Warm Up WRITE DOWN three questions that you still have about limiting reagents or stoichiometry. Today is a review of stoichiometry and limiting reagents.

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Presentation transcript:

Warm Up WRITE DOWN three questions that you still have about limiting reagents or stoichiometry. Today is a review of stoichiometry and limiting reagents because we will have a quiz on these concepts tomorrow You should complete your Limiting Reagent worksheet today, but you do NOT have to turn it in – you should use it to study!!! http://ossfabricators.com/photos/reactor2.jpg

Limiting Reagent: the reagent that is completely used up in a chemical reaction. Excess Reagent: reagent not completely used up in a chemical reaction.

How do you know if there’s a limiting reagent? Situation #1: The problem says it. What to do: Find the limiting reagent. Situation #2: You are given amounts for two reactants, and you need to find how much product is made. Step 1: Find the limiting reagent Step 2: Using the grams of limiting reagent as your starting value, find how much product is made.

Example: Find the limiting reagent when 1. 22g O2 reacts with 1 Example: Find the limiting reagent when 1.22g O2 reacts with 1.05g H2 to produce H2O. There are two solution methods you could use. In both methods, the first step is to convert the mass to moles.

Method 1 Use the moles of one reactant to calculate the necessary moles of the other reactant to fully react. Compare the calculated value with the actual value to see if this reagent is excess or limiting.

Example: Find the limiting reagent when 1. 22g O2 reacts with 1 Example: Find the limiting reagent when 1.22g O2 reacts with 1.05g H2 to produce H2O. Answers using method 1: Convert mass to moles: 0.038 mol O2, 0.5 mol H2 Calculate H2 moles necessary to react with O2: 0.076 mol H2. Compare 0.076 mol H2 to actual mol of H2 (0.5mol H2), Since 0.5 mol H2 is more than 0.076 mol H2, H2 is the excess reagent and O2 is the limiting reagent.

Method 2 Use the moles of each of the reactant to calculate one of the products. The reagent that gave the smaller calculated value of product is the limiting reagent. The actual value of the amount of product is the smaller of the calculated values.

Example: Find the limiting reagent when 1. 22g O2 reacts with 1 Example: Find the limiting reagent when 1.22g O2 reacts with 1.05g H2 to produce H2O. Answers using Method 2: Convert mass to moles: 0.038 mol O2, 0.5 mol H2 Calculate H2O moles produced by using each of the reactants: Using O2: 0.076 mol H2O. Using H2: 0.5 mol H2O. The actual amount H2O produced is the smaller one of the two values(0.076mol H2O). O2 is the limiting reagent, since O2 was used in the calculation of the 0.076mol H2O.