Otto Henry Louis Le Chateau de Montpellier in chemistry to predict the direction of change will rel

In reaction, chemical equilibrium (UK: Chemical equilibrium) is a state where the concentration of precursor substances and products can not be changed even over time. We are called chemistry is in balance. (Equilibrium) the implementation of drug interactions is not ended, but the system continues to change over time is called dynamic equilibrium (dynamic equilibrium).
The concept of chemical equilibrium Was developed after a study of Claude Louis Ballet Barre Thomas (Claude Louis Berthollet) French chemist. Found that some chemical reaction is reversible (reversible reaction) in chemical equilibrium. The reaction rate forward (forward reaction) is equal to the rate of reaction backward (backward or reverse reaction), the following equation. Express chemical equilibrium of the reaction between the substance A and B substances, a chemical substance S and T, where α, β, σ, and τ is the correlation coefficient. (Stoichiometric coefficient) of such reactions.
If the reaction forward too. The concentration of precursor substances B แฃa A lot less. Maybe, in other words, nh3 is there a complete reaction (reaction completeness) or if the reverse reaction occurs very well, making the concentration of the substance A and substance B in the concentration of S and T, very little can be said. That reaction was not complete, so the balance can not describe chemical reactions in the completion of the reaction. This calculation involves Constant chemistry (chemical equilibrium: nh3 K) the equilibrium constant [change].
In a typical nh3 chemical reaction is reversible following \ alpha A + \ beta B ... \ rightleftharpoons \ rho R + \ sigma S ... constant dynamic equilibrium. (KStrikeO.png) is defined by the Union of Pure and Applied Chemistry International Chemistry (IUPAC) [2] [3] as follows: K ^ {\ ominus} = {\ frac {{\ {R \}} ^ {\ rho}. {\ {S \}} ^ {\ sigma} ...} {{\ {A \}} ^ {\ alpha} {\ {B \}} ^ {\ beta} ...}} on {A} is ACTIVITY. City (activity) of substances A, {B} is the activity of the compound B, ... The relationship above. nh3 Gibbs free energy change is considered (Gibbs free energy), but in practice. We used the concentration of substances such as [A], [B], ... rather than using the activity and concentration quotient. (Concentration quotient, Kc) than KStrikeO.png equation.
K_ {c} = {\ frac {{[R]} ^ {\ rho} {[S]} ^ {\ sigma} ...} {{[A]} ^ {\ alpha} {[B]} ^ {\. beta} ...}} When Kc is a constant balance of thermo dynamics divided by the quotient of the activity coefficient (quotient of activity coefficients) when one is equal to that Kc = KStrikeO.png sample chemistry. The [Edit]
Acid - base [edit] nh3 acid - base or weak acid which is a reaction to that. The disintegration of weak acid or weak, are very important. The equilibrium constants nh3 of reactions referred to acid dissolution. Dissociation constant of acid (acid dissociation constant, Ka) HA A- + H +.
By definition, the chemistry of this constant indicates the completion of the dissolution of the acid. The strength of the acid or tell it. Normally, the steady disintegration of acid is very small. Therefore, expressed in terms of the pKa is defined as the -log (Ka) The following table shows an example of the steady disintegration of some acid balance pKa H3PO4 H2PO4- + H + pKa1 = 2.15 H2PO4- . HPO42- nh3 + H + pKa2 = 7.20 HPO42- PO43- + H + pKa3 = 12.37 [VO2 (H2O) 4] + H3VO4 + H + + 2H2O pKa1 = 4.2 H3VO4 H2VO4- + H + pKa2 = 2.60 H2VO4- HVO42- + H +. pKa3 = 7.92 HVO42- VO43- + H + pKa4 = 13.27.
Equilibrium Solubility The melting of the ionic compound in water was less then an ionized. In chemical equilibrium solubility of water-soluble salts, such as calcium sulfate. As for the following {\ mathrm {CaSO}} _ {4} (s) \ rightleftharpoons {\ mbox {Ca}} ^ {{2 +}} (aq) + {\ mbox {SO}} _ {4. } ^ {{2 -}} (aq) \, the constant melting the thermo dynamics of calcium sulfate is as follows K ^ {\ ominus} = {\ frac {\ left \ {{\ mbox. {Ca}} ^ {{2 +}} (aq) \ right \} \ left \ {{\ mbox {SO}} _ {4} ^ {{2 -}} (aq) \ right \}} {\. left \ {{\ mbox {CaSO}} _ {4} (s) \ right \}}} = \ left \ {{\ mbox {Ca}} ^ {{2 +}} (aq) \ right \} \. left \ {{\ mbox {SO}} _ {4} ^ {{2 -}} (aq) \ right \} When KStrikeO.png constant melting of the thermo dynamics. And calculated nh3 using the activity of the ions in a solid value system, however the activity of one, and when we consider the concentration of ions is called constant. The constant multiplier effect ion (ionic solubility product: Ksp) K _ {{{\ mathrm {sp}}}} = \ left [{\ mbox {Ca}} ^ {{2 +}} (aq) \ right] nh3 \. left [{\ mbox {SO}} _ {4} ^ {{2 -}} (aq) \ right]. \,.
Otto Henry Louis Le Chateau de Montpellier in chemistry to predict the direction of change will rely on chemistry. The Le Chateau de Montpellier (Le Chatelier's principle), which was proposed by a French chemist named Otto Henry Louis Le Chateau de Montpellier (Henri Louis Le Châtelier) In principle this with matter.
This reaction nh3 enthalpy, ΔH = -46,11 kJ / mol, which is an exothermic reaction. Reducing the temperature will disturb the balance by reducing heat energy. The system will adjust to the heat balance by moving forward. The system nh3 has a concentration of ammonia increased. The following table shows the Kc that change with temperature.
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