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Topic: Equilibrium constant

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Chemical equilibrium

Acid dissociation constant

Acidity constant

PKa

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	NationMaster.com - Encyclopedia: Equilibrium constant (Site not responding. Last check: 2007-10-13)
		The equilibrium constant is related to the Gibbs free energy through a Boltzmann distribution as: In thermodynamics the Gibbs free energy function is a thermodynamic potential and is therefore a state function of a thermodynamic system.
		The gas constant (also known as the universal or ideal gas constant, usually denoted by symbol R) is a physical constant used in equations of state to relate various groups of state functions to one another.
		Therefore, the equilibrium constant is more rigorously defined by the substances activity coefficients, which are usually assumed to be equal to the molarities of solutes or equal to one for solids and solvents.
	www.nationmaster.com /encyclopedia/Equilibrium-constant (1542 words)

	Equilibrium constant - Wikipedia, the free encyclopedia
		In chemistry, the equilibrium constant is a quantity characterizing a chemical equilibrium in a chemical reaction which is a useful tool to determine the concentration of various reactants or products in a system where chemical equilibrium occurs.
		Examples include the acidity constant (the equilibrium constant for the dissociation of protons from acids) and the solubility constant (the equilibrium constant for precipitating out of solution).
		In an equilibrium between two conformers with energy difference 0, the equilibrium constant is 1 and both conformers are present in a 1:1 ratio.
	en.wikipedia.org /wiki/Equilibrium_constant (522 words)

	Chemical equilibrium - Wikipedia, the free encyclopedia
		The equilibrium position of a reaction is said to lie far to the right if, at equilibrium, nearly all the reactants are used up and far to the left if hardly any product is formed from the reactants.
		Thus, the same equilibrium constant can be found in very fast and very slow reactions, and a fast forward reaction (by itself) does not imply that the reaction equilibrium lies far to the right.
		Classical equilibria are that between the colorless nitrogen dioxide and the brown dinitrogen tetroxide and the Schlenk equilibrium.
	en.wikipedia.org /wiki/Chemical_equilibrium (711 words)

	Chemical Sciences: Form, Nominal Units, and Values of Equilibrium Constants
		There are a large number of different types of equilibrium constant which are distinguished by the specific form of equilibrium to which the constant applies and the approximations to activity made in the use of the constant.
		Equilibrium constants actually have no real units, because chemical activities are actually ratios in which the units divide out to none.
		The value of the second constant is the reciprocal (inverse) of the value of the first; the value of the third constant is the square of the value of the first.
	www.psigate.ac.uk /newsite/reference/plambeck/chem1/p01103.htm (729 words)

	APPLICATION OF EQUILIBRIUM CONSTANT
		A very high value of equilibrium constant indicates that the forward is almost complete and in other words we can say that the reactants are very unstable and they react spontaneously.
		A very small value of equilibrium constant indicates that there is very little tendency for the reaction to occur in the forward direction and in other words we can say that the reactants are very stable.
		When the value of equilibrium constant is neither very high nor very small, we conclude that the reaction occurs both in forward and backward direction and equilibrium will be attained after certain period of time.
	www.citycollegiate.com /chemical_equilibrium3.htm (417 words)

	[No title]
		At equilibrium, the concentrations of the substances participating in the equilibrium are constant.
		Notice that the value of the equilibrium constant is the same, regardless of whether the initial materials were hydrogen and iodine or the hydrogen iodide molecule or a combination of all and whether the components were present in equal or different concentrations.
		The equilibrium constant is a very useful concept, for it allows the prediction and calculation of the concentrations of the various species present in a reaction mixture at equilibrium.
	genchem.chem.wisc.edu /sstutorial/Text13/Tx134/tx134.html (1064 words)

	Rate Equilibrium (Site not responding. Last check: 2007-10-13)
		A chemical equilibrium is dynamic, implying that the forward and reverse reactions are occurring at the same rate.
		is the equilibrium constant for the reaction and is a constant value at a given temperature.
		Equilibrium constants can be used to calculate the concentrations of reactants or products at given points during the reaction, as per the following examples.
	www.scientia.org /cadonline/Chemistry/acidbase/rateequilib.ASP (560 words)

	General Equilibrium
		The equilibrium constant expression can be found by multiplying the equilibrium concentrations of the products raised to their coefficient powers and dividing by the equilibrium concentration of the reactants raided to their coefficient powers.
		Notice also that the equilibrium constant expression for Equation #2 is the reciprocal of the equilibrium constant expression for Equation #1.
		The equilibrium constants may also be used to calculate the equilibrium concentrations of the reactants and products in a chemical equation.
	www.cofc.edu /genchemlab/equilibrium.htm (558 words)

