de Brogile was blind and half deaf, it was until the late 1800's that he found a female companion. in 1902 his first child de Brogile the 2nd (JR) was born. twelve years later de Brogile was sent to an insane asylum for going crazy and murdering his wife and son. He later died of herpes thirteen years later. he was completely irrelevant to the assumption about the motion of tiny particles.
The basic assumption of the kinetic theory of matter is that all matter is made up of particles (atoms or molecules) that are in constant motion. This motion increases with temperature and decreases with lowered temperature.
One assumption of the kinetic theory of gases is that gas particles occupy a negligible volume compared to the volume of the container. Therefore, the idea that gas particles have significant volume or that they interact through forces that significantly affect their motion would not align with the assumptions of the kinetic theory. Additionally, the assumption that gas particles are in constant random motion contradicts any notion of them being at rest or having fixed positions.
One assumption of the kinetic theory of gases is that gas particles are in constant, random motion and do not attract or repel each other. Therefore, a false assumption would be that gas particles experience significant intermolecular forces, as this contradicts the idea that they behave independently. Additionally, the kinetic theory assumes that the volume of the individual gas particles is negligible compared to the total volume of the gas, so assuming that particles occupy significant space would also be incorrect.
The assumption of kinetic theory that explains the pressure a gas exerts is that gas particles are in constant, random motion. This motion results in collisions between gas particles and the walls of the container, creating a force per unit area known as pressure.
At low temperatures, the assumption that gas particles are in constant, random motion fails. This is because at very low temperatures, the kinetic energy of the particles decreases, causing them to move more slowly and exhibit less thermal energy. Consequently, the assumption that gas particles have negligible volume compared to the volume of the container becomes less valid at low temperatures as the particles are closer together.
The basic assumption of the kinetic theory of matter is that all matter is made up of particles (atoms or molecules) that are in constant motion. This motion increases with temperature and decreases with lowered temperature.
One assumption of the kinetic theory of gases is that gas particles occupy a negligible volume compared to the volume of the container. Therefore, the idea that gas particles have significant volume or that they interact through forces that significantly affect their motion would not align with the assumptions of the kinetic theory. Additionally, the assumption that gas particles are in constant random motion contradicts any notion of them being at rest or having fixed positions.
One assumption of the kinetic theory of gases is that gas particles are in constant, random motion and do not attract or repel each other. Therefore, a false assumption would be that gas particles experience significant intermolecular forces, as this contradicts the idea that they behave independently. Additionally, the kinetic theory assumes that the volume of the individual gas particles is negligible compared to the total volume of the gas, so assuming that particles occupy significant space would also be incorrect.
Kinetic molecular theory assumes that gases consist of particles (atoms or molecules) in constant random motion. It also assumes that gas particles are small compared to the distance between them. Additionally, the theory assumes that gas particles are in continuous, rapid, and random motion.
The assumption of kinetic theory that explains the pressure a gas exerts is that gas particles are in constant, random motion. This motion results in collisions between gas particles and the walls of the container, creating a force per unit area known as pressure.
At low temperatures, the assumption that gas particles are in constant, random motion fails. This is because at very low temperatures, the kinetic energy of the particles decreases, causing them to move more slowly and exhibit less thermal energy. Consequently, the assumption that gas particles have negligible volume compared to the volume of the container becomes less valid at low temperatures as the particles are closer together.
According to the kinetic theory of gases, one assumption is that the forces of attraction between particles can be ignored, particularly under ordinary conditions. However, a key point that is not an assumption of the kinetic theory is that gas particles occupy a significant volume compared to the total volume of the gas, which is incorrect; the theory assumes that gas particles themselves have negligible volume. Additionally, the theory assumes that gas particles are in constant, random motion and collide elastically with one another and the walls of their container.
The particles are tightly packed so they vibrate.
One assumption that is not part of the kinetic theory of gases is that gas particles have significant intermolecular forces acting between them. In the kinetic theory, it is assumed that gas particles are in constant random motion, and the interactions between them are negligible except during elastic collisions. Additionally, the theory assumes that gas particles occupy a volume much smaller than the volume of the container, meaning the size of the particles themselves is considered negligible.
Yes, the assumption that energy is transferred when individual particles collide is a key principle of the kinetic-molecular theory. This theory explains the behavior of gases by considering them as a collection of particles in constant motion, colliding with each other and with the walls of their container. The transfer of kinetic energy during these collisions is central to understanding properties such as pressure and temperature.
Brownian motion
Brownian motion is the random moving and mixing of particles.