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**An Introduction to Gases**

Chapter 13

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**Kinetic Molecular Theory**

Postulate #1 Gases consist of tiny particles (atoms or molecules) Postulate #2 These particles are so small, compared with the distances between them, that the volume (size) of the individual particles can be assumed to be negligible (zero). Gases are COMPRESSIBLE

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**Kinetic Molecular Theory**

Postulate #3 The particles are in constant random motion, colliding with the walls of the container. These collisions with the walls cause the pressure exerted by the gas.

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**Kinetic Molecular Theory**

Postulate #4 The particles are assumed not to attract or to repel each other. Postulate #5 The average kinetic energy of the gas particles is directly proportional to the Kelvin temperature of the gas.

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**Avogadro’s Hypothesis**

At the same temp & pressure, equal volumes of gas hold same number of molecules. V and n are directly related. twice as many molecules Avogadro’s Law This is the law we will be using for the lab next week. Now this law wasn’t accepted at first because scientists didn’t understand the difference between an atom and a molecule. What is the difference between an atom and a molecule? Atoms make up molecules. Analogy: It is like a sports team. Each individual player makes completes their specific duties and part of the team but the molecule is the whole team.

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**Pressure Pressure of air is measured with a BAROMETER**

(developed by Torricelli in 1643)

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Pressure What is Pressure? What tool do we use to measure it?

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**Pressure mmHg (or Torr) Atmospheres (atm) Pascals (used in physics:**

1 pascal = 1 newton per square meter) 4. psi Equivalences: 1 atm = 760 mmHg 1 atm = 101,325 Pa = kPa 1 atm = 14.7 psi

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**Pressure Calculation What is 475 mm Hg expressed in atm? 475 mm Hg**

= 0.625 atm 760 mm Hg

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Pressure Calculation The pressure of a tire is measured as 294,000 pascals. What is this pressure in atm? 294, 000 Pa 1 atm 2.90 atm = 101, 325 Pa

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**“The Law of Partial Pressure”**

Dalton’s Law “The Law of Partial Pressure” The total pressure of a mixture of gases is the sum of the partial pressures of the gases in the mixture. Ptotal = PA + PB + PC

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Gas Laws Calculations Get out a calculator!!!

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**PV=nRT P = pressure ( atm or kPa ) V= volume ( L )**

The Gas Law PV=nRT P = pressure ( atm or kPa ) V= volume ( L ) n= number of moles (mol) T= temperature (K)

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**R – The Proportionality Constant**

Value depends on units 8.314 L (kPa) mol (K) 0.0821 L (atm) Or R is the proportionality constant Basically once scientists got the gas laws figured out, they put them all together but realized that the variables behaved according to this proportionality constant. Your value of R, like anything else, will vary depending on the units. Can’t add apples to oranges – If you have 3 apples and 5 oranges how many apples do you have? Because you can’t add apples to oranges. So to add them together you would need to convert to fruit for both and then add them together.

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**The Gas Law – Problem PV = nRT P = 1454.95 kPa P = 1500 kPa**

If 7.0 moles of an ideal gas has a volume of 12.0 L with a temperature of 300. K, what is the pressure in kPa? PV = nRT P (12.0 L) = (7.0 mol)(300 K) 8.314 L (kPa) mol (K) Using the Ideal Gas Law work through this problem with your neighbor. What did everyone get? 1500 kPa, correct Let’s see how you got that: P = kPa P = 1500 kPa

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Combined Gas Law Let’s say we have some O2 gas AND we change some conditions. Would there be anything similar between the two gases?

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**Combined Gas Law – Problem**

You have 3 moles of a solution at 300. K and 15 atm in a 2 L container. If the container is heated to 350. K and the volume decreased to 1 L, what will the new pressure be? P1 15 atm P2 want V1 2 L V2 1 L n1 3 moles n2 R1 constant R2 T1 300. K T2 350. K Work through this problem with your neighbor. What did everyone get? 35 atm, correct Let’s see how you got that: All work is on the powerpoint (click mouse)

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**Combined Gas Law – Problemc**

P1V1 = n1R1T1 P2V2 n2R2T2 If we know that R1 = R2 and the mass is constant then P1V1 = T1 P2V2 T2 Replace with numbers (15 atm)(2 L) = (300. K) P2(1L) (350. K)

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**Combined Gas Law – Problem**

(15 atm)(2 L) = (300. K) P2(1L) (350. K) (15 atm)(2 L)(350. K) = P2 (1L)(300. K) P2 = 35 atm

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**P1V1 = P2V2 Pressure & Volume At constant Temperature**

Pressure and Volume vary inversely. Why? More collisions More pressure P1V1 = P2V2 Smaller volume means particles have shorter distance to go to hit the sides of the container.

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**P & V – Example Problem 1.0 atm = P2**

If you start with L of a gas at 7.0 atm and you move the gas to a container with 3.5 L available, how much pressure will the gas exert? P1 (V1) = P2 (V2) 7.0 atm (0.500 L) = P2 (3.5 L) Work through this problem with your neighbor. What did everyone get? 1.0 atm, correct Let’s see how you got that: All work is on the powerpoint (click mouse) 7 atm (0.500 L) = P2 3.5 L 1.0 atm = P2

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Demo Put a few drops of water in a can. Heat the can until the water boils. What is happening to the gas inside? Now flip the can over into cold water. Predict what do you predict will happen?

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On a Larger Scale The most common (and commonly collapsed) railcar is the DOT 111A100 class or commonly called a "general purpose" tank car. These cars are rated to a test pressure of 100 psig and a minimum burst pressure of 500 psig. Minimum carbon steel plate thickness is 7/16 inch. For a 23,000 gallon car, the tank length is about 55 feet. For comparison purposes the "heaviest" pressure car commonly used is a 105J500, rated to a test pressure of 500 psig and a minimum burst of 1250 psig. They are made of 1 inch thick, high-strength steel plate.

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On a Larger Scale

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**V1 = V2 T1 T2 Temperature & Volume At constant Pressure**

Volume & Temperature vary directly. Why? More collisions More Volume Heating a gas will make it expand. ROOT BEER DEMO Also relate back to gases expanding to take up all space available. V1 = V2 T1 T2

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T & V – Example Problem If a gas is in a balloon with a volume of 12.0 L and at a temperature of 300. K, what will the volume be if you place the balloon in a freezer at 250. K? V1 = V2 T1 T2 12.0 L 300. K 250. K 12.0 L (250. K) 10.0 L Work through this problem with your neighbor. What did everyone get? 10.0 L, correct Let’s see how you got that: All work is on the powerpoint (click mouse)

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S.T.P. Standard Temperature and Pressure These are conditions that are universal Standard Temperature: 0ºC or 273K Standard Pressure: 1atm or kPa

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**S.T.P. – Example Problem PV = nRT V= 22.4 L**

What is the volume of 1 mole of a gas at STP? P 1 atm V want n 1 mole R (L)(atm)/(K)(mole) T 273 K PV = nRT (1atm)V = (1 mole)( [Latm/Kmole])(273K) V= 22.4 L

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Gases Ch.10 and 11. Kinetic-Molecular Theory 1.Gases consist of very small particles that are far apart Most particles are molecules Volume of particles.

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