Today is Wednesday, May 25th, 2016 Pre-Class: Yep, our test is next class. Indeed, we’re doing review today. Certainly, it will be posted online.

Today’s Agenda Mystery Gas Law Practice ExploreLearning Gizmo/Quia Quiz Concepts Review General Review

Review Game You remember the rules: Each of you writes down an answer without looking or talking or gesturing or smiling or anything. We compare answers. Both right = 2 points One right = 1 point None right = 0 points

Review Question 1 When volume is kept constant, what happens to pressure as temperature rises? Pressure increases.

Review Question 2 What law summarizes that relationship between temperature and pressure? Gay-Lussac’s Law.

Review Question 3 Real gases tend not to behave according to which theory? Kinetic theory.

Review Question 4 BONUS NON-CHEMISTRY QUESTION You may wager any/all of your points. Category: Music Who invented the synthesizer? Robert Moog in 1967.

Review Question 5 What is pressure? Force per unit area OR the result of collisions of particles with the walls of a container.

Review Question 6 Atmospheric pressure is typically 0.823 atm in Denver. If you have a can of soda and the air above that soda is at 612 mm Hg, what happens when you open the can? Air rushes in (612 mm Hg = 0.805 atm).

Review Question 7 If you know the partial pressures of all gases in a container, how do you calculate the total pressure? Add them together (Dalton’s Law).

Review Question 8 Why does liquid nitrogen cause balloons placed in it to shrink? Liquid nitrogen is so cold that it lowers the temperature in the balloon, slowing down the molecules and reducing the volume (Charles’ Law).

Review Question 9 If you have 48 grams of oxygen gas at 100 atm and 27 °C, what volume does it occupy? 48 grams O2 = 1.5 mol O2 100 atm = 10130 kPa 27 °C = 300 K Using the Ideal Gas Law, V = 0.369 L.

Review Question 10 Inside one 20 L container are three gases: Oxygen Gas (Partial Pressure = 5.3 atm) Nitrogen Gas (Partial Pressure = 2001 torr) Hydrogen Gas (Partial Pressure = 150 kPa) What is the total pressure on the container? 5.3 atm = 536.89 kPa 2001 torr = 266.71 kPa Then add 150 kPa… Total Pressure = 953.6 kPa Or 9.41 atm or 7154.35 torr/mm Hg or 138.38 psi.

Review Question 11 You have a 20 L container at 250 K. In that container you have 2 moles of nitrogen gas. You also have 5 moles of hydrogen gas. What is the total pressure on the container?

Review Question 12 If given volume and temperature at an unknown constant pressure, which law would best be used to make calculations? Charles’ Law.

Review Question 13 BONUS NON-CHEMISTRY QUESTION You may wager any/all of your points. Category: Food and Drink Which currently available beverage was originally known as “Brad’s Drink?” Pepsi.

Review Question 14 A 500 mL machine compresses air at 400 torr and 35 °C to 13 mL at 50 °C. What is the ending pressure of the air? 16133.866 torr (Combined Gas Law)

Review Question 15 A blimp has 6.0 x 107 liters of helium inside. How many moles does this contain if the pressure is 140 kPa at 24 °C? 3,401,831.643 mol He. You CANNOT just divide 6.0 x 107 L by 22.4 L to get moles – that only works at STP.