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Understanding Gases: Kinetic Molecular Theory and Properties

This chapter delves into the unique properties of gases as a state of matter according to the Kinetic Molecular Theory. It explains how gas molecules are separate and move rapidly in straight lines, leading to pressure as they collide with container walls. We discuss the importance of temperature and volume, influencing the behavior of gases, and introduce key concepts such as Boyle's Law. Understanding these principles is crucial for grasping the dynamics of gases in various conditions and applications.

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Understanding Gases: Kinetic Molecular Theory and Properties

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  1. Chapter 9: Gases

  2. States of Matter

  3. Kinetic Molecular Theory (Review) solid liquid gas (vibrational) (vibrational, (translational) rotational, translational)

  4. What is unique about “gas” state? • There is space between molecules so size of molecules DOES NOT affect the VOLUME a gas occupies. • The volume is affected when the space between the molecule changes by • Temperature - Unit = oC, Kelvin (K) • Pressure – force/unit area - Unit = N/m2 = Pa kPa * old units: psi, mm Hg, torr, atm *Standard temp and Pressure (STP) = 0oC & 101.325 kPa

  5. Kinetic Molecular TheoryAssumptions for Gases • Each gas molecule is separate, surrounded by empty space • Particles move rapidly in straight lines, often colliding with each other and the container walls. • There is no loss of energy when 2 particles collide • In the gas phase, there are no attractive forces between particles • At any given temperature, the average kinetic energy of the particles in gases is the same. http://www.chm.davidson.edu/vce/kineticmoleculartheory/basicconcepts.html

  6. In a container filled with gas there will be collisions between the particles and particles and also collisions between particles and the container walls. • The collisions between the particles and the walls is known as GAS PRESSURE. • The greater the amount of collisions with the wall in a given amount of time, will give a greater pressure.

  7. As the volume decreases, the particles collide more frequently with the containers walls. Therefore, the particles will exert greater force on the walls. • Therefore, PRESSURE INCREASES. * Pressure = force/area = force per surface area

  8. Boyle’s Law Simulation & Graph http://www.chem.iastate.edu/group/Greenbowe/sections/projectfolder/flashfiles/gaslaw/boyles_law_graph.html

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