Equilibrium - Revision history

Nnjm2 at 09:23, 10 December 2018

2018-12-10T09:23:13Z

← Older revision		Revision as of 09:23, 10 December 2018
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	For the reaction: v<sub>a</sub>A + v<sub>b</sub>B ⇌ v<sub>c</sub>C + v<sub>d</sub>D, where v<sub>a</sub>, v<sub>b</sub>, v<sub>c</sub> and v<sub>d</sub> represent the stoichiometry factors of the form ‘products/reactants’:		For the reaction: v<sub>a</sub>A + v<sub>b</sub>B ⇌ v<sub>c</sub>C + v<sub>d</sub>D, where v<sub>a</sub>, v<sub>b</sub>, v<sub>c</sub> and v<sub>d</sub> represent the stoichiometry factors of the form ‘products/reactants’:

	K<sub>c</sub> = [C]<sup>v<sub>c</sub></sup>[D]<sup>v<sub>d</sub></sup> / [A]<sup>v<sub>a</sub></sup>[B]<sup>v</sup>'''<sup><sub>b</sub></sup>'''<ref>Murphy, B.and Hathaway, C. A working method approach for introductory physical chemistry calculations numerical and graphical problem solving. Cambridge : Royal Society of Chemistry. 1997</ref>.		K<sub>c</sub> = [C]<sup>v<sub>c</sub></sup>[D]<sup>v<sub>d</sub></sup> / [A]<sup>v<sub>a</sub></sup>[B]<sup>v</sup>'''<sup><sub>b</sub></sup>'''<ref>Murphy, B. and Hathaway, C. A working method approach for introductory physical chemistry calculations numerical and graphical problem solving. Cambridge : Royal Society of Chemistry. 1997</ref>.

	=== References ===		=== References ===

	<references />		<references />

Nnjm2 at 09:23, 10 December 2018

2018-12-10T09:23:00Z

← Older revision		Revision as of 09:23, 10 December 2018
Line 11:		Line 11:
	For the reaction: v<sub>a</sub>A + v<sub>b</sub>B ⇌ v<sub>c</sub>C + v<sub>d</sub>D, where v<sub>a</sub>, v<sub>b</sub>, v<sub>c</sub> and v<sub>d</sub> represent the stoichiometry factors of the form ‘products/reactants’:		For the reaction: v<sub>a</sub>A + v<sub>b</sub>B ⇌ v<sub>c</sub>C + v<sub>d</sub>D, where v<sub>a</sub>, v<sub>b</sub>, v<sub>c</sub> and v<sub>d</sub> represent the stoichiometry factors of the form ‘products/reactants’:

	K<sub>c</sub> = [C]<sup>v<sub>c</sub></sup>[D]<sup>v<sub>d</sub></sup> / [A]<sup>v<sub>a</sub></sup>[B]<sup>v</sup>'''<sup><sub>b</sub></sup>'''~~<sup><sub>~~<ref>Murphy, B. ~~&amp;amp;amp;amp;~~ Hathaway, C. A working method approach for introductory physical chemistry calculations numerical and graphical problem solving. Cambridge : Royal Society of Chemistry. 1997</ref>.~~</sub></sup>~~		K<sub>c</sub> = [C]<sup>v<sub>c</sub></sup>[D]<sup>v<sub>d</sub></sup> / [A]<sup>v<sub>a</sub></sup>[B]<sup>v</sup>'''<sup><sub>b</sub></sup>'''<ref>Murphy, B.and Hathaway, C. A working method approach for introductory physical chemistry calculations numerical and graphical problem solving. Cambridge : Royal Society of Chemistry. 1997</ref>.

	=== ~~<sup><sub></sub></sup>~~References ===		=== References ===

	<references />		<references />

Nnjm2 at 09:22, 10 December 2018

2018-12-10T09:22:29Z

← Older revision		Revision as of 09:22, 10 December 2018
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	~~'''~~Equilibrium~~'''~~ (⇌) is achieved when the concentration of the ~~'''~~forward rate~~'''~~ of reaction and the ~~'''~~reverse rate~~'''~~ of reaction are ~~'''~~equal~~'''~~.		Equilibrium (⇌) is achieved when the concentration of the forward rate of reaction and the reverse rate of reaction are equal.

	It does not mean that the reaction stops when the equilibrium is achieved. In contrast, the reaction is continued and the rate of the products being formed is equal to the rate of the reactants being converted back.		It does not mean that the reaction stops when the equilibrium is achieved. In contrast, the reaction is continued and the rate of the products being formed is equal to the rate of the reactants being converted back.
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	K<sub>c</sub> = [C][D] / [A][B]		K<sub>c</sub> = [C][D] / [A][B]

	~~'''~~K<sub>c</sub> - the equilibrium constant~~'''~~, a characteristic of a given reaction.		K<sub>c</sub> - the equilibrium constant, a characteristic of a given reaction.

