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Got Gas?
What gases are important for each of the following:  O 2 , CO 2  and/or He? A.  B.  C.  D.
What gases are important for each of the following:  O 2 , CO 2  and/or He?   A.  CO 2   B. O 2 /CO 2   C. O 2   D.  He
Gases  are made up of molecules. Air consists of a mixture of gases, including nitrogen N 2 , Oxygen O 2 , and carbon dioxide CO 2 . Gases exert pressure on any surface with which they come in to contact. The gases in our atmosphere are subject to the Earth’s gravitational pull therefore the atmosphere is much denser nearer the Earths surface and less dense as we travel away from the planet.
Some Gases in Our Lives oxygen O 2 nitrogen N 2 ozone O 3 argon Ar   carbon dioxide  CO 2  water H 2 O Noble gases :  helium He  neon Ne  krypton Kr  xenon Xe Other gases:   fluorine  F 2   chlorine  Cl 2   ammonia NH 3  methane CH 4 carbon monoxide CO nitrogen dioxide NO 2 sulfur dioxide SO 2
Pressure  is one of the most easily measured properties of a gas. We define pressure as the force per unit area.  P= Force/Area.
Pascal:   The SI unit of pressure.  1 Pascal = 1   N /m 2    = 1 kg  x  m/s 2  x   1/m 2 Named after Blaise Pascal
Ice skates are familiar examples of the effects of pressure. The area of the blades of a skate are much smaller than, say, the soles of your feet. So if you strap on ice skates, your weight will act on an area much smaller than it would if you were wearing normal shoes. Since  A  decreases while  F  stays the same, the pressure you exert on the ice will be much greater if you're wearing skates. This pressure is often enough to melt a layer of ice, which allows your skate to glide smoothly across an ice rink. If you try the same maneuver with normal shoes, you will not generate enough pressure to melt the ice and won't get anywhere fast.
Air pressure  is the force exerted on you by the weight of tiny particles of air (air molecules). Although air molecules are invisible, they still have weight and take up space. We are usually unaware of the air pressure around us, probably because we are used to it. Since there's a lot of "empty" space between air molecules, air can be compressed to fit in a smaller  volume.
How much pressure are you under?  Earth's atmosphere is pressing against each square inch of you with a force of 1 kilogram per square centimeter (14.7 pounds per square inch). The force on 1,000 square centimeters (a little larger than a square foot) is about a ton!
Why doesn't all that pressure squash me?  Remember that you have air  inside  your body too, that air balances out the pressure outside so you stay nice and firm and not squishy.  Well…some of us are more squishy than others
Run for Cover!  Air pressure can tell us about what kind of weather to expect as well. When it's compressed, air is said to be "under high pressure". If a  high pressure  system is on its way, often you can expect cooler temperatures and clear skies. If a  low pressure system  is coming, then look for warmer weather, storms and rain.
Some important pressure terms ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Look a barometer!!
Barometer? Weather forecasters measure air pressure with a  barometer  . Barometers are used to measure the current air pressure at a particular location in "inches of mercury" or in "millibars" (mb). A measurement of 29.92 inches of mercury is equivalent  to 1013.25 millibars. Crazy huh? Bar -  A unit of measurement equivalent to 1×10 5  Pascals.
More pressure terminology ,[object Object],[object Object],[object Object]
Why do my ears pop as I increase altitude?   As the number of molecules of air around you decreases, the air pressure decreases. This causes your ears to pop in order to balance the pressure between the outside and inside of your ear. Since you are breathing fewer molecules of oxygen, you need to breathe faster to bring the few molecules there are into your lungs to make up for the deficit.  Air pressure on Mt. Everest is 670 mb less than on the Cayman Islands.
1. If you were on a mountain, would the weight of the air above you (air pressure) be greater than or less than it is now?
What do you think causes wind? Don’t say beans!!!
If you lived in Kansas and observed a sudden drop in air pressure, what kind of weather would you expect to see soon?
 
Why do hot air balloons rise?
Air weighs  less than water, would you expect the pressure exerted by water  to be greater or less than the pressure exerted by the same volume of air?
