Kinetic Theory of Gases
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Kinetic Theory of Gases

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What is a Gas?. But where do pressure and temperature come from?A gas is made up of molecules (or atoms) The pressure is a measure of the force the molecules exert when bouncing off a surfaceWe need to know something about the microscopic properties of a gas to understand its behavior. Mole.
Kinetic Theory of Gases

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1. Kinetic Theory of Gases Physics 202 Professor Lee Carkner Lecture 13

2. What is a Gas? But where do pressure and temperature come from? A gas is made up of molecules (or atoms) The pressure is a measure of the force the molecules exert when bouncing off a surface We need to know something about the microscopic properties of a gas to understand its behavior

3. Mole A gas is composed of molecules m = N = When thinking about molecules it sometimes is helpful to use the mole 1 mol = 6.02 X 1023 molecules 6.02 x 1023 is called Avogadro?s number (NA) M = M = mNA A mole of any gas occupies about the same volume

4. Ideal Gas Specifically, 1 mole of any gas held at constant temperature and constant volume will have almost the same pressure Gases that obey this relation are called ideal gases A fairly good approximation to real gases

5. Ideal Gas Law The temperature, pressure and volume of an ideal gas is given by: pV = nRT Where: R is the gas constant 8.31 J/mol K V in cubic meters

6. Work and the Ideal Gas Law p=nRT (1/V)

7. Isothermal Process If we hold the temperature constant in the work equation: W = nRT ln(Vf/Vi) Work for ideal gas in isothermal process

8. Isotherms From the ideal gas law we can get an expression for the temperature For an isothermal process temperature is constant so: If P goes up, V must go down Lines of constant temperature One distinct line for each temperature

9. Constant Volume or Pressure W=0 W = ?pdV = p(Vf-Vi) W = pDV For situations where T, V or P are not constant, we must solve the integral The above equations are not universal

10. Gas Speed The molecules bounce around inside a box and exert a pressure on the walls via collisions The pressure is a force and so is related to velocity by Newton?s second law F=d(mv)/dt The rate of momentum transfer depends on volume The final result is: p = (nMv2rms)/(3V) Where M is the molar mass (mass of 1 mole)

11. RMS Speed There is a range of velocities given by the Maxwellian velocity distribution We take as a typical value the root-mean-squared velocity (vrms) We can find an expression for vrms from the pressure and ideal gas equations vrms = (3RT/M)? For a given type of gas, velocity depends only on temperature

12. Maxwell?s Distribution

13. Translational Kinetic Energy Using the rms speed yields: Kave = ?mvrms2 Kave = (3/2)kT Where k = (R/NA) = 1.38 X 10-23 J/K and is called the Boltzmann constant Temperature is a measure of the average kinetic energy of a gas

14. Maxwellian Distribution and the Sun The vrms of protons is not large enough for them to combine in hydrogen fusion There are enough protons in the high-speed tail of the distribution for fusion to occur

15. Next Time Read: 19.8-19.11


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