“chemical equilibrium”的概念、定义、翻译、参考文献-科学参考

chemical equilibrium

Chemistry

A reversible chemical reaction in which the concentrations of reactants and products are not changing with time because the system is in thermodynamic equilibrium. For example, the reversible reaction
$3 H_{2} + N_{2} ⇌ 2 {NH}_{3}$
is in chemical equilibrium when the rate of the forward reaction
$3 H_{2} + N_{2} \to 2 {NH}_{3}$
is equal to the rate of the back reaction
$2 {NH}_{3} \to 3 H_{2} + N_{2}$
See also equilibrium constant.

Chemical Engineering

A thermodynamic equilibrium between the reactants and products in a reversible chemical reaction. The balance in a reversible chemical reaction in which two chemical reactions proceed at the same rate but in opposite directions. That is, the rate of the forwards reaction is balanced by the rate of the backwards reaction. For example, in the reaction $w A + x B \leftrightarrow y C + z D$ the reactants A and B form the products C and D, which can also return to form A and B. For the balanced reaction at equilibrium, the equilibrium constant is the ratio of the molar concentrations of the products to the reactants given by:
$K_{c} = \frac{{[C]}^{y} {[D]}^{z}}{{[A]}^{w} {[B]}^{x}}$

The square brackets indicate equilibrium concentrations.

单词	chemical equilibrium
释义	chemical equilibrium Chemistry A reversible chemical reaction in which the concentrations of reactants and products are not changing with time because the system is in thermodynamic equilibrium. For example, the reversible reaction $3 H_{2} + N_{2} ⇌ 2 {NH}_{3}$ is in chemical equilibrium when the rate of the forward reaction $3 H_{2} + N_{2} \to 2 {NH}_{3}$ is equal to the rate of the back reaction $2 {NH}_{3} \to 3 H_{2} + N_{2}$ See also equilibrium constant. Chemical Engineering A thermodynamic equilibrium between the reactants and products in a reversible chemical reaction. The balance in a reversible chemical reaction in which two chemical reactions proceed at the same rate but in opposite directions. That is, the rate of the forwards reaction is balanced by the rate of the backwards reaction. For example, in the reaction $w A + x B \leftrightarrow y C + z D$ the reactants A and B form the products C and D, which can also return to form A and B. For the balanced reaction at equilibrium, the equilibrium constant is the ratio of the molar concentrations of the products to the reactants given by: $K_{c} = \frac{{[C]}^{y} {[D]}^{z}}{{[A]}^{w} {[B]}^{x}}$ The square brackets indicate equilibrium concentrations.
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