Gas compressor - Revision history

95.16.92.80: /* Effect of Cooling During the Compression Process */

2015-01-07T11:49:24Z

Effect of Cooling During the Compression Process

← Older revision		Revision as of 13:49, 7 January 2015
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	My name is ~~Gabriel and~~ I am ~~studying Educational Studies and Computer Science at Jelling~~ / ~~Denmark~~.<br><br>~~Here is my homepage ...~~ [~~https~~://~~www.youtube~~.com~~/watch?v=8SgzgNU80P8 best cars~~]		Hiya and welcome there, I am Adrianne and I totally really like that name. Vermont has always been simple home and I affection every day living suitable here. Gardening is what I do invest in. I am a people manager only soon I'll be on my own. You can find my world wide web here: http://circuspartypanama.com<br><br>My web page - [http://circuspartypanama.com clash of clans hack deutsch]

109.151.35.45 at 19:46, 5 February 2014

2014-02-05T19:46:41Z

← Older revision		Revision as of 21:46, 5 February 2014
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	[[File:Endergonic Reaction.svg\|thumbnail\|An endergonic reaction (such as photosynthesis) is a reaction that requires energy to be driven. The activation energy for the reaction is typically larger than the overall energy of the exergonic reaction(1). Endergonic reactions are nonspontaneous. The progress of the reaction is shown by the line. The change of Gibbs free energy (ΔG) during an endergonic reaction is a positive value because energy is gained (2).]]		My name is Gabriel and I am studying Educational Studies and Computer Science at Jelling / Denmark.<br><br>Here is my homepage ... [https://www.youtube.com/watch?v=8SgzgNU80P8 best cars]
	~~{{unreferenced\|date=May 2009}}~~
	In [[thermochemistry\|chemical thermodynamics]], an '''endergonic reaction''' (also called a '''nonspontaneous reaction''' or an '''unfavorable reaction''') is a [[chemical reaction]] in which the standard change in [[Thermodynamic free energy\|free energy]] is ~~positive,~~ and energy is absorbed. In layman's terms the total amount of energy is a loss (it takes more energy to start the reaction than what you get out of it) so the total energy is a negative net result. For an overall gain in the net result see [[Exergonic reaction\|Exergonic Reaction]].

	~~Under constant temperature~~ and ~~constant pressure conditions, this means that the change in the standard [[Gibbs free energy]] would be positive~~

	~~:<math>\Delta G^\circ > 0<~~/~~math>~~

	~~for the reaction at [[standard state]] (i~~.~~e. at standard pressure (1 [[Bar (unit)\|bar]]), and standard concentrations (1 [[Concentration#Molarity\|molar]]) of all the reagents).~~

	~~== Equilibrium constant ==~~

	~~The [[equilibrium constant]] for the reaction is related to Δ''G''° by the relation:~~

	:<~~math~~>~~K = e^{-\frac{\Delta G^\circ}{RT}}~~<~~/math~~>

	~~where ''T'' is the [[absolute temperature]] and ''R''~~ is ~~the [[gas constant]]~~. ~~A positive value of Δ''G''° therefore implies~~

	~~:<math>K < 1 \,</math>~~

	~~so that starting from molar stoichiometric quantities such a reaction would move backwards toward equilibrium, not forwards~~.

	~~Nevertheless, endergonic reactions are quite common in nature, especially in [[biochemistry]] and [[physiology]]~~. ~~Examples of endergonic reactions in cells include~~ [~~[protein synthesis]], and the [[Na+/K+-ATPase\|Na<sup>+<~~/~~sup>/K<sup>+<~~/~~sup> pump]] which drives [[action potential\|nerve conduction]] and [[muscle contraction]].~~

	~~== Making Endergonic reactions happen ==~~

	~~Endergonic reactions can be achieved if they are either ''pulled'' or ''pushed'' by an [[exergonic]] (stability increasing, negative change in Free Energy) process.~~

	~~=== Pull ===~~

	Reagents can be ''pulled'' through an endergonic reaction, if the reaction products are cleared rapidly by a subsequent exergonic reaction. The concentration of the products of the endergonic reaction thus always remains low, so the reaction can proceed.

	~~A classic example of this might be the first stage of a reaction which proceeds via a [[transition state]]~~. The process of getting to the top of the [[activation energy\|activation energy barrier]] to the transition state is endergonic. However, the reaction can proceed because having reached the transition state, it rapidly evolves via an exergonic process to the more stable final products.

	~~=== Push ===~~

	~~Endergonic reactions can be ''pushed'' by coupling them to another reaction which is strongly exergonic, through a shared intermediate.~~

	~~This is often how biological reactions proceed. For example, on its own the reaction~~
	~~:<math> X + Y \longrightarrow XY<~~/~~math>~~
	may be too endergonic to occur. However it may be possible to make it occur by coupling it to a strongly exergonic reaction – such as, very often, the decomposition of [[Adenosine triphosphate\|ATP]] into [[Adenosine diphosphate\|ADP]] and inorganic phosphate ions, ATP → ADP + P<sub>i</sub>, so that
	~~:<math> X + \mathit{ATP} \longrightarrow \mathit{XP} + \mathit{ADP}</math>~~
	~~:<math> \mathit{XP} + Y \longrightarrow \mathit{XY} + P_i</math>~~
	This kind of reaction, with the ATP decomposition supplying the free energy needed to make an endergonic reaction occur, is so common in cell biochemistry that ATP is often called the "universal energy currency" of all living organisms.

