effective collision number

简明释义

有效碰撞数

英英释义

例句

1.Researchers calculated the effective collision number 有效碰撞数 to predict the outcome of the experiment.

研究人员计算了有效碰撞数 有效碰撞数 以预测实验结果。

2.The effective collision number 有效碰撞数 can vary based on the density of particles in a given volume.

在给定体积内，有效碰撞数 有效碰撞数 可以根据粒子的密度而变化。

3.The simulation showed an increase in the effective collision number 有效碰撞数 with higher temperatures.

模拟显示，随着温度升高，有效碰撞数 有效碰撞数 增加。

4.In nuclear physics, the effective collision number 有效碰撞数 is crucial for understanding reaction rates.

在核物理中，有效碰撞数 有效碰撞数 对于理解反应速率至关重要。

5.In collision theory, the effective collision number 有效碰撞数 helps determine the likelihood of a reaction occurring.

在碰撞理论中，有效碰撞数 有效碰撞数 有助于确定反应发生的可能性。

作文

In the realm of physical chemistry, the concept of effective collision number plays a crucial role in understanding reaction rates. The effective collision number refers to the number of collisions per unit time that actually lead to a chemical reaction, as opposed to all collisions that occur between molecules. This distinction is essential because not all molecular interactions result in a successful reaction; many collisions are ineffective due to various factors such as insufficient energy or incorrect orientation of the reacting species. To illustrate this concept, consider a simple reaction between two gaseous reactants A and B. When these molecules come into contact, they collide with one another. However, only those collisions that possess enough energy to overcome the activation energy barrier will result in a reaction. This means that while the total number of collisions might be high, the effective collision number could be significantly lower, depending on the conditions of the reaction, such as temperature, pressure, and concentration of the reactants.Temperature, for instance, has a profound effect on the effective collision number. As temperature increases, the kinetic energy of the molecules also increases, leading to more frequent and more energetic collisions. This increase in energy enhances the likelihood that collisions will be effective, thereby increasing the effective collision number. Consequently, reactions tend to proceed faster at higher temperatures. Similarly, increasing the concentration of reactants in a solution can lead to a higher effective collision number, as there are more molecules available to collide with each other.Another important aspect of the effective collision number is its dependence on the orientation of the colliding molecules. For a collision to be effective, the molecules must collide in a specific orientation that allows the formation of new bonds. If the orientation is incorrect, even if the collision occurs with sufficient energy, it may not lead to a reaction. Therefore, the geometry of the molecules involved also plays a significant role in determining the effective collision number.In practical applications, understanding the effective collision number can help chemists design better catalysts that facilitate reactions by lowering the activation energy or by providing a favorable environment for effective collisions. Catalysts work by providing an alternative pathway for the reaction that requires less energy, thus increasing the number of effective collisions and speeding up the reaction rate without being consumed in the process.In conclusion, the effective collision number is a fundamental concept in the study of chemical kinetics. It provides insight into why some reactions occur quickly while others do not. By considering factors such as temperature, concentration, and molecular orientation, scientists can better understand and manipulate chemical reactions to achieve desired outcomes. Ultimately, the effective collision number serves as a bridge between the microscopic world of molecular interactions and the macroscopic observations of reaction rates, making it an indispensable part of physical chemistry.

在物理化学领域，有效碰撞数的概念在理解反应速率方面发挥着至关重要的作用。有效碰撞数指的是每单位时间内实际上导致化学反应的碰撞次数，而不是分子之间发生的所有碰撞。这一区别是至关重要的，因为并非所有的分子相互作用都会导致成功的反应；许多碰撞由于各种因素（如能量不足或反应物的方向不正确）而无效。为了说明这一概念，可以考虑两个气态反应物A和B之间的简单反应。当这些分子接触时，它们会相互碰撞。然而，只有那些具有足够能量以克服活化能障碍的碰撞才会导致反应。这意味着，尽管总碰撞次数可能很高，但有效碰撞数可能会显著降低，这取决于反应的条件，如温度、压力和反应物的浓度。例如，温度对有效碰撞数有深远的影响。随着温度的升高，分子的动能也随之增加，从而导致更频繁和更有能量的碰撞。能量的增加增强了碰撞的有效性，从而提高了有效碰撞数。因此，反应在较高温度下往往进行得更快。同样，增加溶液中反应物的浓度可以导致更高的有效碰撞数，因为可供彼此碰撞的分子更多。有效碰撞数的另一个重要方面是其对碰撞分子方向的依赖。为了使碰撞有效，分子必须以特定的方向碰撞，以便形成新键。如果方向不正确，即使碰撞发生且能量充足，也可能不会导致反应。因此，涉及分子的几何形状在确定有效碰撞数方面也起着重要作用。在实际应用中，理解有效碰撞数可以帮助化学家设计更好的催化剂，通过降低活化能或提供有利于有效碰撞的环境来促进反应。催化剂通过提供一种需要更少能量的替代反应路径，增加有效碰撞的数量，加速反应速率，同时不被消耗。总之，有效碰撞数是化学动力学研究中的一个基本概念。它提供了对某些反应为何快速发生而其他反应却不发生的洞察。通过考虑温度、浓度和分子方向等因素，科学家可以更好地理解和操控化学反应，以实现预期的结果。最终，有效碰撞数在微观分子相互作用与宏观反应速率观察之间架起了一座桥梁，使其成为物理化学中不可或缺的一部分。