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**Kinetic Theory of Gases I**

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**Ideal Gas The number of molecules is large**

The average separation between molecules is large Molecules moves randomly Molecules obeys Newton’s Law Molecules collide elastically with each other and with the wall Consists of identical molecules

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**in K The Ideal Gas Law n: the number of moles in the ideal gas**

total number of molecules Avogadro’s number: the number of atoms, molecules, etc, in a mole of a substance: NA=6.02 x 1023/mol. R: the Gas Constant: R = 8.31 J/mol · K

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**Pressure and Temperature**

Pressure: Results from collisions of molecules on the surface Force Pressure: Area Force: Rate of momentum given to the surface Momentum: momentum given by each collision times the number of collisions in time dt

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**Only molecules moving toward the surface hit **

the surface. Assuming the surface is normal to the x axis, half the molecules of speed vx move toward the surface. Only those close enough to the surface hit it in time dt, those within the distance vxdt The number of collisions hitting an area A in time dt is Average density The momentum given by each collision to the surface

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Momentum in time dt: Force: Pressure: Not all molecules have the same

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**is the root-mean-square speed**

Pressure: Average Translational Kinetic Energy:

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Pressure: From and Temperature: Boltzmann constant:

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From and Avogadro’s number Molar mass

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**Pressure Density x Kinetic Energy**

Temperature Kinetic Energy

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**Internal Energy For monatomic gas: the internal energy = sum**

of the kinetic energy of all molecules:

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**HRW 16P (5th ed. ). Consider a given mass of an ideal gas**

HRW 16P (5th ed.). Consider a given mass of an ideal gas. Compare curves representing constant-pressure, constant volume, and isothermal processes on (a) a p-V diagram, (b) a p-T diagram, and (c) a V-T diagram. (d) How do these curves depend on the mass of gas? p V constant pressure isothermal constant volume T (d) Constant temperature Constant volume Constant pressure

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**(d) Cyclic process ∆Eint = 0**

HRW 18P (5th ed.). A sample of an ideal gas is taken through the cyclic process abca shown in the figure; at point a, T = 200 K. (a) How many moles of gas are in the sample? What are (b) the temperature of the gas at point b, (c) the temperature of the gas at point c, and (d) the net heat added to the gas during the cycle? (a) a b c 1.0 3.0 Pressure (kN/m2) 2.5 7.5 (b) (c) (d) Cyclic process ∆Eint = 0 Volume (m3) Q = W = Enclosed Area= 0.5 x 2m2 x 5x103Pa = 5.0 x 103 J

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**(a) (b) Since for 0.5 vrms for 2 vrms**

HRW 30E (5th ed.).(a) Compute the root-mean-square speed of a nitrogen molecule at 20.0 ˚C. At what temperatures will the root-mean-square speed be (b) half that value and (c) twice that value? (a) (b) Since for 0.5 vrms for 2 vrms

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HRW 34E (5th ed.). What is the average translational kinetic energy of nitrogen molecules at 1600K, (a) in joules and (b) in electron-volts? (a) (b) 1 eV = 1.60 x J

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**Kinetic Theory of Gases II**

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**the bigger the molecules**

Mean Free Path Molecules collide elastically with other molecules Mean Free Path l: average distance between two consecutive collisions the bigger the molecules the more collisions the more molecules the more collisions

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**Molar Specific Heat Definition: For constant volume:**

For constant pressure: The 1st Law of Thermodynamics: (Monatomic)

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Constant Volume (Monatomic)

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Constant Pressure (Monatomic)

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1st Law Adiabatic Process Ideal Gas Law (Q=0) Divide by pV:

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Ideal Gas Law

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**Equipartition of Energy**

The internal energy of non-monatomic molecules includes also vibrational and rotational energies besides the translational energy. Each degree of freedom has associated with it an energy of per molecules.

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Monatomic Gases 3 translational degrees of freedom:

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**Diatomic Gases 3 translational degrees of freedom**

2 rotational degrees of freedom 2 vibrational degrees of freedom HOWEVER, different DOFs require different temperatures to excite. At room temperature, only the first two kinds are excited:

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HRW 63P (5th ed.). Let 20.9 J of heat be added to a particular ideal gas. As a result, its volume changes from 50.0 cm3 to 100 cm3 while the pressure remains constant at 1.00 atm. (a) By how much did the internal energy of the gas change? If the quantity of gas present is 2.00x10-3 mol, find the molar specific heat at (b) constant pressure and (c) constant volume. (a) Constant pressure: W = p∆V

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HRW 63P (5th ed.). Let 20.9 J of heat be added to a particular ideal gas. As a result, its volume changes from 50.0 cm3 to 100 cm3 while the pressure remains constant at 1.00 atm. (a) By how much did the internal energy of the gas change? If the quantity of gas present is 2.00x10-3 mol, find the molar specific heat at (b) constant pressure and (c) constant volume. (b) (c)

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**(a) Adiabatic Monatomic**

HRW 81P (5th ed.). An ideal gas experiences an adiabatic compression from p =1.0 atm, V =1.0x106 L, T = 0.0 ˚C to p =1.0 x 105 atm, V =1.0x103 L. (a) Is the gas monatomic, diatomic, or polyatomic? (b) What is its final temperature? (c) How many moles of gas are present? (d) What is the total translational kinetic energy per mole before and after the compression? (e) What is the ratio of the squares of the rms speeds before and after the compression? (a) Adiabatic Monatomic

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HRW 81P (5th ed.). An ideal gas experiences an adiabatic compression from p =1.0 atm, V =1.0x106 L, T = 0.0 ˚C to p =1.0 x 105 atm, V =1.0x103 L. (a) Is the gas monatomic, diatomic, or polyatomic? (b) What is its final temperature? (c) How many moles of gas are present? (d) What is the total translational kinetic energy per mole before and after the compression? (e) What is the ratio of the squares of the rms speeds before and after the compression? (b)

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HRW 81P (5th ed.). An ideal gas experiences an adiabatic compression from p =1.0 atm, V =1.0x106 L, T = 0.0 ˚C to p =1.0 x 105 atm, V =1.0x103 L. (a) Is the gas monatomic, diatomic, or polyatomic? (b) What is its final temperature? (c) How many moles of gas are present? (d) What is the total translational kinetic energy per mole before and after the compression? (e) What is the ratio of the squares of the rms speeds before and after the compression? (c) (Pay attention to the units) (d) For N/n = 1

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HRW 81P (5th ed.). An ideal gas experiences an adiabatic compression from p =1.0 atm, V =1.0x106 L, T = 0.0 ˚C to p =1.0 x 105 atm, V =1.0x103 L. (a) Is the gas monatomic, diatomic, or polyatomic? (b) What is its final temperature? (c) How many moles of gas are present? (d) What is the total translational kinetic energy per mole before and after the compression? (e) What is the ratio of the squares of the rms speeds before and after the compression? (e)

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Chapter 19 The Kinetic Theory of Gases To study p, V, E int, T, …etc. from a “molecular” approach 19.1 A new way to look at gases: Warm up: How many moles.

Chapter 19 The Kinetic Theory of Gases To study p, V, E int, T, …etc. from a “molecular” approach 19.1 A new way to look at gases: Warm up: How many moles.

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