Limiting reactants and percent yield

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Presentation transcript:

Limiting reactants and percent yield

Reactant A Reactant B Product 1.0 g 0.25 g 0.50 g 0. 75 g 1.25 g Looking at our variables, what do you predict will happen to the amount of product produced? Why do you think that?

What is actually Happening? Reactant A Reactant B Product 1.0 g 0.25 g 1.25 g 0.50 g 1.50 g 0. 75 g 1.75 g What is actually Happening?

How many sandwiches can we make with 3 bread, 2 meat, and 2 cheese How many sandwiches can we make with 3 bread, 2 meat, and 2 cheese? What is limiting us from making more?

Limiting reactant - What is it? Controls how much product is produced. The other reactant is considered excess.

4 NH3(g) + 5 O2(g)  4 NO(g) + 6 H2O(g) Using the following chemical equation; if you have 68.2 g of NH3 and 128 g of O2, which item is the limiting reactant? So how many grams of water will be produced? 4 NH3(g) + 5 O2(g)  4 NO(g) + 6 H2O(g)

The amount we calculated is the theoretical yield OR how much is supposed to be produced. The actual yield comes from doing the experiment. What is the percent yield of the previous experiment if 75.0g is actually produced?