The Gas Laws: ,[object Object],[object Object]
Temperature  - Temperature changes cause particle motion changes which cause a volume change.  Pressure  - Gases can be compressed, or squeezed, causing a change in the gas volume.
The Four Gas Law Variables: ,[object Object],[object Object],[object Object],[object Object]
Volume All gases must be enclosed in a container that, if there are openings, can be sealed with no leaks. The three-dimensional space enclosed by the container walls is called volume. When the generalized variable of volume is discussed, the symbol V is used.
Volume in chemistry is usually measured in liters (symbol = L)  or milliliters  (symbol = mL).   A mL is also called a cubic centimeter cm 3 A liter is also called a cubic decimeter dm 3
Temperature All gases have a temperature, usually measured in degrees Celsius (symbol = °C). Note that Celsius is capitalized since this was the name of a person (Anders Celsius). When the generalized variable of temperature is discussed, the symbol T is used.
There is another temperature scale which is very important in gas behavior. It is called the Kelvin scale (symbol = K). Note that K does not have a degree sign and Kelvin is captalized because this was a person's title (Lord Kelvin, his real name was William Thomson).
All gas law problems will be done with Kelvin temperatures. You can convert between Celsius and Kelvin like this: Kelvin = Celsius + 273 For example, 25 °C = 298 K, because  25 + 273 = 298.
Standard temperature is defined as  zero degrees Celsius  or  273 K.
Pressure Gas pressure is created by the molecules of gas hitting the walls of the container. This concept is very important in helping you to understand gas behavior. Keep it solidly in mind. I will use this idea of gas molecules hitting the wall often. When the generalized variable of pressure is discussed, the symbol P is used.
Three different units of pressure used in chemistry .  ,[object Object],[object Object],[object Object]
When working with gas laws, all pressure units must be the same in any calculation. 1 atm =  760 mm Hg =  101 kPa =  101,300 Pascals =  1013 mb =  29.92 in Hg If needed, be able to  convert  from one pressure unit to another.
[object Object],[object Object],[object Object],[object Object],[object Object]
Standard temperature and pressure =STP:
Standard temperature is  0 0 Celcius. But All gas calculations must use Kelvin temperatures. K =  0 C + 273
Standard pressure is 1 ATM  (at sea-level). mm Hg  is millimeters of mercury. This describes the height of a vertical column of mercury that the pressure will support against gravity. The unit  Torr  can be used to indicate mm Hg. The barometric pressure reported in U.S. weather reports is usually expressed as  inches  of mercury. There are 25.4 millimeters in one inch. kPa  is kiloPascals. A  Pascal  is a unit of force equal to a N / m 2 .  It is describing the pressure exerted by the molecules of the gas striking a surface. mb  is millibars.  One millibar is equal to 100 N / m 2 .  Crazy huh?
The last gas law variable Amount of Gas ,[object Object]
To be successful working gas law problems, do the following: ,[object Object]
What do you know?  ,[object Object]
What are you trying to find? ,[object Object]
Reread the question to see what conditions change. ,[object Object],[object Object]
Find the gas equation that connects the variables used in the problem . Boyles Charles Gay/Lussac
Plug the variables into the gas equation you’ve chosen
Rearrange the gas equation to solve for the “Find” variable. V T P
Plug and Chug ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]
Avagadro’s Law Equal volumes of gasses,  at the same temperature and pressure,  have equal numbers of particles.
Important points to note…. ,[object Object],[object Object],[object Object],[object Object]
Molar volume = volume of 1 mole of gas At STP, (273k, 1atm)  1 mole of any gas = 22.4 Liters
What is the molar mass of… 22.40 Liters of H 2   (g)
What is the molar mass of….. 22.40 Liters of N 2   (g)
What is the molar mass of….. 22. 40 liters of O 2   (g)
Calculate the number of liters of occupied by 2.5 moles of N 2  gas
Calculate the number of liters of occupied by 0.350 moles O 2  gas
The universal gas constant = R This is a constant that lets us solve “ideal gas” equation problems Think of it as a correction factor
Boyles law  Pressure and volume are inversely proportional P = V PV = ______
Charles Law Volume & Temperature are directly proportional V = T V  =____ T
Avagadro’s Law Volume & moles are directly proportional V = n V  = _______ n
If we rearrange….. PV  = R nT At STP what is the gas constant ??? (watch your units)

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Gas Laws Modified

  • 2. What gases are important for each of the following: O 2 , CO 2 and/or He? A. B. C. D.
