ch67answerkey.pdf | |
File Size: | 139 kb |
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Need extra practice problems? Check below:
gas_laws_201314_review_sheet_w_answers_2.doc | |
File Size: | 37 kb |
File Type: | doc |
Need to know what you can have on your notecard for the test?
Pressure conversions: 1 atm = 101.3 kPa = 760 torr = 760 mmHg
R Values:
- 0.0821 L*atm/mol*K
- 8.314 L*kPa/mol*K
1 mol = 22.4 L of any gas at STP
V1/T1 = V2/T2 P1/T1 = P2/T2 P1V1 = P2V2 V1P1/T1 = V2P2/T2 pV=nRT
r1/r2 = (square root of M2)/(square root of M1)
Pressure conversions: 1 atm = 101.3 kPa = 760 torr = 760 mmHg
R Values:
- 0.0821 L*atm/mol*K
- 8.314 L*kPa/mol*K
1 mol = 22.4 L of any gas at STP
V1/T1 = V2/T2 P1/T1 = P2/T2 P1V1 = P2V2 V1P1/T1 = V2P2/T2 pV=nRT
r1/r2 = (square root of M2)/(square root of M1)
Click here for the powerpoint for Chapters 6 & 7.
Chapter 6 Online Lecture Timestamps:
Introduction: Beginning - 4:16 Units of Pressure Conversions: 4:16 - 8:56 STP: 8:56 - 9:25 Partial Pressures: 9:25 - 15:17 Gas Laws: Charles' Laws: 15:17 - 20:45 Gas Laws: Gay - Lussac's Law: 20:45 - 23:21 Gas Laws: Boyle's Law: 23:21 - 26:20 Combined Gas Laws: 26:20 - 26:40 Deciding Which to Use: 26:40 - End |
Chapter 6 Online Lecture Timestamps:
Avogadro's Law: Beg - 2:45 Ideal-Gas Equation: 2:45 - 4:30 Deriving "R" Constant: 4:30 - 7:52 Example Problem Ideal-Gas Law: 7:52 - 15:16 Real Gases: 15:16 - 16:38 Kinetic-Molecular Model: 16:38 - 19:34 Effusion & Diffusion: 19:34 - End |
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