Gases Over View. Schweitzer

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1 Gases Over View Schweitzer

2 Collision theory Describing Ideal gases Particles are very far apart relative to their size. Particles are traveling very fast Particles are traveling in straight lines Collisions are elastic There are no attractive or repulsive forces between particles.

3 Ideal gas vs. non-ideal gas Ideal gas: A gas where particles are small, traveling very fast, and therefore do not interact. All gas particles act the same. When performing mathematical calculations the type of gas particle is not a necessary piece of information. Non-ideal: particles are interacting therefore you will need to take into account the individual affects of each substance.

4 Collision theory Non-Ideal gases Take a gas, Cool the gas Compress it Re-peat the process The Collision theory will start to fail. In other words particles are interacting with each other.

5 Factors affecting Gases Pressure Volume Temperature # of particles (moles(n))

6 Pressure Mathmatically what is pressure? Pressure = Force per area

7 Atmospheric pressure atmospheric pressure is the weight of all the air above you.

8 Atomspheric pressure How do you know you are even under atmospheric pressure. Like gravity you are always under this force. How do you think a person might calculate atmospheric pressure much less know that it is even present?

9 Manometer/barometer An individual set up a device and noticed over the course of several days the height of mercury would change.

10 Atmospheric Pressure Sunny days the volume increased On Cloudy days the volume dropped Why?

11 Units of pressure Units of pressure mm of mercury (mmhg) represents how large of a column of mercury is needed to balance the pressure of the atmosphere. Also known as a torr Atmospheres (S.I. Unit) 1 atmosphere = 760 mmhg Pascal = Newton of force/square meter Bar Common unit of pressure used by meteorologist

12 Evangelista Torricelli (October 15, 1608 October 25, 1647) The torr (symbol: Torr) or millimetre of mercury (mmhg) is a non-si unit of pressure. It is the atmospheric pressure that supports a column of mercury 1 millimeter high. The unit is named after Evangelista Torricelli, Italian physicist and mathematician, for his discovery of the principle of the barometer in 1643.

13 Volume Unlike solids a gas will change shape to fill any size or shape container. The standard unit of volume for gases is the Liter.

14 Temperature Temperature: Measures the relative (average) motion of particles Average Kinetic energy

15 Absolute Scales vs. Relative scales Absolute Zero = zero No possible negative values Example: Golf Absolute: total number of swings Relative: Par, how many times have you swung the club relative to the course standard Relative Two points are set on a scale and we measure relative to these points. Negative values are possible and common.

16 Relative Temperature Scales Celsius Relative scale based on the boiling and freezing points of water. Fahrenheit Relative scale based on the body temperature and the freezing point of a salt solution similar to the human

17 Absolute Temperature Fahrenheit: Celsius: Kelvin: Kelvin: Increments of K and C are equal. Changing a substance 10C or 10K is the same change. Absolute Zero: All movement has been stopped. To my knowledge never been achieved.

18 # of Particles How do things change when more particles increase? Increase pressure? Increase Volume? Maybe maybe not.

19 Boyles Law P =? v =? n = moles T = Constant If you increase the atmospheric pressure on a container what will happen to the Volume?

20 Boyles law

21 Boyles Law P 1 V 1 = P 2 V 2 Increasing the pressure Reduces the volume Inverse proportion

22 Boyles Law -- Mathmatics P 1 V 1 = P 2 V 2 A balloon has a volume of 1 liter at 1 atm. What happens to the volume as the atmospheric pressure is dropped to.5 atm. P 1 = 1 atm V 1 = 1 L P 2 =.5 atm Q: What units can we use? A: Any absolute scaled unit? V 2 =? Substitute in and solve for V 2

23 Charles Law V 1 /T 1 = V 2 /T 2 V =? T =? P = constant n = constant What will happen to a sealed container when the temperature is increased?

24 Gay-Lussac s Law P 1 /T 1 = P 2 /T 2 T = P = n = constant V = constant As temperature increases the pressure increases as well. If you increase the pressure on an item what will happen to the temperature?

25 Combined gas law P 1 V 1 /T 1 = P 2 V 2 /T 2 Mathematically solve for the missing variable. If a variable doesn t change. You can drop it out to the experiment.

26 Try it!!! A Helium balloon has a volume of 10.0 L at STP. It floats up into the sky at a temperature of 10.0 C and.500 atm. What is the new volume?

27 Here is the answer P 1 V 1 /T 1 = P 2 V 2 /T 2 P 1 = 1 atm V 1 = 1 L T 1 = 273 P 2 =.5 V 2 =? T 2 = 283 P 1 V 1 T 2 /T 1 P 2 = V 2 Substitute and solve 1. *10. *273/283 *.500 = 20.7 L

28 Ideal Gas Law PV = nrt This equation must be used when you want to indicate the number of moles. The units are very specific because R has very specific units P = ATM V = L N = moles T = Kelvin

29 Give it a try!!! A balloon has a volume of 500 ml at a temperature of 100 C at 750mmHg. How many moles of gas are present? If the gas is all nitrogen the what is the mass of the balloon?

30 Here is the answer P = 750/760 =.987 atm V =.5L n =? R =.0821 T = 373 K PV/RT= n.0161 moles.0161 * (28g/mol) =.451g of gas

31 Non-Ideal gas law (real gases) Van der waals equation (P + n 2 a/v 2 )(V-nb) = nrt Very similar to PV = nrt

32 RMS Root Mean Square Average speed Temperature: Average kinetic energy KE = 1/2mv 2 Energy of a particle is composed of its velocity and its mass. Given the same amount of energy a more massive particle will move slower then a less massive particle.

33 Urms Calculation Urms = 3RT/M R = 8.31J/molK J = Kg m 2 /s 2 Since the joule is composed of kg the molar mass must also be a kg. Speed of an oxygen molecule at 25C. = 3*8.31*298/32E-3Kg(or.032kg) = 481m/s

34 Give it a try!! How fast does a methane (CH 4 ) molecule travel at room temperature (23C) U = 3 * 8.31* 296 /.016 = 679.1m/s

35 Diffusion Due to Brownian motion (random motion of particles) particles of high concentration move to areas of low concentration. Faster moving particles diffuse faster

36 effusion Effusion: rate at which randomly moving particles slip through holes. Example Helium balloon vs. air balloon

37 Graham's law of effusion Less mass particles effuse faster because they are moving faster (at a given temperature)

38 Give it a try A particle effuses twice as fast as Oxygen. What is the molar mass of this substance?

39 Here it is? 1 = unknown compound 2 = Oxygen compound 2/1 = ratio of effusion 2 = (M2/M1) (2)^2 = (32/M1) 4 = 32/X 8 g/mol

40 Stoichiometry and gases Remember ALL ideal gases act the same so the actual type of particle does not matter. 2H 2 (g) + O 2 (g) => 2H 2 O(g) If we have 4 liters of H 2 how many liters of O 2 are required and H 2 O are produced?

41 Stoichiometry and gases Remember ALL ideal gases act the same so the actual type of particle does not matter. 2H 2 (g) + O 2 (g) => 2H 2 O(g) 4 L 2 L 4L Gases are proportional to the coefficients.

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