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To understand the ideal gas law and use it in calculations

Objectives. To understand the ideal gas law and use it in calculations To understand the relationship between the partial and total pressure of a gas mixture To do calculations involving Dalton’s law of partial pressures To understand the molar volume of an ideal gas

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To understand the ideal gas law and use it in calculations

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  1. Objectives • To understand the ideal gas law and use it in calculations • To understand the relationship between the partial and total pressure of a gas mixture • To do calculations involving Dalton’s law of partial pressures • To understand the molar volume of an ideal gas • To learn the definition of STP • To do stoichiometry calculations using the ideal gas law

  2. A. The Ideal Gas Law • Boyle’s Law V = k(at constant T and n) P • Charles’s Law V = bT (at constant P and n) • Avogadro’s Law V = an (at constant T and P) We can combine these equations to get

  3. A. The Ideal Gas Law • Rearranging the equation gives the ideal gas law: • PV = nRT • R is a constant = 0.08206 L atm • mol K • Note the units that are used with this constant

  4. The Combined Gas Law Ideal Gas Law: PV = nRT P1V1 = nRT1or P1V1/T1 = nR P2V2 = nRT2or P2V2/T2 = nR Combined Gas Law: P1V1/T1 = P2V2/T2 (for a constant number of moles)

  5. B. Dalton’s Law of Partial Pressures • What value do we measure for the pressure of a gas as we mix different gases in a container? Dalton’s law of partial pressures • For a mixtures of gases in a container, the total pressure exerted is the sum of the partial pressures of the gases present. • Ptotal = P1 + P2 + P3 + …….

  6. B. Dalton’s Law of Partial Pressures • The pressure of the gas is affected by the number of particles. • The pressure is independent of the nature of the particles.

  7. B. Dalton’s Law of Partial Pressures Two crucial things we learn from this are: • The volume of the individual particles is not very important • The forces among the particles must not be very important

  8. B. Dalton’s Law of Partial Pressures Collecting a gas over water • Total pressure is the pressure of the gas + the vapor pressure of the water. Collecting Hydrogen

  9. B. Dalton’s Law of Partial Pressures Collecting a gas over water • How can we find the pressure of the gas collected alone?

  10. C. Gas Stoichiometry Molar Volume • Standard temperature and pressure (STP) • 0oC and 1 atm • For one mole of a gas at STP, what is the volume? • Molar volume of an ideal gas at STP = 22.4 L

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