Temperature and Gas

Looking for a Gas Gas is ein truthwhere. There is something called the atmosphere. Thats a big layer of botch that surrounds the Earth. Gases are random groups of atoms. Insolids,atomsand molecules are compact and close together. Liquids admit atoms that are spread out a little more. Gases are in reality spread out and the atoms and molecules are full of talent. They are bouncing almost uninterruptedly. Gases understructure fill a container of any sizing or stipulation. It doesnt however matter how big the container is. The molecules stillspread outto fill the unhurt space equally.That is wholeness of theirphysicalcharacteristics. Think about a globoon. No matter what shape you make the lumpoon, it pass on be evenly fill with the splatter molecules. The molecules are spread equally throughout the entire balloon. Liquids toilet solely fill the bottom of the container, while mishandlees can fill it entirely. The shape of liquids is really dependent on the result ofgrav ity, while gases are blowzy enough to have a little more freedom to go away. compression Gases Gases hold huge amounts ofenergy, and their molecules are spread out as lots as possible.With very little military press, when compared to liquids and solids, those molecules can be wedge. It happens all of the time. Combinations of pressing and decreasing temperature force gases into tubes that we use every day. You might see compressed air in a spray bottle or tonicity the carbon dioxide rush out of a can of soda. Those are some(prenominal) examples of gas forced into a smaller space than it would want, and the gas escapes the calculate 1 chance it gets. The gas molecules move from an area of high thrust to one of low contract level.What is the kinetic-molecular possibleness? The kinetic-molecular theory states 1) All matter is composed of very small particles called atoms,ions or molecules. 2) All of these small particles are in constant motion, even at the coldest temperat ure whether vibratory or translatory. 3)The kinetic energy of the particles is a measure of temprature. The greater the number of impacts the greater will be the force per unit area and vice-versa. 4) These particles collide but the impart energy remains same. PropertiesThe Link amidPandnThe pressure of a gas results from collisions between the gas particles and the walls of the container. single(a)ly time a gas particle hits the wall, it exerts a force on the wall. An increase in the number of gas particles in the container increases the frequency of collisions with the walls and thereof the pressure of the gas. Amontons rightfulness (PT)The last postulate of the kinetic molecular theory states that the intermediate kinetic energy of a gas particle depends only on the temperature of the gas.Thus, the average kinetic energy of the gas particles increases as the gas becomes warmer. Because the mass of these particles is constant, their kinetic energy can only increase if the average velocity of the particles increases. The faster these particles are moving when they hit the wall, the greater the force they exert on the wall. Since the force per collision becomes larger as the temperature increases, the pressure of the gas must increase as well. Boyles Law (P= 1/v)Gases can be compressed because most of the book of account of a gas is avoid space.If we compress a gas without changing its temperature, the average kinetic energy of the gas particles stays the same. There is no change in the revivify with which the particles move, but the container is smaller. Thus, the particles travel from one end of the container to the other in a shorter period of time. This means that they hit the walls more often. Any increase in the frequency of collisions with the walls must lead to an increase in the pressure of the gas. Thus, the pressure of a gas becomes larger as the volume of the gas becomes smaller.Charles Law (VT)The average kinetic energy of the particles in a gas is proportional to the temperature of the gas. Because the mass of these particles is constant, the particles must move faster as the gas becomes warmer. If they move faster, the particles will exert a greater force on the container distributively time they hit the walls, which leads to an increase in the pressure of the gas. If the walls of the container are flexible, it will expand until the pressure of the gas once more balances the pressure of the atmosphere.The volume of the gas therefore becomes larger as the temperature of the gas increases. Avogadros Hypothesis (VN)As the number of gas particles increases, the frequency of collisions with the walls of the container must increase. This, in turn, leads to an increase in the pressure of the gas. Flexible containers, such as a balloon, will expand until the pressure of the gas inside the balloon once again balances the pressure of the gas outside. Thus, the volume of the gas is proportional to the number of gas partic les. Daltons Law of partial tone Pressures (Pt=P1+P2+P3+ Imagine what would happen if six ball bearings of a different surface were added to themolecular dynamics simulator. The total pressure would increase because there would be more collisions with the walls of the container. But the pressure due to the collisions between the original ball bearings and the walls of the container would remain the same. There is so much empty space in the container that each type of ball bearing hits the walls of the container as often in the mixture as it did when there was only one kind of ball bearing on the glass plate.The total number of collisions with the wall in this mixture is therefore equal to the sum of the collisions that would occur when each size of ball bearing is present by itself. In other words, the total pressure of a mixture of gases is equal to the sum of the partial pressures of the individual gases. Grahams law of effusioncan be demonstrated with the apparatus in the figur e below. A thick-walled filter flaskful is evacuated with a vacuum pump. A syringe is filled with 25 mL of gas and the time involve for the gas to escape through the syringe needle into the evacuated filter flask is measured with a stop watch.