	For the reaction: v<sub>a</sub>A + v<sub>b</sub>B ⇌ v<sub>c</sub>C + v<sub>d</sub>D, where v<sub>a</sub>, v<sub>b</sub>, v<sub>c</sub> and v<sub>d</sub> represent the stoichiometry factors of the form ‘products/reactants’:		For the reaction: v<sub>a</sub>A + v<sub>b</sub>B ⇌ v<sub>c</sub>C + v<sub>d</sub>D, where v<sub>a</sub>, v<sub>b</sub>, v<sub>c</sub> and v<sub>d</sub> represent the stoichiometry factors of the form ‘products/reactants’:

	~~'''~~K<sub>c</sub> = [C]<sup>v<sub>c</sub></sup>[D]<sup>v<sub>d</sub></sup> / [A]<sup>v<sub>a</sub></sup>[B]<sup>v<sub>b</sub></sup>'''<sup><sub><ref>Murphy, B. &amp;amp;amp; Hathaway, C. A working method approach for introductory physical chemistry calculations numerical and graphical problem solving. Cambridge : Royal Society of Chemistry. 1997</ref></sub></sup>		K<sub>c</sub> = [C]<sup>v<sub>c</sub></sup>[D]<sup>v<sub>d</sub></sup> / [A]<sup>v<sub>a</sub></sup>[B]<sup>v</sup>'''<sup><sub>b</sub></sup>'''<sup><sub><ref>Murphy, B. &amp;amp;amp;amp; Hathaway, C. A working method approach for introductory physical chemistry calculations numerical and graphical problem solving. Cambridge : Royal Society of Chemistry. 1997</ref>.</sub></sup>

			=== <sup><sub></sub></sup>References ===

			<references />

180326813 at 23:51, 9 December 2018

2018-12-09T23:51:37Z

← Older revision		Revision as of 23:51, 9 December 2018
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	For the reaction: v<sub>a</sub>A + v<sub>b</sub>B ⇌ v<sub>c</sub>C + v<sub>d</sub>D, where v<sub>a</sub>, v<sub>b</sub>, v<sub>c</sub> and v<sub>d</sub> represent the stoichiometry factors of the form ‘products/reactants’:		For the reaction: v<sub>a</sub>A + v<sub>b</sub>B ⇌ v<sub>c</sub>C + v<sub>d</sub>D, where v<sub>a</sub>, v<sub>b</sub>, v<sub>c</sub> and v<sub>d</sub> represent the stoichiometry factors of the form ‘products/reactants’:

	'''K<sub>c</sub> = [C]<sup>v<sub>c</sub></sup>[D]<sup>v<sub>d</sub></sup> / [A]<sup>v<sub>a</sub></sup>[B]<sup>v<sub>b</sub></sup>'''<sup><sub><ref>Murphy, B. &amp;amp; Hathaway, C. A working method approach for introductory physical chemistry calculations numerical and graphical problem solving. Cambridge : Royal Society of Chemistry. 1997</ref></sub></sup>		'''K<sub>c</sub> = [C]<sup>v<sub>c</sub></sup>[D]<sup>v<sub>d</sub></sup> / [A]<sup>v<sub>a</sub></sup>[B]<sup>v<sub>b</sub></sup>'''<sup><sub><ref>Murphy, B. &amp;amp;amp; Hathaway, C. A working method approach for introductory physical chemistry calculations numerical and graphical problem solving. Cambridge : Royal Society of Chemistry. 1997</ref></sub></sup>

180326813 at 23:50, 9 December 2018

2018-12-09T23:50:24Z

← Older revision		Revision as of 23:50, 9 December 2018
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	'''K<sub>c</sub> - the equilibrium constant''', a characteristic of a given reaction.		'''K<sub>c</sub> - the equilibrium constant''', a characteristic of a given reaction.

	~~In general, for~~ the reaction: v<sub>a</sub>A + v<sub>b</sub>B ⇌ v<sub>c</sub>C + v<sub>d</sub>D, where v<sub>a</sub>, v<sub>b</sub>, v<sub>c</sub> and v<sub>d</sub> represent the stoichiometry factors of the form ‘products/reactants’:		For the reaction: v<sub>a</sub>A + v<sub>b</sub>B ⇌ v<sub>c</sub>C + v<sub>d</sub>D, where v<sub>a</sub>, v<sub>b</sub>, v<sub>c</sub> and v<sub>d</sub> represent the stoichiometry factors of the form ‘products/reactants’:

