Lecture%205%20part%20II%20Chem%20102

Lecture%205%20part%20II%20Chem%20102 - Chapter 5 Gas part...

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Chapter 5 Gas part II
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Gas Stoichiometry Example 1. What is the volume at STP of 4.00 g of CH 4 ? Example 2. How many L of O 2 are needed to react 28.0 g NH 3 at 24°C and 0.950 atm? 4 NH 3 (g) + 5 O 2 (g) 4 NO(g) + 6 H 2 O(g)
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Ideal Gas Law Problems Consider the decomposition of Calcium carbonate. 1:1 mole ratio so you produce 0.3 mol CaO CaCO 3 (s) Î CaO(s) + CO 2 (g) This reaction produces 0.3 mol CO 2 how much CaO is produced? PV = nRT, g CaO = 52g/n (0.0304n) => 0.0304 mol CaO If the reaction produced 732 mL of CO 2 at 21°C and 77.1 cm Hg, how much CaO is produced? 1:1 n ratio want g CaO! n = PV/RT = 1.015 atm(0.732L)/(0.0832 L atm/mol K)(294) = 0.0304 mol = 1.58 g
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Molar Mass Determination Example 3. What is the molar mass of a gas if 0.250 g of the gas occupy 215 mL at 0.813 atm and 30.0°C? 4
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Dalton’s Law of Partial Pressures For a mixture of gases in a container, P Total = P 1 + P 2 + P 3 + . . . The total pressure exerted is the sum of the pressures that each gas would exert if it were alone. P 1 , P 2 , P 3 – partial pressure of individual gas Each gas behaves as ideal gas V RT n V RT n n P V RT n P V RT n P total total = + = = = ) ( ,.... , 2 1 2 2 1 1 Note: temperature and volume are the same
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Example 4. 27.4 L of oxygen gas at 25.0°C and 1.30 atm, and 8.50 L of helium gas at 25.0°C and 2.00 atm were pumped into a tank with a volume of 5.81 L at 25°C. Calculate the new partial pressure of
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Lecture%205%20part%20II%20Chem%20102 - Chapter 5 Gas part...

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