“mass action”的概念、定义、翻译、参考文献-科学参考

mass action

Physics

The law of mass action states that the rate at which a chemical reaction takes place at a given temperature is proportional to the product of the active masses of the reactants. The active mass of a reactant is taken to be its molar concentration. For example, for a reaction

$x A + y B \to products$

the rate is given by

$R = k {[A]}^{x} {[B]}^{y}$

where k is the rate constant. The principle was introduced by C. M. Guldberg and P. Waage in 1863. It is strictly correct only for ideal gases. In real cases activities can be used.

Chemistry

The law of mass action states that the rate at which a chemical reaction takes place at a given temperature is proportional to the product of the active masses of the reactants. The active mass of a reactant is taken to be its molar concentration. For example, for a reaction
$x A + y B \to products$
The rate is given by
$R = k {[A]}^{x} {[B]}^{y},$
where k is the rate constant. The principle was introduced by Cato Maximilian Guldberg (1836–1902) and Peter Waage (1833–1900) in 1863. It is strictly correct only for ideal gases. In real cases activities can be used. See also equilibrium constant.

单词	mass action
释义	mass action Physics The law of mass action states that the rate at which a chemical reaction takes place at a given temperature is proportional to the product of the active masses of the reactants. The active mass of a reactant is taken to be its molar concentration. For example, for a reaction $x A + y B \to products$ the rate is given by $R = k {[A]}^{x} {[B]}^{y}$ where k is the rate constant. The principle was introduced by C. M. Guldberg and P. Waage in 1863. It is strictly correct only for ideal gases. In real cases activities can be used. Chemistry The law of mass action states that the rate at which a chemical reaction takes place at a given temperature is proportional to the product of the active masses of the reactants. The active mass of a reactant is taken to be its molar concentration. For example, for a reaction $x A + y B \to products$ The rate is given by $R = k {[A]}^{x} {[B]}^{y},$ where k is the rate constant. The principle was introduced by Cato Maximilian Guldberg (1836–1902) and Peter Waage (1833–1900) in 1863. It is strictly correct only for ideal gases. In real cases activities can be used. See also equilibrium constant.
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