F05L14_6 - aside. Lets have a more dramatic look at...

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1 aside. Let’s have a more dramatic look at limiting reagents: 1. A balloon is filled with 0.06 mol O 2 and 0.02 mol H 2 then ignited. Given the following reaction: What is the “limiting reagent”? How many moles of water are produced? 2 H 2 (g) + O 2 (g) 2 H 2 O (g) 0.06 mol O 2 X 2 mol H 2 O 1 mol O 2 = 0.12 mol H 2 O 0.02 mol H 2 X 2 mol H 2 O 2 mol H 2 = 0.02 mol H 2 O E. Yields 1. Theoretical Yields – the quantity of product that is calculated to form when all of the limiting reagent reacts 2. Experimental Yields or Actual Yields – the quantity of product that is actually obtained – usually less than theoretical yield – never greater 3. Percent Yield – compares the actual yield to the theoretical yield Percent yield = actual yield theoretical yield X 100% 4. Percent Error – compares the experimental value (exper) to the actual (literature or theoretical) (lit) value - note the difference in the way the term actually is used!! 5. Percent Difference – compares two values, neither of which is considered to be more correct than the other Percent Error = exper value - lit value literature value X 100% Percent Difference
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This note was uploaded on 03/12/2010 for the course CHEM 140 taught by Professor Ferrence during the Fall '08 term at Illinois State.

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F05L14_6 - aside. Lets have a more dramatic look at...

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