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Chapter 14-3

Chapter 14-3. I. Avogadro’s Principle A. Equal volumes of gases at same T and P contain equal #’s of molecules B. H 2 + Cl 2 → 2HCl 1 vol. 1 vol. 2 vol. 1 mol 1 mol 2 mol. Chapter 14-4. II. Molar Volume of Gases

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Chapter 14-3

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  1. Chapter 14-3 I. Avogadro’s Principle A. Equal volumes of gases at same T and P contain equal #’s of molecules B. H2 + Cl2→ 2HCl 1 vol. 1 vol. 2 vol. 1 mol 1 mol 2 mol

  2. Chapter 14-4 II. Molar Volume of Gases A. 1 mole = 6.022 x 10 23 molecules B. STP = 22.4L C. 1 mol 22.4L D. 1 cm3 = 1 mL III. Practice problems 1. At STP, what is the volume of 7.08 mol of nitrogen gas? 159 L N2

  3. Practice problems 2. At STP, a sample of neon gas occupies 550. cm3. How many moles of neon gas does this represent? .0246 mol Ne 3. What is the mass of 1.33 x 104 mL of oxygen at STP? 19.0 g O2 4. What is the volume of 77.0g of nitrogen dioxide gas at STP? 37.5L NO2

  4. Ideal Gas Law • PV = nRT • R = .0821 L x atm/ mol x K • n= # of moles of a gas

  5. Practice problem • If the pressure exerted by a gas at 25°C in a volume of 0.044L is 3.81atm, how many moles of gas are present? • Calculate the grams of N2 present in a 0.600L sample kept at 1.00atm pressure and a temperature of 22.0°C

  6. Gas Stoichiometry 7. Ammonia (NH3) is synthesized from hydrogen and nitrogen gases If 5.00L of nitrogen reacts completely by this reaction at a constant pressure and temperature of 3.00atm and 298K, how many grams of ammonia are produced?

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