	Chemical Sciences: Chemical Equilibrium: The Different Types of Equilibrium Constants
		Equilibrium constants of all types are usually given the symbol K, and unless further qualified this symbol has no more specific meaning.
		specifies only that the equilibrium constant shall have as their nominal units, and the substances used in it shall have as their actual units, some pressure units.
		The (molar) stability constant of a complex ion is the equilibrium constant for the formation of the complex ion in a solvent from its constituent ions.
	www.psigate.ac.uk /newsite/reference/plambeck/chem1/p01104.htm (779 words)

	chemical equilibrium on Encyclopedia.com
		This equilibrium point is characterized by specific relative concentrations of reactants and products and will also be reached from the opposite direction, i.e., if one starts with hydrogen iodide and allows it to decompose into hydrogen and iodine.
		The equilibrium constant is related to the change in the standard free energy, G °, of the system by the equation Δ G ° = - RT.
		Chemical equilibrium can be defined for many types of chemical processes, such as dissociation of a weak acid in solution, solubility of slightly soluble salts, and oxidation-reduction reactions.
	www.encyclopedia.com /html/c1/chem-equi.asp (634 words)

	Chemistry : Chapter 15 : Overview (Site not responding. Last check: 2007-10-13)
		The law of mass action states that any reaction mixture eventually reaches a state (equilibrium) in which the ratio of the concentration terms of the products to the reactants, each raised to a power corresponding to the stoichiometric coefficient for that substance in the balanced chemical equation, is a characteristic value for a given temperature.
		Therefore the equilibrium constant of the reverse reaction is the reciprocal of the equilibrium constant of the forward reaction.
		In addition, the equilibrium constant for an equation that is the sum of two chemical equations is the product of the equilibrium constants of those two reactions.
	www.wwnorton.com /chemistry/overview/ch15.htm (724 words)

	Chemical Equilibrium
		Equilibrium occurs when there is a constant ratio between the concentration of the reactants and the products.
		A reaction may look "finished" when equilibrium is reached, but actually the forward and reverse reactions continue to happen at the same rate.
		Calculate the equilibrium concentrations of the three molecules and the value of K. equilibrium solution.
	www.shodor.org /UNChem/advanced/equ (1146 words)

	Chemical Equilibria
		During an dynamic equilibrium, the rate of the forward reaction equals the rate of the reverse reaction.
		Upon examining the equilibrium, one sees that there are five moles of gas particles on the left hand side of the equilibrium, while there are two moles of gas particles on the right hand side of the equilibrium.
		Thus if the equilibrium shifts to the right, the number of gas particles in the container become reduced, and the excess pressure is relieved.
	www.towson.edu /~ladon/chemeq.html (1411 words)

	Dissociation constant: Facts and details from Encyclopedia Topic (Site not responding. Last check: 2007-10-13)
		In chemistry, the equilibrium constant is a theoretically-calcucated number associated to a reaction which is an useful tool to determine the concentration...
		The dissociation constant is represented by the symbol K
		A carboxyl or carboxylic group is a functional group consisting of a carbon atom doubly bonded to an oxygen atom and single-bonded to a hydroxyl...
	www.absoluteastronomy.com /encyclopedia/d/di/dissociation_constant.htm (627 words)

	equilibrium - Hutchinson encyclopedia article about equilibrium
		In a dynamic equilibrium, in contrast, a steady state is maintained by constant, though opposing, changes.
		For example, in a sealed bottle half-full of water, the constancy of the water level is a result of molecules evaporating from the surface and condensing on to it at the same rate.
		Each molecule of the gutter bore away a molecule of heat radiating from Gringoire's loins, and the equilibrium between the temperature of his body and the temperature of the brook, began to be established in rough fashion.
	encyclopedia.farlex.com /equilibrium (295 words)

	equilibrium constants - Kc
		The equilibrium constant always has the same value (provided you don't change the temperature), irrespective of the amounts of A, B, C and D you started with.
		That is all that is left in the equilibrium constant expression.
		It covers equilibrium constant calculations starting with the most trivial cases, and gradually getting harder - up to the moderately difficult examples which may be asked in a UK A' level examination.
	www.chemguide.co.uk /physical/equilibria/kc.html (1114 words)

	CHM 1046 (Site not responding. Last check: 2007-10-13)
		To summarize the interpretation for the magnitude of the equilibrium constant:
		By definition, equilibrium implies that we have both a "forward" and a "backward" reaction in a balanced chemical equation.
		Therefore, an equilibrium constant, in the absence of information about the direction of the reaction, is ambiguous (i.e.
	wine1.sb.fsu.edu /chm1046/notes/ChmEquil/EqConst/EqConst.htm (818 words)

