real gas

简明释义

实在气体

英英释义

例句

1.The Van der Waals equation accounts for the interactions between molecules in a real gas 真实气体.

范德瓦尔斯方程考虑了分子之间的相互作用，这在真实气体 真实气体中是很重要的。

2.In thermodynamics, we often compare ideal gases to real gas 真实气体 behavior.

在热力学中，我们经常将理想气体与真实气体 真实气体的行为进行比较。

3.The behavior of a real gas 真实气体 deviates from that of an ideal gas at high pressures.

在高压下，真实气体 真实气体的行为与理想气体的行为有所偏离。

4.When calculating pressure, it's essential to consider the properties of a real gas 真实气体.

在计算压力时，考虑真实气体 真实气体的特性是至关重要的。

5.Understanding real gas 真实气体 behavior is crucial for engineers working in chemical processes.

理解真实气体 真实气体的行为对于从事化学过程的工程师至关重要。

作文

In the study of thermodynamics and physical chemistry, we often encounter the term real gas, which refers to gases that do not behave ideally under all conditions. Unlike ideal gases, which are governed by the ideal gas law and assume that particles have no volume and do not interact with each other, real gases exhibit behaviors that can be significantly different from these assumptions, particularly at high pressures and low temperatures. Understanding the concept of real gas is crucial for various applications in science and engineering, as it helps us predict how gases will behave in real-world situations.When we talk about real gases, we must consider the intermolecular forces that come into play. In an ideal gas, the molecules are considered to be point particles with no volume and no attractive or repulsive forces acting between them. This simplification allows us to use the ideal gas law, expressed as PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature. However, in reality, all gases have some degree of intermolecular attraction, which means that when they are compressed or cooled, their behavior deviates from that predicted by the ideal gas law.For example, at high pressures, the volume occupied by the gas molecules themselves becomes significant compared to the total volume of the gas, leading to a situation where the assumptions of the ideal gas law break down. Similarly, at low temperatures, the kinetic energy of gas molecules decreases, allowing intermolecular forces to dominate, causing the gas to condense into a liquid. These phenomena illustrate the importance of recognizing that real gases do not always conform to the ideal gas law.One way to account for the behavior of real gases is through the use of equations of state, such as the Van der Waals equation. This equation introduces correction factors for both the volume occupied by gas molecules and the attractive forces between them. The Van der Waals equation is expressed as (P + a(n/V)^2)(V - nb) = nRT, where 'a' and 'b' are constants specific to each gas. By using this equation, scientists and engineers can better predict the behavior of real gases under various conditions, leading to more accurate models in chemical processes, environmental studies, and industrial applications.Moreover, understanding real gases is essential in fields such as meteorology and climate science. The behavior of atmospheric gases, including water vapor, carbon dioxide, and methane, can significantly impact weather patterns and climate change. By studying the properties of real gases, scientists can develop more reliable climate models and make informed predictions about future environmental changes.In conclusion, the concept of real gas is fundamental to our understanding of gas behavior in the real world. Unlike ideal gases, real gases take into account the volume of gas molecules and the intermolecular forces that affect their interactions. By using equations of state like the Van der Waals equation, we can gain valuable insights into the behavior of gases in various scientific and engineering contexts. Recognizing the differences between ideal and real gases allows us to make more accurate predictions and develop better technologies that rely on gas behavior, ultimately contributing to advancements in multiple fields of study.

在热力学和物理化学的研究中，我们经常遇到术语真实气体，它指的是在所有条件下不表现出理想行为的气体。与理想气体不同，理想气体遵循理想气体定律，假设粒子没有体积且彼此之间没有相互作用，而真实气体则表现出与这些假设显著不同的行为，尤其是在高压和低温下。理解真实气体的概念对于科学和工程中的各种应用至关重要，因为它帮助我们预测气体在现实世界中的行为。当我们谈论真实气体时，必须考虑到分子间作用力的影响。在理想气体中，分子被认为是没有体积的点粒子，并且没有吸引或排斥力作用于它们之间。这种简化使我们能够使用理想气体定律，其表达式为PV = nRT，其中P是压力，V是体积，n是摩尔数，R是理想气体常数，T是温度。然而，实际上，所有气体在某种程度上都有分子间的吸引力，这意味着当它们被压缩或冷却时，它们的行为会偏离理想气体定律所预测的结果。例如，在高压下，气体分子本身占据的体积相对于气体的总体积变得显著，从而导致理想气体定律的假设失效。同样，在低温下，气体分子的动能降低，使得分子间的作用力占主导地位，导致气体凝结成液体。这些现象说明了认识到真实气体并不总是符合理想气体定律的重要性。一种考虑真实气体行为的方法是使用状态方程，例如范德瓦尔斯方程。该方程引入了气体分子占据的体积和它们之间的吸引力的修正因子。范德瓦尔斯方程的表达式为(P + a(n/V)²)(V - nb) = nRT，其中'a'和'b'是特定于每种气体的常数。通过使用这个方程，科学家和工程师可以更好地预测真实气体在各种条件下的行为，从而在化学过程、环境研究和工业应用中得到更准确的模型。此外，理解真实气体在气象学和气候科学等领域也至关重要。大气气体（包括水蒸气、二氧化碳和甲烷）的行为会显著影响天气模式和气候变化。通过研究真实气体的性质，科学家可以开发出更可靠的气候模型，并对未来的环境变化做出明智的预测。总之，真实气体的概念是我们理解现实世界中气体行为的基础。与理想气体不同，真实气体考虑了气体分子的体积和影响其相互作用的分子间作用力。通过使用像范德瓦尔斯方程这样的状态方程，我们可以获得关于气体在各种科学和工程背景下行为的宝贵见解。认识到理想气体和真实气体之间的差异使我们能够做出更准确的预测，并开发出依赖于气体行为的更好技术，最终促进多个研究领域的进步。