 Chemistry Honors/AP

Course Materials are always under revision! Weblecture content may change anytime prior to two weeks before scheduled chat session for content. Homework

Homework

WebLecture: The Ideal Gas Law

Kotz and Triechel, Chemistry and Chemical Reactivity Chapter 10: 1-3

• 10.1: We know how to measure volume in standard metric units of distance (meters to liters), and we've already used temperature units (%deg;C, Kelvin). Now we look at units used to measure pressure: 1 atm (atmosphere) = 760 mmHg = 1.013 * 105 P (Pascal) = 101.3 kPa (kilo Pascal) = 1.013 bar.
• 10.2: Over several centuries, different philosophers recognized certain relationships between pressure, volume, temperature, and the amount of gas in a sample:
• Boyle's Law: Pressure * Volume = Constant
• Charles's Law: Volume = Constant * Temperature
• Avogadro's Law: Volume = number of molecules * Constant
• 10.3: We can combine the three laws we know now into a single law: PV = nRT. Since a mole of any gas has a molar mass M, a sample of n molecules has a mass m = nM, or n = m/M. We also know that density = mass/volume, so we can rewrite the gas law in terms of molar mass and mass: PV = (m/M) RT, and P(m/d) = nRT = P(m/d) = (m/M) RT so d = MP/RT. These relationships allow us to determine molar mass M for a substance.

Formula

1 Pa = 1 newton/meter2

1 atm = 760 mmHg = 101.325 kPa

Boyle's Law: PV = C

Charles's Law: V = CT

Avogadro's Law: V = nC

Combind gas law: P1V1/T1 = P2V2/T2

Ideal Gas Law: PV = nRT

Videos for Chapter 10: Gases and their Properties

Review the Videos at Thinkwell Video Lessons.

• Under "Gases: Gases and Gas Laws"
• Properties of Gas laws
• Boyle's Law
• Charles's Law
• The Combined Gas Law