	Equilibrium Constant from Spectrometry
		The equilibrium constant expression for this reaction is
		In the five different equilibrium solutions, the equilibrium concentrations, and hence the equilibrium positions, are different.
		But your measured values of the equilibrium constant should be the same, within expected experimental variation.
	www.usm.maine.edu /chy/manuals/116/text/KeqSpec.html (1494 words)

	Chemical Equilibrium
		To determine the amount of each compound that will be present at equilibrium you must know the equilibrium constant.
		Le Chatelier's principle states that when a system in chemical equilibrium is disturbed by a change of temperature, pressure, or a concentration, the system shifts in equilibrium composition in a way that tends to counteract this change of variable.
		Therefore the shift caused by a change in temperature depends upon whether the reaction is exothermic or endothermic.
	library.thinkquest.org /10429/low/equil/equil.htm (452 words)

	The Net Equation: Your Online Source for Chemistry Solutions
		At equilibrium, the reaction is still proceeding on a microscopic scale, but the conversion from products to reactants exactly equals the reverse reaction.
		Note that solids are never included in an equilibrium constant (since concentrations vary in solids), nor are pure liquids for the same reason (this second rule usually applies only to water).
		If you reverse the reaction, you must take the reciprocal of the equilibrium constant (if K for one reaction were 2/7, K for the reverse would be 7/2).
	library.thinkquest.org /C004970/reactions/k.htm?tqskip1=1&tqtime=0214 (917 words)

	Untitled (Site not responding. Last check: 2007-10-13)
		This model (below) demonstrates the attainment of equilibrium in a model chemical reaction.The way in which the position of equilibrium is affected by altering the conditions is summarised by Le Chatelier's principle.
		If the conditions of a system at equilibrium are changed, the system moves in such a way as to oppose the effects of that change.
		it is possible to use the equilibrium concentration data generated by the model to calculate an equilibrium constant for the model.
	chem.salve.edu /chemistry/equilbrm.asp (459 words)

	Le Chatelier's Principle - Chemical equilibrium
		In 1864, Cato Maximilian Guldberg and Peter Waage postulated the expression for the equilibrium constant.
		The equilibrium expression for a reaction written in one direction is the reciprocal of the one for the reaction written in the reverse direction.
		The constant of equilibrium expression for the dissolution of NaCl in water is given by:
	bouman.chem.georgetown.edu /S02/lect8/lect8.htm (1365 words)

	Free energy and equilibrium (Site not responding. Last check: 2007-10-13)
		,the equilibrium constant expressed in pressure units, is the special value of Q that corresponds to the equlibrium composition.
		Notice that an equilibrium constant of unity implies a standard free energy change of zero, and that positive values of ΔG° lead to values of K less than unity.
		Measurement of an equilibrium constant is generally much easier, and often well within the capabilities of anyone who has had an introductory Chemistry course.
	www.chem1.com /acad/webtext/thermeq/TE5.html (2335 words)

	Problems in Chemical Equilibrium (Site not responding. Last check: 2007-10-13)
		The equilibrium constant for a reaction is the ratio of the forward to reverse rate constants, and is a function of temperature, only.
		The rate constant for the forward reaction is less than that of the reverse reaction.
		The synthesis of ammonia is an exothermic reaction, so the rate of product formation may increase with temperature, but the equilibrium constant, and thus the yield of the the reaction, decreases with increasing temperature.
	itl.chem.ufl.edu /2041_f00/lectures/EQprob1.html (474 words)

	Weak acid K
		In writing an equilibrium constant expression for this heterogeneous equilibrium, we leave out the concentration of the liquid water.
		The equilibrium constant for this expression is called the acid dissociation constant, K
		When the equilibrium in question occurs in solution, the chemical formulas enclosed in brackets in the equilibrium constant expression represent the molarities of the substances (moles of solute per liter of solution).
	www.mpcfaculty.net /mark_bishop/weak_acid_equilibrium.htm (579 words)

	Chapter 16: Chemical Equilibrium: General Concepts
		4. To calculate the equilibrium constant from experimental data on the percent of reaction, the concentration of the reactant that actually undergoes the process, or the equilibrium concentrations of each species in the system.
		1. When given the equilibrium constant for one balanced equation, know how to obtain the new equilibrium constant if the original equation is reversed, multiplied by a constant, or combined with other balanced equations.
		the equilibrium does shift to the left, and the concentrations of hydrogen and iodine gases are less than they were after the extra iodine was added.
	www.fairbornchempage.com /Ap/Objectives/apobj16.htm (436 words)

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