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The kinetic theory of gases is a simple classical model of the thermodynamic behavior of gases. It treats a gas as composed of numerous particles, too small to see with a microscope, which are constantly in random motion.
The simplest kinetic model is based on the assumptions that: (1) the gas is composed of a large number of identical molecules moving in random directions, separated by distances that are large compared with their size; (2) the molecules undergo perfectly elastic collisions (no energy loss) with each other and with the walls of the container, but...
- The Editors of Encyclopaedia Britannica
分子運動論 （英語： kinetic theory of gases ，又稱 氣體動力論 ）是描述氣體為大量做永不停息的 隨機運動 的粒子（ 原子 或 分子 ，物理學上一般不加區分，都稱作分子）。 快速運動的分子不斷碰撞其他分子或容器的壁。 分子運動理論就是通過分子的成分和運動來解釋氣體的宏觀性質，如 壓力 、 溫度 、 體積 等。 分子運動理論認為，壓力不是如 牛頓 猜想的那樣，來自分子之間的靜態排斥，而是來自以不同速度做 熱運動 的分子之間的碰撞。 分子的體積很小，不能直接觀察。 顯微鏡下花粉迸裂出之微粒做的無規則運動—— 布朗運動 ，是分子碰撞的直接結果，可以作為分子存在的間接證據。 理論假設 [ 編輯] 理想氣體動理論建立在如下假設之上：
Kinetic theory is the atomic description of gases as well as liquids and solids. It models the properties of matter in terms of continuous random motion of molecules. The ideal gas law can be expressed in terms of the mass of the gas’s molecules and \(\bar{v^2}\), the average of the molecular speed squared, instead of the temperature.
Kinetic theory is based on an atomic model of matter. The basic assumption of kinetic theory is that the measurable properties of gases, liquids, and solids reflect the combined actions of countless numbers of atoms and molecules.
According to the kinetic molecular theory, the average kinetic energy of an ideal gas is directly proportional to the absolute temperature. Kinetic energy is the energy a body has by virtue of its motion: \[ KE = \dfrac{1}{2}m v^2\] with \(KE\) is the kinetic energy of a
The Model Kinetic Interpretation of Temperature Derivation of the Ideal Gas Law Contributors and Attributions The kinetic theory describes a gas as a large number of submicroscopic particles (atoms or molecules), all of which are in constant, random motion.
