Reading: All of Chapter 15 HW 13.1: Due 7/10/14

Reading: All of Chapter 15 • HW13.1: Due 7/10/14 • Chap. 13 #s 7, 9, 15, 17, 21, 23, 27, 31, 35, 37, 39, 43, 49, 55, 57, 59, 63 • HW 13.2: Due 7/14/14 • Chap. 13 #s 66, 67, 71, 73, 74, 78, 79, 85, 87, 89, 95, 112, 143 • Lab Tomorrow (WET LAB!) • Monday – Nomenclature Proficiency Quiz 2

Increases and Decreases in Pressure Effect of temperature

LOWER pressure HIGHER pressure LOWER temperature HIGHER temperature

T P Increases and Decreases in Pressure Effect of temperature Temperature goes up, pressure goes up Temperature goes down, pressure goes down Temperature and pressure are DIRECTLY related

Increases and Decreases in Pressure Effect of volume

LOWER pressure HIGHER pressure LARGER volume SMALLER volume

V P Increases and Decreases in Pressure Effect of volume Volume goes up, pressure goes down Volume goes down, pressure goes up Volume and pressure are INVERSELY related

Increases and Decreases in Pressure Effect of number of particles

LOWER pressure HIGHER pressure FEWER particles MORE particles

# part P Increases and Decreases in Pressure Effect of number of particles # of particles goes up, pressure goes up # of particles goes down, pressure goes down # of particles and pressure are DIRECTLY related

“Laws” Boyle’s Law – Pressure and Volume Volume and pressure are inversely related P x V must remain constant PV = k P1V1 = P2V2 assumes temperature and # of particles are constant

= k “Laws” Charles’s Law – Temperature and Volume Temperature and volume are directly proportional TEMPERATURE MUST BE IN KELVIN!!!! assumes pressure and # of particles are constant

= k “Laws” Gay-Lussac’s Law – Temperature and Pressure Temperature and pressure are directly proportional TEMPERATURE MUST BE IN KELVIN!!!! assumes volume and # of particles are constant

= k “Laws” Avogadro’s Law – Particles and Volume Particles and volume are directly proportional assumes temperature and pressure are constant

Molar Mass molar has nothing to do with teeth!!!!!!! molar means “per 1 mole” molar mass means mass per 1 mole

Molar Volume molar means “per 1 mole” molar volume means volume per 1 mole molar volume means volume per 1 mole OF GAS

GASES • All gases at the same temperature have the same molar volume (all at 1 atm) He CO2 1 mol @ 0 oC 22.4 L 22.4 L 1 mol @ 100 oC 30.6 L 30.6 L 1 mol @ 1000 oC 104.5 L 104.5 L

Molar Volume 1 mol of ANY gas = 22.4 L of gas 1 mol of ANY gas = 22.4 L of gas @ STP STP = Standard Temperature and Pressure HUH?!?!?! 0 oC 273 K 1 atm 760 torr 760 mmHg

Molar Volume 1 mol of ANY gas = 22.4 L of gas @ STP 1 mol N2(g) = 22.4 L N2(g) 1 mol CO2(g) = 22.4 L CO2(g) 1 mol HCl(g) = 22.4 L HCl(g)

Avogadro’s # The mole Only 2 options of what to do with the mole: mole particles molar mass mole mass mole-to-mole ratio mole “X” mole “Y”

Avogadro’s # The mole Only 2 options of what to do with the mole: mole particles molar mass mole mass mole-to-mole ratio mole “X” mole “Y” molar volume mole volume

mol RECAP 1 mol H2(g) = 6.022x1023 molecules H2(g) 1 mol H2(g) = 2.02 g H2(g) 1 mol H2(g) = 22.4 L H2(g) 1 mol H2(g) = 2 mol H(g)

more mol calculations What mass of chlorine gas occupies 13.90 L at STP? 1 mol Cl2(g) = 70.90 g Cl2(g) 1 mol Cl2(g) = 22.4 L Cl2(g) 43.99598214 g Cl2(g) 44.0 g Cl2(g) 1 mol Cl2(q) = 6.022x1023 molecules Cl2(g)

“Laws” Combined Gas Law – Pressure, Temperature and Volume Combination of Boyle’s, Charles’s, and Gay-Lussac’s P1V1 = P2V2 assumes # of particles is constant

“Laws” Combined Gas Law – Pressure, Temperature and Volume Combination of Boyle’s, Charles’s, and Gay-Lussac’s assumes # of particles is constant

“ “Laws” ” “Super Combined Gas Law” – Pressure, Temperature, Particles, and Volume Combination of Boyle’s, Charles’s, Avogadro’s, and Gay-Lussac’s

“ “Laws” ” You need to know how these variables are related P V P T P n T n V T V n

Using Ratios Let’s say that we want to multiply 6 by the ratio above that will make it get bigger: <1, so the answer is smaller than 6 >1, so the answer is larger than 6 Larger number on top of the ratio  larger answer (number goes up) Larger number on bottom of the ratio  smaller answer (number goes down)

Using Ratios Let’s say that we want to multiply 31 by the ratio above that will make it get smaller: <1, so the answer is smaller than 31 >1, so the answer is larger than 31 Larger number on top of the ratio  larger answer (number goes up) Larger number on bottom of the ratio  smaller answer (number goes down)

Did you get it? A steel container filled with nitrous oxide at 15.0 atm is cooled from 25.0 ºC to -40.0 ºC. Calculate the final pressure. TEMPERATURE MUST BE KELVIN! or T so P must

Did you get it? A steel container filled with nitrous oxide at 15.0 atm is cooled from 25.0 ºC to -40.0 ºC. Calculate the final pressure.

Did you get it? A nitrogen gas sample occupies 50.5 mL at -80.0 ºC and 1250 torr. What is the volume at STP?

Dalton’s law of partial pressures states that the total pressure of a gaseous mixture is equal to the sum of the individual pressures of each gas. P1 + P2 + P3 + … = Ptotal The pressure exerted by each gas in a mixture is its partial pressure, Pn.

An atmospheric sample contains nitrogen, oxygen, argon, and traces of other gases. If the partial pressure of nitrogen is 587 mmHg, oxygen is 158 mmHg, and argon is 7 mmHg, what is the observed pressure as read on the barometer?

Reading: All of Chapter 15 HW 13.1: Due 7/10/14