1. Tuesday April 21 Objective: Describe the main points of the kinetic molecular theory. Checkpoint: Convert the following temperatures and pressures: 834 torr  kPa 3.5 atm  torr 532 mm Hg  torr -273⁰C  K 298 K  ⁰C Homework: – Combined Gas Laws worksheet due Wed/Thurs – Study for quiz on Wed/Thurs (temp & pressure conversions, combined gas law). – Last day to for stoich re-take is Friday.

2. 834 torr  kPa 834 torr x torr kPa = 760 101 111 kPa

3. 3.5 atm  torr 3.5 atm x atm torr = 1 760 2660 torr

4. 532 torr  mm Hg 532 mm Hg x mm Hg torr = 760 532 torr

5. 1)-273⁰C  K 2) 298 K  ⁰C -273 + 273 = 0 K 298 - 273 = 25⁰C

6. Gay-Lussac’s Law: Pressure and Temperature When temperature increases, pressure increases. When temperature decreases, pressure decreases. Think about why this is true: COLD HOT

7. Boyle’s Law: Pressure and Volume As volume decreases, pressure increases. As volume increases, pressure decreases.

8. Charles’ Law: Volume and Temperature When temperature increases, volume increases. When temperature decreases, volume decreases.

9. Combined Gas Law T 1 P 2 V 2 = T 2 P 1 V 1 Temperature (T) MUST be in Kelvin! P = pressure (units must match) V = volume (units must match)

12. Kinetic Molecular Theory / Diffusion Notes http://goo.gl/FKBuoO Watch the video and read the article. Write down the 4 points of the kinetic molecular theory. http://goo.gl/KX3pUZ Watch the video. http://goo.gl/KX3pUZ – Describe the difference that happens when bromine gas is released into air, and when bromine gas is released into a vacumm. – Which travels faster, NH 3 gas or HCl gas? How do you know? Answer key to Gas Laws Calculations (Standard Conditions = 0⁰C and 1 atm) 1.0.164 atm, 323.2 kPa, 40.5 torr4. 142 mL7. 2.6 atm10. 3.41 L 2. 273 K, 300 K, 223 K, 0 K5. 121 K8. 0.36 atm 3. V 2 = 100 mL, V 1 = 280 mL6. 406 mL9. 14.6 mL