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.

834 torr  kPa 834 torr x torr kPa = kPa

3.5 atm  torr 3.5 atm x atm torr = torr

532 torr  mm Hg 532 mm Hg x mm Hg torr = torr

1)-273⁰C  K 2) 298 K  ⁰C = 0 K = 25⁰C

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

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

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

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)

Kinetic Molecular Theory / Diffusion Notes Watch the video and read the article. Write down the 4 points of the kinetic molecular theory. Watch the video. – 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) atm, kPa, 40.5 torr mL atm L K, 300 K, 223 K, 0 K K atm 3. V 2 = 100 mL, V 1 = 280 mL mL mL