  • 3. What gases are important for each of the following: O 2 , CO 2 and/or He? A. CO 2 B. O 2 /CO 2 C. O 2 D. He
  • 4. Gases are made up of molecules. Air consists of a mixture of gases, including nitrogen N 2 , Oxygen O 2 , and carbon dioxide CO 2 . Gases exert pressure on any surface with which they come in to contact. The gases in our atmosphere are subject to the Earth’s gravitational pull therefore the atmosphere is much denser nearer the Earths surface and less dense as we travel away from the planet.
  • 5. Some Gases in Our Lives oxygen O 2 nitrogen N 2 ozone O 3 argon Ar carbon dioxide CO 2 water H 2 O Noble gases : helium He neon Ne krypton Kr xenon Xe Other gases: fluorine F 2 chlorine Cl 2 ammonia NH 3 methane CH 4 carbon monoxide CO nitrogen dioxide NO 2 sulfur dioxide SO 2
  • 6. Pressure is one of the most easily measured properties of a gas. We define pressure as the force per unit area. P= Force/Area.
  • 7. Pascal: The SI unit of pressure. 1 Pascal = 1 N /m 2 = 1 kg x m/s 2 x 1/m 2 Named after Blaise Pascal
  • 8. Ice skates are familiar examples of the effects of pressure. The area of the blades of a skate are much smaller than, say, the soles of your feet. So if you strap on ice skates, your weight will act on an area much smaller than it would if you were wearing normal shoes. Since A decreases while F stays the same, the pressure you exert on the ice will be much greater if you're wearing skates. This pressure is often enough to melt a layer of ice, which allows your skate to glide smoothly across an ice rink. If you try the same maneuver with normal shoes, you will not generate enough pressure to melt the ice and won't get anywhere fast.
  • 9. Air pressure is the force exerted on you by the weight of tiny particles of air (air molecules). Although air molecules are invisible, they still have weight and take up space. We are usually unaware of the air pressure around us, probably because we are used to it. Since there's a lot of "empty" space between air molecules, air can be compressed to fit in a smaller volume.
  • 10. How much pressure are you under? Earth's atmosphere is pressing against each square inch of you with a force of 1 kilogram per square centimeter (14.7 pounds per square inch). The force on 1,000 square centimeters (a little larger than a square foot) is about a ton!
  • 11. Why doesn't all that pressure squash me? Remember that you have air inside your body too, that air balances out the pressure outside so you stay nice and firm and not squishy. Well…some of us are more squishy than others
  • 12. Run for Cover! Air pressure can tell us about what kind of weather to expect as well. When it's compressed, air is said to be "under high pressure". If a high pressure system is on its way, often you can expect cooler temperatures and clear skies. If a low pressure system is coming, then look for warmer weather, storms and rain.
  • 13.
  • 15. Barometer? Weather forecasters measure air pressure with a barometer . Barometers are used to measure the current air pressure at a particular location in "inches of mercury" or in "millibars" (mb). A measurement of 29.92 inches of mercury is equivalent to 1013.25 millibars. Crazy huh? Bar - A unit of measurement equivalent to 1×10 5 Pascals.
  • 16.
  • 17. Why do my ears pop as I increase altitude? As the number of molecules of air around you decreases, the air pressure decreases. This causes your ears to pop in order to balance the pressure between the outside and inside of your ear. Since you are breathing fewer molecules of oxygen, you need to breathe faster to bring the few molecules there are into your lungs to make up for the deficit. Air pressure on Mt. Everest is 670 mb less than on the Cayman Islands.
  • 18. 1. If you were on a mountain, would the weight of the air above you (air pressure) be greater than or less than it is now?
  • 19. What do you think causes wind? Don’t say beans!!!
  • 20. If you lived in Kansas and observed a sudden drop in air pressure, what kind of weather would you expect to see soon?
  • 21.  
  • 22. Why do hot air balloons rise?
  • 23. Air weighs less than water, would you expect the pressure exerted by water to be greater or less than the pressure exerted by the same volume of air?
