1. Pressure Unit 10 Chapter 13

2. The Weight of the World The atmosphere is 78% N 2, 21% O 2, 1% Ar, and < 1% other gases. The atmosphere is 78% N 2, 21% O 2, 1% Ar, and < 1% other gases. 99.9% of the Earth’s Atmosphere can be found in the Troposphere (0 to 11 km) and Stratosphere (11 to 50 km). 99.9% of the Earth’s Atmosphere can be found in the Troposphere (0 to 11 km) and Stratosphere (11 to 50 km). All that gas has a weight. That weight is pushing down on us all the time. All that gas has a weight. That weight is pushing down on us all the time.

3. Weight of the World II A 1 in 2 column of air weighs approximately 14.7 lbs. A 1 in 2 column of air weighs approximately 14.7 lbs. This is defined as 1 atmosphere of pressure This is defined as 1 atmosphere of pressure 1 atm = 14.7 psi (pounds per square inch = lb/in 2 ) 1 atm = 14.7 psi (pounds per square inch = lb/in 2 )

4. Forcing the Issue Pressure is the amount of force being exerted on a surface. Pressure is the amount of force being exerted on a surface. The formula is: The formula is: P = Force  Area (P = F/A) P = Force  Area (P = F/A) When dealing with the atmosphere, When dealing with the atmosphere, Pressure can be thought of as the weight of the atmosphere on top of an object. Pressure can be thought of as the weight of the atmosphere on top of an object.

5. Weight of the World III The total weight of atmosphere on top of an object: Since P = F/A, then F = P*A The total weight of atmosphere on top of an object: Since P = F/A, then F = P*A Calculate surface area (use in 2 ) Calculate surface area (use in 2 ) Multiply by 14.7 psi Multiply by 14.7 psi What force is being exerted on the desk? What force is being exerted on the desk? L = 24.25”, W = 18.25” L = 24.25”, W = 18.25” 24.25” x 18.25” = 442.6 in 2 24.25” x 18.25” = 442.6 in 2 442.6 in 2 x 14.7 psi = about 6500 lbs 442.6 in 2 x 14.7 psi = about 6500 lbs

6. When is Length = To Pressure?!? Nature abhors a vacuum; however, mercury doesn’t mind it so much! Air pushes down on a pool of mercury. Height of 1” column of mercury ~760 mm.

7. Measuring It Gas Pressure can be measured using a Manometer (enclosed). Or a Barometer (open)

8. Equal to Each Other Additional units for measuring air pressure Additional units for measuring air pressure  14.6959488 psi  1 atm (exact)  760 mmHg (exact)  760 torr (exact)  29.92125984 inHg  1.01325 bar (exact)  101,325 Pa (exact)  101.325 kPa (exact) These values are all equal to each other! In calculations, you have to use the correct # of Sig Figs for psi & inHg.

9. Conversions Use equalities to interconvert Use equalities to interconvert What is the pressure in mmHg if the news gives it as 29.85 inHg? What is the pressure in mmHg if the news gives it as 29.85 inHg? 29.85 inHg  29.92 inHg * 760 mmHg 29.85 inHg  29.92 inHg * 760 mmHg 758.2219251 758.2219251 4 sig figs 4 sig figs 758.2 mmHg 758.2 mmHg

10. Partially Acceptable The Law of Partial Pressures The Law of Partial Pressures Declared by John Dalton (remember him?) Declared by John Dalton (remember him?) States Total Pressure is the sum of the individual pressures added together. States Total Pressure is the sum of the individual pressures added together. P T = P 1 + P 2 + P 3 + … P T = P 1 + P 2 + P 3 + … Pneumatic Chemist # 1!!!

11. Check some Grey Matter Venus’ atmosphere consists of CO 2 & N 2. Venus’ atmosphere consists of CO 2 & N 2. What is the total pressure on Venus in psi? What is the total pressure on Venus in psi? CO 2 partial pressure = 87.6 atm CO 2 partial pressure = 87.6 atm N 2 partial pressure = 3.2 atm N 2 partial pressure = 3.2 atm P T = 87.6 + 3.2 = 90.8 atm P T = 87.6 + 3.2 = 90.8 atm 90.8 atm  1 atm * 14.7 psi = 1,334.76 90.8 atm  1 atm * 14.7 psi = 1,334.76 1,330 psi (3 sig figs) 1,330 psi (3 sig figs)

12. PP & n Assuming constant volume and temp in a mixture of gases, the partial pressure of a gas (P 1 ) is proportional to the moles of the gas (n 1 ), therefore:

13. Air Vs. Can Pour a little water in an empty soda can. Place on hot plate (on high) Fill a large beaker with water and set to the side of the hot plate. Take measurements of other can then add water and put on hot plate, also. Calculate the surface area of the cans. When soda can boils, wait ~30 seconds. Quickly turn can into top of filled beaker. Observe.

14. Gas Collection Density higher than air Density lower than air Low solubility in water

15. Fun with Water! For gases collected over a liquid, the partial pressure of the liquid must be accounted for. Vapor is present because some of the molecules are able to escape the surface of the liquid. The vapor pressure of the liquid is dependent on temperature.

16. Vapor Pressure

17. Attack of the Vapors A sample of gas is collected over water at room temperature. At that temperatures, water’s vapor pressure is 17.3 mmHg If the total pressure is 764.7 mmHg, what is the partial pressure of the gas? 764.7 – 17.3 = 747.4 mmHg

18. Phasing it Out Melting & Boiling points are directly affected by two things: Temperature Pressure The phase boundaries vary depending on those two factors.

19. Phase Diagrams Triple Point Critical Point Sublimation / Deposition Boiling / Condensing 0°C

20. Standard Stuff Since gases change a lot with temperature & pressure, several institutions define “standard conditions” Since gases change a lot with temperature & pressure, several institutions define “standard conditions” Called “STP” Called “STP” IUPAC = 0°C & 1 bar IUPAC = 0°C & 1 bar NIST = 20°C & 1 atm NIST = 20°C & 1 atm

21. Moles at STP Original STP was 0°C & 1 atm Original STP was 0°C & 1 atm 1 mole of any gas (including diatomics) occupies 22.4 Liters at STP 1 mole of any gas (including diatomics) occupies 22.4 Liters at STP We can measure amount of gas without weighing it. We can measure amount of gas without weighing it. First, calculate the number of moles, and then multiply by 22.4 L/mol to get volume (in Liters) First, calculate the number of moles, and then multiply by 22.4 L/mol to get volume (in Liters) For this class, use these values for STP!

22. Check More Grey Matter What vol does 50.0 g of O 2 require at STP? What vol does 50.0 g of O 2 require at STP? n = m / Mw n = m / Mw = 50.0 g / (16.00 * 2) = 50.0 g / (16.00 * 2) = 1.5625 = 1.56 moles O 2 = 1.5625 = 1.56 moles O 2 V = 1.5625 moles O 2 * 22.4 L/mol V = 1.5625 moles O 2 * 22.4 L/mol = 35 = 35 = 35.0 L O 2 (3 sig figs) = 35.0 L O 2 (3 sig figs)