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Ideal Gas Law & Gas Stoichiometry

Ideal Gas Law & Gas Stoichiometry. Ideal Gas Law. P V = n R T P = Pressure (atm) V = Volume (L) T = Temperature (K) n = number of moles R is a constant, called the Ideal Gas Constant

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Ideal Gas Law & Gas Stoichiometry

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  1. Ideal Gas Law & Gas Stoichiometry

  2. Ideal Gas Law P V = n R T • P = Pressure (atm) • V = Volume (L) • T = Temperature (K) • n = number of moles • R is a constant, called the Ideal Gas Constant • Instead of learning a different value for R for all the possible unit combinations, we can just memorize one value and convert the units to match R. • R = 0.0821 L atm / mol K

  3. PV = nRT • Calculate the number of moles of a gas contained in a 3.0 L vessel at 300.0K with a pressure of 1.50 atm

  4. PV = nRT • n = ? • V = 3.0 L • T = 300.0 K • P = 1.50 atm • PV = nRT • (1.50 atm)(3.0 L) = n (0.0821L atm / mol K)(300.0 K) • n = 0.18 mol

  5. Example Dinitrogen monoxide (N2O), laughing gas, is used by dentists as an anesthetic. If 2.86 mol of gas occupies a 20.0 L tank at 23°C, what is the pressure (mmHg) in the tank in the dentist office? Note: 1atm = 760 mm Hg

  6. Avogadro’s Principle • Avogadro’s Principle – equal volumes of gases at equal temperature and pressure contain the same number of particles • Molar volume – the volume of gas that 1 mole of a substance occupies at STP • At STP 1 mol of a gas = 22.4 L • New conversion factor at STP ONLY! 1 mol 22.4 L

  7. Example • Calculate the volume 0.881 mol of a gas will occupy at STP. • 0.881 mol x 22.4 L = 19.7 L 1 mol (You could also have worked this out with the ideal gas law equation)

  8. Example • Calculate the volume that 2.000 kg of methane would occupy at STP. • 2.000 kg x 1x10 3g x 1 mol x 22.4 L = 1kg 16.05g 1 mol • 2791 L CH4

  9. Gas Stoichiometry Rules • Balance the equation. • STARTING IN VOLUME: • Use the ideal gas law to find moles of the gas. • Use the molar ratio. • Convert from moles to what you want. • STARTING IN MOLES: • Use the molar ratio. • Use the ideal gas law to convert from moles to volume.

  10. Problem #1 • How many grams of copper (II) carbonate are required to produce 11.2 dm3 of carbon dioxide at 22.3° C and standard pressure? • 57.1 g CuCO3

  11. Problem #2 • How many grams of potassium chlorate are required to produce 22.40 liters of oxygen at 25.00° C and 202.6 kPa? • 149.7 g KClO3

  12. Problem #3 • How many grams of water are produced with 10.0 dm3 of carbon dioxide at 273° C and standard pressure by the combustion of ethane? • 6.0 g H2O

  13. Problem #4 • How many grams of magnesium are required to react with hydrochloric acid to produce 0.50 dm3 of hydrogen at 21° C and standard pressure? • 0.50 g Mg

  14. Problem #5 • How many grams of sodium are required to react with water to produce 2.40 dm3 of hydrogen at 25° C and standard pressure? • 4.6 g Na

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