	'''K<sub>c</sub> = [C]<sup>v<sub>c</sub></sup>[D]<sup>v<sub>d</sub></sup> / [A]<sup>v<sub>a</sub></sup>[B]<sup>v<sub>b</sub></sup>'''<sup><sub><ref>Murphy, B. &amp; Hathaway, C. A working method approach for introductory physical chemistry calculations numerical and graphical problem solving. Cambridge : Royal Society of Chemistry. 1997</ref></sub></sup>		'''K<sub>c</sub> = [C]<sup>v<sub>c</sub></sup>[D]<sup>v<sub>d</sub></sup> / [A]<sup>v<sub>a</sub></sup>[B]<sup>v<sub>b</sub></sup>'''<sup><sub><ref>Murphy, B. &amp;amp; Hathaway, C. A working method approach for introductory physical chemistry calculations numerical and graphical problem solving. Cambridge : Royal Society of Chemistry. 1997</ref></sub></sup>

180326813 at 23:48, 9 December 2018

2018-12-09T23:48:38Z

← Older revision		Revision as of 23:48, 9 December 2018
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	Equilibrium (⇌) is achieved when the concentration of ~~thr~~ forward rate of reaction and the reverse rate of reaction are equal.~~ ~~It does not mean that the reaction stops when the equilibrium is achieved. In contrast, the reaction is continued and the rate of the products being formed is equal to the rate of the reactants being converted back.		'''Equilibrium''' (⇌) is achieved when the concentration of the '''forward rate''' of reaction and the '''reverse rate''' of reaction are '''equal'''.

			It does not mean that the reaction stops when the equilibrium is achieved. In contrast, the reaction is continued and the rate of the products being formed is equal to the rate of the reactants being converted back.

			For example, for the reaction, A + B ⇌ C + D, at equilibrium:

			K<sub>c</sub> = [C][D] / [A][B]

			'''K<sub>c</sub> - the equilibrium constant''', a characteristic of a given reaction.

			In general, for the reaction: v<sub>a</sub>A + v<sub>b</sub>B ⇌ v<sub>c</sub>C + v<sub>d</sub>D, where v<sub>a</sub>, v<sub>b</sub>, v<sub>c</sub> and v<sub>d</sub> represent the stoichiometry factors of the form ‘products/reactants’:

			'''K<sub>c</sub> = [C]<sup>v<sub>c</sub></sup>[D]<sup>v<sub>d</sub></sup> / [A]<sup>v<sub>a</sub></sup>[B]<sup>v<sub>b</sub></sup>'''<sup><sub><ref>Murphy, B. &amp; Hathaway, C. A working method approach for introductory physical chemistry calculations numerical and graphical problem solving. Cambridge : Royal Society of Chemistry. 1997</ref></sub></sup>

170263289 at 02:12, 6 December 2017

2017-12-06T02:12:00Z

← Older revision		Revision as of 02:12, 6 December 2017
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	Equilibrium (⇌) is achieved when the forward rate of reaction and the reverse rate of reaction are equal. It does not mean that the reaction stops when the equilibrium is achieved. In contrast, the reaction is continued and the rate of the products being formed is equal to the rate of the reactants being converted back.		Equilibrium (⇌) is achieved when the concentration of thr forward rate of reaction and the reverse rate of reaction are equal. It does not mean that the reaction stops when the equilibrium is achieved. In contrast, the reaction is continued and the rate of the products being formed is equal to the rate of the reactants being converted back.

Nnjm2 at 10:11, 23 November 2013

2013-11-23T10:11:59Z

← Older revision		Revision as of 10:11, 23 November 2013
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	~~''' ~~Equilibrium~~'''~~ (⇌) is achieved when the forward rate of reaction and the reverse rate of reaction are equal. It does not mean that the reaction stops when the equilibrium is achieved. In contrast, the reaction is continued and the rate of the products being formed is equal to the rate of the reactants being converted back.		Equilibrium (⇌) is achieved when the forward rate of reaction and the reverse rate of reaction are equal. It does not mean that the reaction stops when the equilibrium is achieved. In contrast, the reaction is continued and the rate of the products being formed is equal to the rate of the reactants being converted back.

140001691 at 09:57, 23 November 2013

2013-11-23T09:57:12Z

← Older revision		Revision as of 09:57, 23 November 2013
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	''' Equilibrium''' (⇌) is achieved when the forward rate of reaction and the reverse rate of reaction are equal.		''' Equilibrium''' (⇌) is achieved when the forward rate of reaction and the reverse rate of reaction are equal. It does not mean that the reaction stops when the equilibrium is achieved. In contrast, the reaction is continued and the rate of the products being formed is equal to the rate of the reactants being converted back.

100682218: Created page with "''' Equilibrium''' (⇌) is achieved when the forward rate of reaction and the reverse rate of reaction are equal. "

2011-12-02T10:26:42Z

Created page with "''' Equilibrium''' (⇌) is achieved when the forward rate of reaction and the reverse rate of reaction are equal. "

New page

''' Equilibrium''' (⇌) is achieved when the forward rate of reaction and the reverse rate of reaction are equal. 