state the assumptions that makes up the kinetic theory and evidence to prove sny two of these assumptions
The four assumptions are
1. The number of molecules is large, but their separation is large compared to their molecular size.
2.Molecules obey Newton's laws of motion.
3.Molecules move randomly with a distribution is speed which is constant.
4.Molecules undergoe elastic collisions with other molecules and the walls, but otherwise exert no forces on each other.
Molecules move randomly with a distribution is speed which is constant.
I would reword this. Molecules move randomly, undergoing many collisions, so that molecular speed is a distribution about some mean, that mean velocity determines what we macroscopically call "temperature"
The kinetic theory of gases is a scientific model that explains the behavior of gases based on certain assumptions. The assumptions that make up the kinetic theory include:
1. Gases are composed of individual particles: This assumption states that gases consist of small particles, such as atoms or molecules, that are in constant random motion. Evidence for this assumption comes from various experiments, such as Brownian motion. In 1827, Robert Brown observed pollen particles suspended in water, which were randomly jiggling due to collisions with water molecules. This observation provided evidence that gases are made up of small particles.
2. Gas particles are in constant motion: The kinetic theory assumes that gas particles are in continuous motion and move in random directions at various speeds. This assumption is supported by the observation of diffusion. Diffusion refers to the gradual mixing of one gas with another when they are brought into contact. For example, when a perfume is sprayed in one corner of a room, the smell spreads throughout the room due to the random motion of gas particles.
3. Gas particles have negligible volume: According to the kinetic theory, gas particles are assumed to occupy a negligible volume compared to the total volume of the gas. This assumption is supported by the compressibility of gases. When a gas is compressed (e.g., by reducing its volume), the gas particles are forced closer together. This suggests that the individual particles occupy very little space compared to the empty space between them.
4. There are no intermolecular forces between gas particles: The kinetic theory assumes that gas particles do not exert attractive or repulsive forces on each other. Evidence for this assumption can be seen in the behavior of an ideal gas. An ideal gas follows the gas laws, such as Boyle's Law and Charles' Law, which describe the relationships between pressure, volume, and temperature. These laws are based on the assumption that there are no intermolecular forces between gas particles.
It is worth mentioning that while the assumptions of the kinetic theory are generally applicable to most gases, they have limitations at extreme conditions (e.g., high pressures or low temperatures) where intermolecular forces become significant.