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In [[chemistry]], a '''reaction quotient: Q<sub>r</sub>''' is a function of the [[activity (chemistry)|activities]] or [[concentration]]s of the chemical species involved in a chemical reaction. In the special case that the reaction is at [[chemical equilibrium|equilibrium]] the reaction quotient is constant and equal to the [[equilibrium constant]] which appears in the expression of the [[law of mass action]]. | |||
A general chemical reaction in which α moles of a reactant A and β moles of a reactant B react to give σ moles of a product S and τ moles of a product T can be written as | |||
:αA + βB {{eqm}} σS + τT | |||
The reaction is written as an equilibrium even though in many cases it may appear to have gone to completion. When a mixture of A and B is made up and the reaction is allowed to occur, the reaction quotient, ''Q<sub>r</sub>'', is defined as:<ref>{{cite book | author=Zumdahl, Steven; Zumdahl, Susan | title=Chemistry 6th Edition| publisher=Houghton Mifflin Company | year=2003 | isbn=0-618-22158-1}}</ref> | |||
:<math>Q_r = \frac{\left\{S_t\right\}^\sigma \left\{T_t\right\}^\tau }{\left\{A_t\right\}^\alpha \left\{B_t\right\}^\beta } </math> | |||
where {''X''<sub>t</sub>} denotes the ''instantaneous'' [[activity (chemistry)|activity]]<ref>Under certain circumstances (see [[chemical equilibrium]]) each activity term such as {''A''} may be replaced by a concentration term, [''A'']. Both the reaction quotient and the equilibrium constant are then concentration quotients.</ref> of a species X at time, t. | |||
A compact general definition is (where П<sub>j</sub> is the product across all j-indexed variables, and idem for П<sub>i</sub>): | |||
:<math>Q_r=\frac{\prod_j a_{j(t)}^{\nu_j}}{\prod_i a_{i(t)}^{\nu_i}}</math> | |||
where the numerator is a product of reaction product activities, ''a<sub> j</sub>'', each raised to the power of a [[stoichiometric coefficient]], ''ν<sub> j</sub>'', and the denominator is a similar product of reactant activities. All activities refer to a time ''t''. | |||
As the reaction proceeds (assuming that there is no [[energy barrier]] to the reaction) with the passage of time the species' activities and hence the reaction quotient change. Eventually the activities become constant and the mixture is then said to be at equilibrium. An [[equilibrium constant]], ''K'', can be expressed symbolically as | |||
:'''K''' = '''Q<sub>r</sub>''' (t=∞) | |||
though equilibrium will be effectively reached in a finite time in most reactions. | |||
==External links== | |||
Reaction quotient tutorials | |||
*[http://elchem.kaist.ac.kr/vt/chem-ed/courses/equil/intro/reactquo.htm tutorial I] | |||
*[http://www.chem.purdue.edu/gchelp/howtosolveit/Equilibrium/Reaction_Quotient.htm tutorial II] | |||
*[http://www.cartage.org.lb/en/themes/sciences/chemistry/Miscellenous/Helpfile/Equilibrium/ReactionQuotient.htm tutorial III] | |||
==References== | |||
{{reflist}} | |||
{{Chemical equilibria}} | |||
[[Category:Equilibrium chemistry]] | |||
[[Category:Physical chemistry]] | |||
Revision as of 07:01, 16 December 2013
In chemistry, a reaction quotient: Qr is a function of the activities or concentrations of the chemical species involved in a chemical reaction. In the special case that the reaction is at equilibrium the reaction quotient is constant and equal to the equilibrium constant which appears in the expression of the law of mass action.
A general chemical reaction in which α moles of a reactant A and β moles of a reactant B react to give σ moles of a product S and τ moles of a product T can be written as
- αA + βB Template:Eqm σS + τT
The reaction is written as an equilibrium even though in many cases it may appear to have gone to completion. When a mixture of A and B is made up and the reaction is allowed to occur, the reaction quotient, Qr, is defined as:[1]
where {Xt} denotes the instantaneous activity[2] of a species X at time, t. A compact general definition is (where Пj is the product across all j-indexed variables, and idem for Пi):
where the numerator is a product of reaction product activities, a j, each raised to the power of a stoichiometric coefficient, ν j, and the denominator is a similar product of reactant activities. All activities refer to a time t.
As the reaction proceeds (assuming that there is no energy barrier to the reaction) with the passage of time the species' activities and hence the reaction quotient change. Eventually the activities become constant and the mixture is then said to be at equilibrium. An equilibrium constant, K, can be expressed symbolically as
- K = Qr (t=∞)
though equilibrium will be effectively reached in a finite time in most reactions.
External links
Reaction quotient tutorials
References
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My blog: http://www.primaboinca.com/view_profile.php?userid=5889534 - ↑ Under certain circumstances (see chemical equilibrium) each activity term such as {A} may be replaced by a concentration term, [A]. Both the reaction quotient and the equilibrium constant are then concentration quotients.