  • 24.
  • 25. Temperature - Temperature changes cause particle motion changes which cause a volume change. Pressure - Gases can be compressed, or squeezed, causing a change in the gas volume.
  • 26.
  • 27. Volume All gases must be enclosed in a container that, if there are openings, can be sealed with no leaks. The three-dimensional space enclosed by the container walls is called volume. When the generalized variable of volume is discussed, the symbol V is used.
  • 28. Volume in chemistry is usually measured in liters (symbol = L) or milliliters (symbol = mL). A mL is also called a cubic centimeter cm 3 A liter is also called a cubic decimeter dm 3
  • 29. Temperature All gases have a temperature, usually measured in degrees Celsius (symbol = °C). Note that Celsius is capitalized since this was the name of a person (Anders Celsius). When the generalized variable of temperature is discussed, the symbol T is used.
  • 30. There is another temperature scale which is very important in gas behavior. It is called the Kelvin scale (symbol = K). Note that K does not have a degree sign and Kelvin is captalized because this was a person's title (Lord Kelvin, his real name was William Thomson).
  • 31. All gas law problems will be done with Kelvin temperatures. You can convert between Celsius and Kelvin like this: Kelvin = Celsius + 273 For example, 25 °C = 298 K, because 25 + 273 = 298.
  • 32. Standard temperature is defined as zero degrees Celsius or 273 K.
  • 33. Pressure Gas pressure is created by the molecules of gas hitting the walls of the container. This concept is very important in helping you to understand gas behavior. Keep it solidly in mind. I will use this idea of gas molecules hitting the wall often. When the generalized variable of pressure is discussed, the symbol P is used.
  • 34.
  • 35. When working with gas laws, all pressure units must be the same in any calculation. 1 atm = 760 mm Hg = 101 kPa = 101,300 Pascals = 1013 mb = 29.92 in Hg If needed, be able to convert from one pressure unit to another.
  • 36.
  • 37. Standard temperature and pressure =STP:
  • 38. Standard temperature is 0 0 Celcius. But All gas calculations must use Kelvin temperatures. K = 0 C + 273
  • 39. Standard pressure is 1 ATM (at sea-level). mm Hg is millimeters of mercury. This describes the height of a vertical column of mercury that the pressure will support against gravity. The unit Torr can be used to indicate mm Hg. The barometric pressure reported in U.S. weather reports is usually expressed as inches of mercury. There are 25.4 millimeters in one inch. kPa is kiloPascals. A Pascal is a unit of force equal to a N / m 2 . It is describing the pressure exerted by the molecules of the gas striking a surface. mb is millibars. One millibar is equal to 100 N / m 2 . Crazy huh?
  • 40.
  • 41.
  • 42.
  • 43.
  • 44.
  • 45. Find the gas equation that connects the variables used in the problem . Boyles Charles Gay/Lussac
  • 46. Plug the variables into the gas equation you’ve chosen
  • 47. Rearrange the gas equation to solve for the “Find” variable. V T P
  • 48.
  • 49. Avagadro’s Law Equal volumes of gasses, at the same temperature and pressure, have equal numbers of particles.
  • 50.
  • 51. Molar volume = volume of 1 mole of gas At STP, (273k, 1atm) 1 mole of any gas = 22.4 Liters
  • 52. What is the molar mass of… 22.40 Liters of H 2 (g)
  • 53. What is the molar mass of….. 22.40 Liters of N 2 (g)
  • 54. What is the molar mass of….. 22. 40 liters of O 2 (g)
  • 55. Calculate the number of liters of occupied by 2.5 moles of N 2 gas
  • 56. Calculate the number of liters of occupied by 0.350 moles O 2 gas
  • 57. The universal gas constant = R This is a constant that lets us solve “ideal gas” equation problems Think of it as a correction factor
  • 58. Boyles law Pressure and volume are inversely proportional P = V PV = ______
  • 59. Charles Law Volume & Temperature are directly proportional V = T V =____ T
  • 60. Avagadro’s Law Volume & moles are directly proportional V = n V = _______ n
  • 61. If we rearrange….. PV = R nT At STP what is the gas constant ??? (watch your units)