to be transformed fully into heat, but forbids heat to be totally converted into work. If heat could be transformed fully into work it would violate the laws of [[entropy]]. The maximum amount of work one can attain from heat is given by the [[Carnot efficiency]].		* The Second Law allows work to be transformed fully into heat, but forbids heat to be totally converted into work. If heat could be transformed fully into work it would violate the laws of [[entropy]]. The maximum amount of work one can attain from heat is given by the [[Carnot efficiency]].

	* Heat is the energy associated with the random motion of particles, while work is the energy of ordered motion in one direction. Therefore heat is "low-quality" energy and work is "high-quality" energy, and this supports the [[Second law of thermodynamics#Disorder Statement\|~~Entropy~~ statement]] of the Second Law.		* Heat is the energy associated with the random motion of particles, while work is the energy of ordered motion in one direction. Therefore heat is "low-quality" energy and work is "high-quality" energy, and this supports the [[Second law of thermodynamics#Disorder Statement\|entropy statement]] of the Second Law.

	Heat and work each have their own distinct properties, and ~~how~~ they differ in how they affect a system. These are listed and compared below:<ref name=Knight>R. D. Knight, "Work in Ideal-Gas Processes" and "Heat" in ''Physics for Scientists and Engineers: A Strategic Approach,'' 3nd ed. San Francisco, U.S.A.: Pearson Addison-Wesley, 2008, ch.17, sec.2 and 3, pp.471-477 </ref>		Heat and work each have their own distinct properties, and they differ in how they affect a system. These are listed and compared below:<ref name=Knight>R. D. Knight, "Work in Ideal-Gas Processes" and "Heat" in ''Physics for Scientists and Engineers: A Strategic Approach,'' 3nd ed. San Francisco, U.S.A.: Pearson Addison-Wesley, 2008, ch.17, sec.2 and 3, pp.471-477 </ref>

	{\| class="wikitable"		{\| class="wikitable"
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	\| Equilibrium \|\| A system is in mechanical equilibrium when there is no net force or torque on it. \|\| A system is in thermal equilibrium when it is at the same temperature as the environment.		\| Equilibrium \|\| A system is in mechanical equilibrium when there is no net force or torque on it. \|\| A system is in thermal equilibrium when it is at the same temperature as the environment.
	\|}		\|}

			==For Further Reading==
			*[[Heat]]
			*[[Work]]
			*[[First law of thermodynamics]]
			*[[Second law of thermodynamics]]
			*[[System and surrounding]]
			*Or explore a [[Special:Random\|random page]]

	==References==		==References==
	{{reflist}}		{{reflist}}
	[[Category:Uploaded]]		[[Category:Uploaded]]

J.williams: 1 revision imported

2015-08-26T21:31:10Z

1 revision imported

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J.williams at 16:54, 12 August 2015

2015-08-12T16:54:40Z

New page

[[Category:Done 2015-06-01]]
<onlyinclude>The concept of '''Heat vs Work''' is an important one in the field of [[thermodynamics]]. The idea of how [[heat]] and [[work]] are distinct but interchangeable forms of energy is crucial to how thermodynamic processes work. Although heat can be transformed into work and vice verse (see [[mechanical equivalent of heat]]), they aren't necessarily the same thing.</onlyinclude> The [[first law of thermodynamics]] states that heat and work both contribute to the total internal energy of a system, but the [[second law of thermodynamics]] limits the relationship between work and heat.

===Main Differences===

* The Second Law allows work to be transformed fully into heat, but forbids heat to be totally converted into work. If heat could be transformed fully into work it would violate the laws of [[entropy]]. The maximum amount of work one can attain from heat is given by the [[Carnot efficiency]].

* Heat is the energy associated with the random motion of particles, while work is the energy of ordered motion in one direction. Therefore heat is "low-quality" energy and work is "high-quality" energy, and this supports the [[Second law of thermodynamics#Disorder Statement|Entropy statement]] of the Second Law.

Heat and work each have their own distinct properties, and how they differ in how they affect a system. These are listed and compared below:<ref name=Knight>R. D. Knight, "Work in Ideal-Gas Processes" and "Heat" in ''Physics for Scientists and Engineers: A Strategic Approach,'' 3nd ed. San Francisco, U.S.A.: Pearson Addison-Wesley, 2008, ch.17, sec.2 and 3, pp.471-477 </ref>

{| class="wikitable"
|-
! !! Work (W) !! Heat (Q)
|-
| Interaction || Mechanical || Thermal
|-
| Requires || Force and Displacement || Temperature difference
|-
| Process || Macroscopic pushes and pulls || Microscopic collisions
|-
| Positive value || W > 0 when a gas is compressed. Energy is transferred into system. || Q > 0 when the environment is at a higher temperature than the system. Energy is transferred into system.
|-
| Negative value || W < 0 when a gas expands. Energy is transferred out of system. || Q < 0 when the system is at a higher temperature than the environment. Energy is transferred out of system.
|-
| Equilibrium || A system is in mechanical equilibrium when there is no net force or torque on it. || A system is in thermal equilibrium when it is at the same temperature as the environment.
|}

==References==
{{reflist}}
[[Category:Uploaded]]