Does adding more particles increase temperature and does temperature change the speed of particles?
Suppose that you were talking about polyethylene particles 0.1 mm in size dispersed (using a surfactant) in water at 20*C and 1 bar pressure. If you poured in a bit more surfactant at 20*C and then added particles from a bottle where they had been kept for an hour at a 40*C, those hot particles would raise the temperature of the dispersion. If you repeated the experiment using particles from a bottle kept at 0*C, the temperature of the dispersion would decrease. Since the Brownian motion (random jiggling) of the particles depends on the temperature, a hotter dispersion means the particles move about more rapidly. Thus, adding particles changes the temperature of a dispersion (and the average speed of its particles) only if the added particles are hotter than the original dispersion.
Temperature is a measure of the average value of the kinetic energy of the particles in an object. As the temperature of something increases, the average speed of its particles increases. The temperature of hot tea is higher than the temperature of iced tea because the particles in the hot tea are moving faster. If the temperature is increased the particles gain more kinetic energy or vibrate faster. This means that they move faster and take more space. If the temperature is decreased, it is the opposite. Particles move slower, because of less energy. Temperature directly affects the movement of particles such as molecules. Molecules move faster when temperature increases and move slower when temperature decreases. The increased molecular movement causes solids, liquids, and gases to expand when heated. The temperature of a gas is a measure of the average translational kinetic energy of the molecules. In a hot gas, the molecules move faster than in a cold gas; the mass remains the same, but the kinetic energy, and hence the temperature, is greater because of the increased velocity of the molecules. As the temperature of a solid, liquid or gas increases, the particles move more rapidly. As the temperature falls, the particles slow down. No matter what they're in, solid, liquid, or gas, molecules are always moving, even if just a little bit. The speed of the molecules depends on their temperature. Cold things have slow-moving molecules, while hot things have fast-moving molecules. In fact, temperature is really a measurement of molecule speed. Particles within matter are in constant motion. The amount of motion of these particles depends on the kinetic energy they possess. Particles with more kinetic energy move faster and farther apart. Particles with less energy move more slowly and stay closer together. When we add energy to an object, its atoms and molecules move faster increasing its energy of motion or heat. Even objects which are very cold have some heat energy because their atoms are still moving. Fundamentally, atoms and molecules move faster as a result of heat transfer because microscopic kinetic energy has been transferred to them from other atoms or molecules of an object having greater kinetic energy (higher temperature). If we heat the gas to a higher temperature, the particles in the container will move faster. This is because heating increases the kinetic energy of the particles. If the particles are moving more quickly, there will be more collisions between particles. If you add gas particles to an insulated container of fixed volume, what happens to the temperature depends entirely on what energy you give those particles when you add them. If you give them the same average kinetic energy as the ideal gas particles already in the container, the temperature will not change. Gay Lussac's Law - states that the pressure of a given amount of gas held at constant volume is directly proportional to the Kelvin temperature. If you heat a gas you give the molecules more energy so they move faster. This means more impacts on the walls of the container and an increase in the pressure. As we know, gas pressure results from the number of collisions that occur between gas particles and the walls of their container. If we add more gas particles to the container, the number of collisions, and thus the pressure, will increase.
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