	~~==See also~~==
	*[[Endergonic]]
	*[[Exergonic]]
	*[[Exergonic reaction]]
	*[[Exothermic]]
	*[[Endothermic]]
	*[[Exothermic reaction]]
	*[[Endothermic reaction]]
	*[[Warm-blooded\|Endotherm]]
	*[[Warm-blooded\|Exotherm]]

	~~[[Category:Thermochemistry]~~]

en>Mogism: /* Scroll compressors */Cleanup/Typo fixing, typo(s) fixed: , → , using AWB

2014-01-30T12:11:45Z

Scroll compressors: Cleanup/Typo fixing, typo(s) fixed: , → , using AWB

← Older revision		Revision as of 14:11, 30 January 2014
Line 1:		Line 1:
			[[File:Endergonic Reaction.svg\|thumbnail\|An endergonic reaction (such as photosynthesis) is a reaction that requires energy to be driven. The activation energy for the reaction is typically larger than the overall energy of the exergonic reaction(1). Endergonic reactions are nonspontaneous. The progress of the reaction is shown by the line. The change of Gibbs free energy (ΔG) during an endergonic reaction is a positive value because energy is gained (2).]]
			{{unreferenced\|date=May 2009}}
			In [[thermochemistry\|chemical thermodynamics]], an '''endergonic reaction''' (also called a '''nonspontaneous reaction''' or an '''unfavorable reaction''') is a [[chemical reaction]] in which the standard change in [[Thermodynamic free energy\|free energy]] is positive, and energy is absorbed. In layman's terms the total amount of energy is a loss (it takes more energy to start the reaction than what you get out of it) so the total energy is a negative net result. For an overall gain in the net result see [[Exergonic reaction\|Exergonic Reaction]].

			Under constant temperature and constant pressure conditions, this means that the change in the standard [[Gibbs free energy]] would be positive

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			for the reaction at [[standard state]] (i.e. at standard pressure (1 [[Bar (unit)\|bar]]), and standard concentrations (1 [[Concentration#Molarity\|molar]]) of all the reagents).

			== Equilibrium constant ==

			The [[equilibrium constant]] for the reaction is related to Δ''G''° by the relation:

			:<math>K = e^{-\frac{\Delta G^\circ}{RT}}</math>

			where ''T'' is the [[absolute temperature]] and ''R'' is the [[gas constant]]. A positive value of Δ''G''° therefore implies

			:<math>K < 1 \,</math>

			so that starting from molar stoichiometric quantities such a reaction would move backwards toward equilibrium, not forwards.

			Nevertheless, endergonic reactions are quite common in nature, especially in [[biochemistry]] and [[physiology]]. Examples of endergonic reactions in cells include [[protein synthesis]], and the [[Na+/K+-ATPase\|Na<sup>+</sup>/K<sup>+</sup> pump]] which drives [[action potential\|nerve conduction]] and [[muscle contraction]].

			== Making Endergonic reactions happen ==

			Endergonic reactions can be achieved if they are either ''pulled'' or ''pushed'' by an [[exergonic]] (stability increasing, negative change in Free Energy) process.

			=== Pull ===

			Reagents can be ''pulled'' through an endergonic reaction, if the reaction products are cleared rapidly by a subsequent exergonic reaction. The concentration of the products of the endergonic reaction thus always remains low, so the reaction can proceed.

			A classic example of this might be the first stage of a reaction which proceeds via a [[transition state]]. The process of getting to the top of the [[activation energy\|activation energy barrier]] to the transition state is endergonic. However, the reaction can proceed because having reached the transition state, it rapidly evolves via an exergonic process to the more stable final products.

			=== Push ===

			Endergonic reactions can be ''pushed'' by coupling them to another reaction which is strongly exergonic, through a shared intermediate.

			This is often how biological reactions proceed. For example, on its own the reaction
			:<math> X + Y \longrightarrow XY</math>
			may be too endergonic to occur. However it may be possible to make it occur by coupling it to a strongly exergonic reaction – such as, very often, the decomposition of [[Adenosine triphosphate\|ATP]] into [[Adenosine diphosphate\|ADP]] and inorganic phosphate ions, ATP → ADP + P<sub>i</sub>, so that
			:<math> X + \mathit{ATP} \longrightarrow \mathit{XP} + \mathit{ADP}</math>
			:<math> \mathit{XP} + Y \longrightarrow \mathit{XY} + P_i</math>
			This kind of reaction, with the ATP decomposition supplying the free energy needed to make an endergonic reaction occur, is so common in cell biochemistry that ATP is often called the "universal energy currency" of all living organisms.

			==See also==
			*[[Endergonic]]
			*[[Exergonic]]
			*[[Exergonic reaction]]
			*[[Exothermic]]
			*[[Endothermic]]
			*[[Exothermic reaction]]
			*[[Endothermic reaction]]
			*[[Warm-blooded\|Endotherm]]
			*[[Warm-blooded\|Exotherm]]

			[[Category:Thermochemistry]]

en>Mbeychok: /* Temperature */ Using R as the "compression" ratio might lead to confusion with the universal gas constant R.

2012-07-31T16:05:13Z

Temperature: Using R as the "compression" ratio might lead to confusion with the universal gas constant R.

New page

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