Tuesday, January 12th
• Consider the synthesis of water as shown in Model
3. A container is filled with 10.0 g of H2 and 5.0 g of
O2.
Which reactant is the limiting reactant? Show your
work (note that your starting quantities are in MASS
not MOLES!)
b. What mass of water can be produced? Show your work
c. Which reactant is present in excess, and what mass of
that reactant remains after the reaction is complete?
Show your work.
a.
Steps
1. Set up and balance your equation
2. For each reactant:
Calculate the moles of product you can produce
a.
•
Moles of A to moles of B
•
Or
Grams of A to moles of A to moles B
b. If the question requires it, go all the way to grams of
product (read carefully! What are you being asked to
find?)
3. Whichever number is smaller will be your
limiting reactant.
Practice
• Aluminum metal and hydrogen chloride react.
• What kind of reaction is this?
• Write the balanced equation
• If you have 57.1 grams of aluminum metal and 72.6 grams of
hydrogen chloride, what is the limiting reactant?
Practice
• Aluminum bromide and sodium hydroxide react.
• What kind of reaction is this?
• Write the balanced reaction
• If you have 200.0 grams of aluminum bromide and 89.2 grams of
sodium hydroxide, how many grams of aluminum hydroxide will
form?
Practice
• Iron and water react to form hydrogen gas and iron (III)
oxide.
• Write the balanced reaction
• If you have 79.6 grams of iron and 30.4 grams of water, what is the
limiting reagent?
Homework
• Limiting Reactant Practice
• Add this to your pink sheet!
• Tomorrow
• Limiting Reactant Lab: Aluminum and Copper (II) Chloride
• More limiting Reactant Practice
• Thursday
• Lab Analysis
• Start Iron nail lab
• Friday
• Finish iron nail lab
• Quiz: limiting reactants
• Hand out test review
• Today is the last day to retake the Math and Moles test.