均质和异质均衡之间的区别

在我们的日常生活中，我们会目睹铁锈、烧纸、凝乳发酸、产生臭氧等几种反应。许多这些反应需要存在不同相的成分，例如固体铁与气态氧反应生成固体氧化铁，我们称之为生锈。类似地，气态氢和气态氧结合形成液态水。必须处理此类反应是一项耗时的工作。当组件处于同一阶段时，它们的交互很容易理解；但是，当组件处于不同阶段时，交互变得更加复杂。

均质和异质平衡

为了简化困难并掌握概念，我们将此类反应分为两类：均相反应，其中所涉及的组分存在于同一相中，以及非均相反应，其中所涉及的组分存在于不同相中。处理这两种反应的方法以及确定平衡状态的方法不同。

所有产物和反应物具有相同相的反应。例如，所有的产物和反应物都可以是气体，或者所有的产物和反应物都可以是液体。平衡反应是在反应物和产物的浓度保持不变的情况下可以逆转和前进的反应。

平衡是一种化学反应状态，其中正向和反向反应的速率相同。此外，有两种形式的平衡：均质平衡和异质平衡。单相中的均匀平衡定义为均匀混合物（反应物和产物在单一溶液中）。请记住，反应物在等式的左侧，而产物在等式的右侧。结果，溶质之间的反应对应于单一的均质平衡。另一方面，非均相平衡是产物和反应物以两相或多相存在的反应体系。

均匀平衡可以进一步分为两种类型。第一类产物中的分子数与该特定方程式中反应物中的分子数相同。举个例子：

N ₂ (g)+O ₂ (g) ⇌ 2NO (g)

从上面的例子中，我们可以看到右侧有两个反应物分子（每个分子一个）和两个产物分子。在齐次平衡方程的第二类中，会发生相反的事件。产物的分子数不等于或等于反应物的分子数。举个例子：

2SO ₂ (g)+O ₂ (g) ⇌ 2SO ₃ (g)

从前面的例子中我们可以看出，反应中只有三分子反应物和两分子产物。溶质在液体溶液中的反应属于均相平衡中的一种均相平衡，所涉及的化学物种可以是分子、离子或两者的混合物。

Difference between K_C and K_P

The two equilibrium constants are distinguished by the fact that they are applied to different concentrations. K_P denotes the equilibrium constant at partial pressure during a reaction. These values can be calculated using the reactant and product values, the equations, and the specific values of those formulae. A relationship exists between the two equilibrium constants, which is shown below:

K_P = K_C(RT)^Δn

均质和异质平衡之间的差异

• 平衡被定义为反应物和产物的浓度恒定的情况。均质平衡和异质平衡是两种类型的平衡。均相平衡和异相平衡的主要区别在于非均相平衡，即反应物和产物处于物质的同一相，但在异相平衡中，它们处于不同相。
• 此外，在确定均相平衡的平衡常数时，我们必须包括所有反应物和产物的浓度；但是，在确定非均相平衡的平衡常数时，我们必须排除固体和纯液体的浓度，并使用其他反应物和产物的浓度。作为例证，
  • 2SO ₂ (g) + O ₂ (g) ⇌ 2SO ₃ (g)是均相平衡，并且
  • O ₂ (g) + 2C(s) ⇌ 2CO(g)是异质平衡的一个例子。
• 简而言之，平衡是反应物和产物的浓度保持不变的情况。均质平衡和异质平衡是两种类型的平衡。均相平衡和异相平衡的主要区别在于非均相平衡，即反应物和产物处于物质的同一相，但在异相平衡中，它们处于不同相。此外，均相平衡的平衡常数包括所有反应物和产物浓度，而非均相平衡的平衡常数必须忽略固体和纯液体浓度。

示例问题

问题1：异质均衡是什么意思？

回答：

The heterogeneous equilibrium refers to a system in which the reactants and products exist in two or more phases. The system’s phases are any combination of liquids, gases, solids, and solutions. It is vital to remember that pure liquids and solids cannot appear as equilibrium constant expressions when dealing with heterogeneous equilibrium.

问题2：缓冲溶液是什么意思？

回答：

Buffer solutions are composed of either a weak base and its conjugate acid or a weak acid and its conjugate base. When extra ions are introduced to a buffer solution, the pH of the solution changes. According to Le Chatelier’s principle, when more ions are introduced, the equilibrium changes and the reactions shift to favour the solid or deionized form. In the case of an acidic buffer, the concentration of the hydrogen ion reduces, and the solution produced is less acidic than a solution containing pure weak acid.

问题3：什么是平衡常数？

回答：

The word equilibrium constant can be defined as the expression that reflects the concentration of reactants and products after the chemical process has reached equilibrium. Temperature is critical in maintaining the equilibrium constant within the reactions. If the temperature remains constant, the equilibrium remains constant as well. This is evident throughout the equation, and it ultimately plays a critical role in maintaining a constant balance.

问题4：均质混合物和非均质混合物有什么区别？

回答：

When viewed at a macroscopic level, homogeneous mixes are frequently thought to be indistinguishable from the pure substance. The reaction that occurs between the solutes is part of a single homogeneous equilibrium. Sugar, salt, water, dye, air, and blood are examples of homogeneous mixes. A heterogeneous mixture has a distinct identifying quality in which the various components of the combination can be seen. It is a reaction system in which the reactants and products are found in two or more phases. Pizza, cookies, rocks, and other such items are examples of heterogeneous mixtures.

问题5：共离子效应是什么意思及其作用？

回答：

The common ion effect depicts the changes that occur when ions are injected into a solution containing the same ion. When common ions are added to a solution, the solubility of a molecule decreases due to a shift in the equilibrium. The common ion effect is crucial in the modulation of buffers. A buffering solution contains either an acid or a base, either of which is accompanied by its conjugate counterpart. The pH of the solution changes as additional conjugate ions are added. This effect must be considered when evaluating solution equilibrium when common ions are introduced.