The Ideal Gas Law Objectives:

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Gas Laws Robert Boyle Jacques Charles Amadeo Avogadro
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Presentation transcript:

The Ideal Gas Law Objectives: 7.0 Explain the behavior of ideal gases in terms of pressure, volume, temperature, and number of particles using Charles's law, Boyle's law, Gay-Lussac's law, the combined gas law, and the ideal gas law. 6.0 Solve stoichiometric problems involving relationships among the number of particles, moles, and masses of reactants and products in a chemical reaction.

Intro What will happen to the pressure in a tire as air is added, if the volume and temperature of the tire do not change? So the amount of gas (moles) and the pressure both change. Remember: Combined Gas Law: P1V1 = P2V2 T1 T2

Ideal Gas Law Since the ratio remains the same, then we can say it is constant. We call the constant k. k is a constant based on the amount of gas (n) present, where k = nR. (R is an experimentally determined constant, called the ideal gas constant, and equal to 0.0821 L-atm/mol-K. Ideal gas law equation: PV=nRT

What is an Ideal Gas? A gas that follows all the gas laws When do gases not follow the gas laws?: Gases tend not to behave “ideally” under very high pressures and low temperatures, as there is more inter-particular interactions. Also, polar particles (like water vapor) are more attracted to each other because of their partial charges. Large particles interact more.

Applying the Ideal Gas Law PV=nRT: What is n? How can n be used to find the mass of a gas present? From stoichiometry, what else can be determined from n? How?????? Substitutions in the ideal gas equation: n = mass (m)/molar mass (M) Rearrange the formula to solve for M. Density (D) = ?????

Examples & Assignment Examples: p.437 (41, 45) and p.438 (46, 50) Other Practice Problems can be used to practice and make sure you know how to solve problems. Assignment: Section Assessment: p. 439 (53, 55) 449: 97-100

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