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Chapter 12

Chapter 12. Stoichiometry. Stoichiometry. Stoichiometry Calculation of quantities in chem rxns. Mole Ratio --- particles. N 2 (g) + 3H 2 (g) → 2NH 3 (g). 1 molecule of N 2 reacts with 3 molecules H 2 to yield 2 molecules of ammonia (NH 3 ). Ratio is 1:3:2.

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Chapter 12

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  1. Chapter 12 Stoichiometry

  2. Stoichiometry Stoichiometry • Calculation of quantities in chemrxns.

  3. Mole Ratio --- particles N2(g) + 3H2(g)→ 2NH3(g) 1 molecule of N2reacts with 3 molecules H2to yield 2 molecules of ammonia (NH3). Ratio is 1:3:2 1 mole of nitrogen reacts with 3 moles of hydrogen to yield 2 moles of ammonia.

  4. Mole Ratio N2(g) + 3H2(g) → 2NH3(g) mol N2 : mol H 2 = 1:3 mol N2 : mol NH3 = 1:2 mol H2 : mol NH3 =

  5. Volume & Mole N2(g) + 3H2(g) → 2NH3(g) At STP, 22.4 L N2 react with 3 x 22.4 L H2 to form 2 x 22.4 L NH3 • volume applies only for gases • Avogadro Principle • 1 mole of any gas occupies 22.4L at STP.

  6. Mole to Mole • How many moles ammonia are produced when 0.60 mol nitrogen reacts with hydrogen? N2(g) + 3H2(g) → 2NH3(g)

  7. Mass to Mass 2. Calculate the # g ammonia produced by the rxn of 5.4 g hydrogen with an excess of nitrogen. N2 (g) + 3H2(g) → 2NH3 (g)

  8. Mass to Mass 3. Acetylene gas (C2H2) is produced by adding water to calcium dicarbide (CaC2). How many g of acetylene are produced by adding water to 5.00g CaC2? CaC2 (s) +2H2O(l) → C2H2 (g) + Ca(OH)2 (aq)

  9. Mass to # of Particles 4. How many molecules of oxygen are produced when a sample of 29.2 g of water is decomposed by electrolysis? 2H2O (l) electricity 2H2 (g) + O2 (g)

  10. Volume to Mole 5. Assuming STP, how many L of oxygen are needed to produce 19.8 L SO3? 2SO2 (g) + O2 (g) → 2SO3 (g)

  11. Mole & Volume 2CO (g) + O2 (g)→ 2CO2 (g) 6. The eqn for the combustion of carbon monoxide is How many L of oxygen are required to burn 3.86 L of carbon monoxide at STP?

  12. Mg3N2(s) + 6H2O (l) → 2NH3(aq) + 3Mg(OH)2(s) CST example 1 If 54.0 g of water are mixed with excess magnesium nitride, then how many g of ammonia are produced? A 1.00 B 17.0 C 51.0 D 153

  13. Fe2O3 + 3CO → 2Fe + 3CO2 CST problem 2 In this rxn, how many g of Fe2O3 are required to completely react with 84 g of CO? A 64 g B 80 g C 160 g D 1400 g

  14. CST problem 3 A mass of 5.4 g of aluminum (Al) reacts with an excess of copper (II) chloride (CuCl2) in soln, as shown below. What mass of solid copper (Cu) is produced? A 0.65 g B 8.5 g C 13 g D 19 g 3CuCl2 + 2Al → 2AlCl3 + 3Cu

  15. The End

  16. 2. How many g of H2O can be formed from 24.0 g O2 and 6.00 g H2? • 30.0 g • 27.0 g • 54.0 g • 13.5 g

  17. 3. Octane burns according to the following eqn. 2C8H18 + 25O2  16CO2 + 18H2O What is the % yield if 14.6 g of CO2 are produced when 5.00 g of C8H18 are burned? • 106% • 94.8% • 34.2% • 62.5%

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