Lecture 13 9-21-11 - 1 Today’s Lecture Chapter 4 Material...

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Unformatted text preview: 1 Today’s Lecture Chapter 4: Material Balances involving chemical reactions Exam #1(Closed Book) Wednesday, September 21, 2011 7:00 - 9:00 p.m. PHSC Room 108 Reaction Terminology Stoichiometric proportions Limiting and excess reactant Conversion Extent of reaction Yield Selectivity Chemical Equilibrium (reversible and irreversible reactions) used for multiple reactions Stoichiometry Objectives: 1. Write and balance chemical reaction equations 2. Calculate the stoichiometric quantities of reactants and products given the chemical reaction. 3. Define excess reactant, limiting reactant, conversion, degree of completion. 4. Know the products of common reactions given the reactants Example: A 2.0 g sample of ammonia is mixed with 4.00 g of oxygen. Which is the limiting reactant and what is the percent excess of the excess reactant? NH 3(g) + O 2(g) → NO (g) + H 2 O (g) MW NH 3 = 17 MW O 2 = 32 MW NO =30 MW H 2 O =18 4NH 3(g) + 5O 2(g) → 4NO (g) + 6H 2 O (g) 3 3 3 3 3 NH mol 118 . NH g 17 NH mol 1 NH g 2.0 NH of moles = = 2 2 2 2 2 O mol 125 . O g 32 O mol 1 O g 4.0 O of moles = = : NH O 3 2 Ratio in feed Ratio in chemical equation 25 . 1 4 5 = 06 . 1 0.118 0.125 = 2 3 2 3 2 O mol 1475 . NH mol 4 O mol 5 NH mol 118 . O of moles = = needed oxygen is limiting Example: A 2.0 g sample of ammonia is mixed with 4.00 g of oxygen. Which is the limiting reactant and what is the percent excess of the excess reactant? 2 %) 100 ( reagent limiting the react with to required moles excess in moles excess % = 3 3 3 3 3 NH mol 118 ....
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This note was uploaded on 09/26/2011 for the course CH E 2033 taught by Professor Staff during the Fall '11 term at The University of Oklahoma.

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Lecture 13 9-21-11 - 1 Today’s Lecture Chapter 4 Material...

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