law of partial pressure

简明释义

道尔顿法则

英英释义

例句

1.The law of partial pressure helps us understand how gases behave under different conditions.

分压定律帮助我们理解气体在不同条件下的行为。

2.According to the law of partial pressure, the total pressure of a gas mixture is equal to the sum of the partial pressures of each individual gas.

根据分压定律，气体混合物的总压力等于每种气体的分压之和。

3.When scuba diving, divers must consider the law of partial pressure to avoid nitrogen narcosis.

潜水时，潜水员必须考虑分压定律以避免氮醉。

4.The law of partial pressure can be observed when mixing gases like carbon dioxide and nitrogen in a sealed container.

在密闭容器中混合二氧化碳和氮气时，可以观察到分压定律。

5.In a laboratory, we can use the law of partial pressure to calculate the concentration of oxygen in a gas mixture.

在实验室中，我们可以使用分压定律来计算气体混合物中氧气的浓度。

作文

The concept of the law of partial pressure is fundamental in understanding how gases behave in mixtures. This principle, formulated by the renowned chemist John Dalton in the early 19th century, states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of each individual gas. In simpler terms, each gas in a mixture contributes to the overall pressure in proportion to its amount. This understanding is crucial in various scientific fields, including chemistry, physics, and environmental science.To illustrate the law of partial pressure, consider a container filled with three different gases: oxygen, nitrogen, and carbon dioxide. If the total pressure in the container is measured to be 1 atmosphere, we can determine the partial pressure of each gas based on its mole fraction in the mixture. For example, if there are 0.8 moles of nitrogen, 0.2 moles of oxygen, and 0.1 moles of carbon dioxide in the container, the total number of moles is 1.1. The partial pressure of nitrogen would then be calculated as follows: Partial Pressure of Nitrogen = (Mole Fraction of Nitrogen) × (Total Pressure) = (0.8/1.1) × 1 atm ≈ 0.727 atm.Similarly, the partial pressures of oxygen and carbon dioxide can be calculated, showcasing how each gas independently contributes to the total pressure without interfering with one another.Understanding the law of partial pressure is particularly important in fields such as respiratory physiology. The air we breathe is a mixture of gases, primarily nitrogen and oxygen. When these gases enter our lungs, they exert partial pressures that drive the diffusion process between the alveoli and the bloodstream. For instance, the higher partial pressure of oxygen in the alveoli compared to the blood allows oxygen to diffuse into the bloodstream, while the lower partial pressure of carbon dioxide in the alveoli facilitates its release from the blood.Moreover, the law of partial pressure has practical applications in industries such as scuba diving and anesthesia. Divers must understand how changes in pressure affect the solubility of gases in the body, particularly nitrogen, to avoid decompression sickness, commonly known as 'the bends.' Similarly, anesthesiologists utilize this principle to calculate the correct dosages of anesthetic gases to ensure patient safety during surgical procedures.In conclusion, the law of partial pressure is a vital principle that helps us comprehend the behavior of gases in mixtures. Its applications span across various scientific disciplines and real-world scenarios, emphasizing its significance in both theoretical and practical contexts. By grasping this concept, we can better appreciate the complex interactions that occur within gaseous systems, leading to advancements in science, medicine, and technology.

部分压力定律的概念对于理解气体在混合物中的行为至关重要。这个原则由著名化学家约翰·道尔顿在19世纪初提出，指出在一个非反应性气体的混合物中，施加的总压力等于每种单独气体的部分压力之和。简单来说，混合物中的每种气体根据其数量对总体压力做出贡献。这一理解在化学、物理和环境科学等多个科学领域中都是至关重要的。为了说明部分压力定律，考虑一个充满三种不同气体的容器：氧气、氮气和二氧化碳。如果测得容器中的总压力为1个大气压，我们可以根据混合物中每种气体的摩尔分数来确定其部分压力。例如，如果容器中有0.8摩尔的氮气、0.2摩尔的氧气和0.1摩尔的二氧化碳，则总摩尔数为1.1。氮气的部分压力可以按以下方式计算：氮气的部分压力 =（氮气的摩尔分数）×（总压力）=（0.8/1.1）×1 atm ≈ 0.727 atm。同样，氧气和二氧化碳的部分压力也可以计算出来，展示了每种气体如何独立地对总压力做出贡献而不相互干扰。理解部分压力定律在呼吸生理学等领域尤为重要。我们呼吸的空气是气体的混合物，主要是氮气和氧气。当这些气体进入我们的肺部时，它们施加的部分压力驱动着肺泡与血流之间的扩散过程。例如，肺泡中氧气的部分压力高于血液，使氧气能够扩散进入血液，而肺泡中二氧化碳的部分压力较低则促进其从血液释放。此外，部分压力定律在潜水和麻醉等行业中具有实际应用。潜水员必须理解压力变化如何影响气体在体内的溶解度，尤其是氮气，以避免减压病，通常称为“弯曲病”。同样，麻醉师利用这一原则计算麻醉气体的正确剂量，以确保手术过程中患者的安全。总之，部分压力定律是一个重要的原则，帮助我们理解气体在混合物中的行为。它的应用跨越多个科学学科和现实场景，强调了它在理论和实践环境中的重要性。通过掌握这一概念，我们可以更好地理解气体系统内发生的复杂相互作用，从而推动科学、医学和技术的发展。