File Name: gas laws and kinetic theory of gases ppt to .zip
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Published in: Business , Technology. Full Name Comment goes here. Are you sure you want to Yes No. Monika Jain , teacher. Mandeep Singh. Show More. No Downloads. Views Total views. Actions Shares. No notes for slide. Physics Chapter Kinetic Theory of Gases 1. Sketch and interpret b. Physics DF Chapter P The pressure of a fixed mass of gass at constant temperature is inversely T2 propertional to its volume.
P Physics DF Chapter 14 The Since the vessels A and B arevessels are filled with an ideal gas connected by a narrow tube thus the pressure for both vessels is same,and are at a steady state. The finally i. Initially A contains 3. Calculate the pressure after the connecting tap has been opened and the system reached equilibrium, assuming that A is kept at K and B is kept at K.
Physics DF Chapter 14 Exercise A gas has a volume of What would its volume be at STP? Estimate the number of molecules in a flask of volume 5. A cylinder contains a hydrogen gas of volume 2. Calculate a. Explain and use roota. State the assumptions mean square rms of kinetic theory of speed, gases. Apply the equations of 2 kT ideal gas, v 3 m 1 of gas molecules. Gravity has no effect on molecular motion. Figure Wa Wall B ll A The time For N molecules of the ideal gas,taken for this movement is m 2 m 2 m 2 2d Fx vx1 vx Physics DF Chapter 14 where vx1 is the x Thus, the x component for the component of velocity of total force exerted on the wall of molecule 1, vx2 is the x the cubical container is component of velocity of molecule 2 and so on.
The mean speed of the Eight gas molecules chosen molecules is given by at random are found to have speeds of 1,1,2,2,2,3,4 and N 8 5 m s 1.
Determine N a. The mean square speed of c. By using the equation of b. PV RT M The root mean square speed of the oxygen molecules is 3RT 3 8. In a period of 1. If the molecules move with a speed of m s 1 and strike the wall head-on in the elastic collisions, determine the pressure exerted on the wall. The mass of one N2 molecule is 4. Initially, the r. The pressure and volume of the gas are each doubled while the number of moles of the gas is kept constant. Calculate the final translational r.
Given that the r. The molar mass of O2 is Explain and use c. Define degree of freedom translational kinetic energy of gases, d. State the principle of equipartition of energy.
Explain internal energy f. Explain and use of gas and relate the internal energy of an internal energy to the ideal gas number of degree of freedom, The average translational C. Determine kinetic energy of a moleculea. Physics DF Chapter 14Diatomic gas e. The total translational translational kinetic energy, thuskinetic energy of the gas 3molecules is 3. Physics DF Chapter 14 Table Table One mole of oxygen has a mass of 32 g.
Assuming oxygen behaves as an ideal gas, calculate a. You just clipped your first slide! Clipping is a handy way to collect important slides you want to go back to later. Now customize the name of a clipboard to store your clips. Visibility Others can see my Clipboard. Cancel Save.
Understanding Kinetic Molecular Theory can help us identify when a gas will behave like an ideal gas, and when it will deviate and not behave like an ideal gas. There are five postulates to the Kinetic Molecular Theory, and gases will deviate from the ideal gas law when these postulates break down. The fifth postulate is very important to note as it relates kinetic energy to temperature. For a gaseous particle most of the kinetic energy is in translation. But a gas is not a particle, but an ensemble of particles, all moving with different velocities in different directions.
Charles's law also known as the law of volumes is an experimental gas law that describes how gases tend to expand when heated. A modern statement of Charles's law is:. When the pressure on a sample of a dry gas is held constant, the Kelvin temperature and the volume will be in direct proportion. This relationship of direct proportion can be written as:. V is the volume of the gas,.
By the late 19th century, scientists had begun accepting the atomic theory of matter started relating it to individual molecules. The Kinetic Molecular Theory of Gases comes from observations that scientists made about gases to explain their macroscopic properties. The following are the basic assumptions of the Kinetic Molecular Theory:. This can be written as:. According to Kinetic Molecular Theory, an increase in temperature will increase the average kinetic energy of the molecules.
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