Science Starter (Week 12, Day 2, 4/26/16)

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Presentation transcript:

Science Starter (Week 12, Day 2, 4/26/16) Grab a calculator Science Starter (Week 12, Day 2, 4/26/16) Place HW on Desk How many moles are present in 64 gram of Oxygen (O2)? What is the atmospheric pressure (atm) when the outside has a pressure of 1650 torr? 1.0 L of a gas at 1 atm is compressed to .473L. What is the new pressure of the gas? Nitrogen (N2) gas under a pressure of 2.3 atm and at a temperature of 293 K occupies a 500.0 mL container. How many grams of gas are in the container?

Objective SWBAT calculate problems using Dalton’s Law of Partial Pressure SWBAT use the gas laws to determine moles of reactant or product NOT at STP

Agenda Science Starter Announcements Notes Unit 6 Stations Dalton’s Law of Partial Pressures Unit 6 Stations

Announcements Tuesday: Dalton’s Law Wednesday: Unit 6 Review Thursday: Unit 6 Test Friday: CIA #2 Review Day (Units 1 -3) Monday (5/2): CIA #2 Review Day (Units 4-6) Tuesday (5/3): CIA #2 Test Day

Unit 6: Gas Laws Dalton’s Law of Partial Pressure

Notes: Partial Pressure Dalton's Law of Partial Pressure = The pressure of a mixture of gases is equal to the sum of the pressures of all of the individual gases alone. PressureTotal = Pressure1 + Pressure2 ... Pressuren

Example 1. A container holds parts of oxygen, nitrogen, and helium gas. The total gas pressure is 30 atm. If oxygen takes holds 12 atm of pressure and nitrogen holds 11 atm, what pressure is given off by helium?

Dalton’s Law of Partial Pressures V and T are constant P2 Ptotal = P1 + P2 P1

Example 2. The total pressure in a closed system containing N2, O2, and CO2 is 30 atm. If the partial pressure of N2 is 4 atm, and the partial pressure of O2 is 6 atm, what is the partial pressure of CO2?

Stations 6.1 Gas & Pressure 6.2 Pressure Conversions 6.3 Gas Laws (Ideal or Combined