“dissociation”的概念、定义、翻译、参考文献-科学参考

dissociation

Chemistry

The breakdown of a molecule, ion, etc., into smaller molecules, ions, etc. An example of dissociation is the reversible reaction of hydrogen iodide at high temperatures
$2 HI (g) ⇌ H_{2} {(g) + I}_{2} (g)$
The equilibrium constant of a reversible dissociation is called the dissociation constant. The term ‘dissociation’ is also applied to ionization reactions of acids and bases in water; for example
${HCN + H}_{2} O ⇌ H_{3} O^{+} + {C N}^{-}$
which is often regarded as a straightforward dissociation into ions
$HCN ⇌ H^{+} + {CN}^{-}$
The equilibrium constant of such a dissociation is called the acid dissociation constant or acidity constant, given by
$K_{a} {= [H}^{+} {] [A}^{-}] / [HA]$
for an acid HA (the concentration of water [H₂O] can be taken as constant). K_a is a measure of the strength of the acid. Similarly, for a nitrogenous base B, the equilibrium
${B + H}_{2} O ⇌ {BH}^{+} + {OH}^{-}$
is also a dissociation; with the base dissociation constant, or basicity constant, given by
$K_{b} {= [BH}^{+} {] [OH}^{-}] / [B]$
For a hydroxide MOH,
$K_{b} = [M^{+}] [{OH}^{-}] / [MOH]$

Chemical Engineering

A reversible chemical reaction in which ionic compounds break down into smaller particles. For example, in the reversible dissociations of:
$2 H I \Leftrightarrow H_{2} + I_{2}$

the dissociation constant is constant and is given by:
$K_{d} = \frac{[H_{2}] [I_{2}]}{{[H I]}^{2}}$

The brackets denote the equilibrium concentrations. For gases, this can be expressed in partial pressures.

单词	dissociation
释义	dissociation Chemistry The breakdown of a molecule, ion, etc., into smaller molecules, ions, etc. An example of dissociation is the reversible reaction of hydrogen iodide at high temperatures $2 HI (g) ⇌ H_{2} {(g) + I}_{2} (g)$ The equilibrium constant of a reversible dissociation is called the dissociation constant. The term ‘dissociation’ is also applied to ionization reactions of acids and bases in water; for example ${HCN + H}_{2} O ⇌ H_{3} O^{+} + {C N}^{-}$ which is often regarded as a straightforward dissociation into ions $HCN ⇌ H^{+} + {CN}^{-}$ The equilibrium constant of such a dissociation is called the acid dissociation constant or acidity constant, given by $K_{a} {= [H}^{+} {] [A}^{-}] / [HA]$ for an acid HA (the concentration of water [H₂O] can be taken as constant). K_a is a measure of the strength of the acid. Similarly, for a nitrogenous base B, the equilibrium ${B + H}_{2} O ⇌ {BH}^{+} + {OH}^{-}$ is also a dissociation; with the base dissociation constant, or basicity constant, given by $K_{b} {= [BH}^{+} {] [OH}^{-}] / [B]$ For a hydroxide MOH, $K_{b} = [M^{+}] [{OH}^{-}] / [MOH]$ Chemical Engineering A reversible chemical reaction in which ionic compounds break down into smaller particles. For example, in the reversible dissociations of: $2 H I \Leftrightarrow H_{2} + I_{2}$ the dissociation constant is constant and is given by: $K_{d} = \frac{[H_{2}] [I_{2}]}{{[H I]}^{2}}$ The brackets denote the equilibrium concentrations. For gases, this can be expressed in partial pressures.
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