Download Stoichiometry Guided Notes

Stoichiometry Guided Notes
Name__________________________________
Stoichiometry
study of the ____________ relationships in a ____________ ____________
based on ________________ equations
The ___________ in a ___________ ___________ give the ___________ ___________ for the ___________
involved in the ___________.
Mole to Mole Conversions:
1. When elemental aluminum reacts with elemental iodine, aluminum iodide is produced.
mole ratios:
_____ mol Al =_____ mol I2
_____ mol Al =_____ mol AlI3
_____ mol I2 =_____ mol AlI3
If you start with 4 moles of Al, how many moles of AlI 3 will be produced?
2. Dinitrogen tetrahydride reacts with Dinitrogen tetroxide to produce nitrogen gas and water.
? moles N2O4 = 2.72 moles N2H4
? moles N2 = 2.72 moles N2H4
Mass to Mole Conversions:
1. How many moles of water will be produced when 8.0 grams of hydrogen gas react with the oxygen in the air?
(Hint: To “make the switch” between different substances in a reaction, use the ________ ratio from the
______________ equation.)
2.
In photosynthesis, carbon dioxide and water react to form glucose, C6H12O6 and oxygen gas.
___CO2 + ___H2O  ___ C6H12O6 + ___O2
If 15.6 grams of carbon dioxide react, how many moles of glucose will be produced?
How many grams of carbon dioxide must react to produce 0.25 moles of glucose?
Mass to Mass Conversions:
1. When nitrogen and hydrogen react, they form ammonia gas, which has the formula NH3. If 56.0 g of nitrogen are
used up in the reaction, how many grams of ammonia will be produced?
2. Sodium metal reacts with oxygen to produce solid sodium oxide. How many grams of sodium must react to
produce 42.0 g of sodium oxide?
3. When 12.0 g of hydrogen reacts with oxygen, how many grams of water are produced?
% Yield:
Actual Yield: amount of __________ produced when the __________ is performed in a __________
Theoretical Yield: amount of __________ expected to be __________ based on the _________ _________ and the
amount of __________
Percent Yield = (__________ yield / __________ yield) x 100%
1. What is the % yield of carbon dioxide when __________ grams of propane are burned and __________ grams of
carbon dioxide are collected?
C3H8 + O2  CO2 + H2O
Limiting Reactant
____________ used up _________ in a _____________ reaction.
Excess Reactant
____________ that is not used up in a chemical ____________
1. When FeCl3 reacts with O2, Fe2O3 and Cl2 are produced. If 4.0 moles of FeCl3 and 4.0 moles of O2 are mixed,
how many grams of Fe2O3 will be produced? (Hint: Work two separate problems, using one reactant at a time.)
(Hint: Answer will be the smaller amount of product.)
What is the limiting reactant?
What is the excess reactant?
2. Iron (III) oxide reacts with carbon monoxide to form molten iron and carbon dioxide. If 0.18 g of iron (III) oxide
reacts with 0.11 g of carbon monoxide, how many grams of iron would be produced?
Fe2O3 + CO  Fe + CO2
What is the limiting reactant?
What is the excess reactant?
Molar Volume
Samples of ____________ ____________ at the same____________ and ____________ contain the ____________
number of____________, then the ____________ of all the ____________ must be____________.
• At ____________, one ____________ of any gas occupies a ____________of ____________.
• ____________ is the ____________ ____________ of a gas.
1. 3.2 moles of KNO3 are heated, producing O2 and KNO2. Calculate the volume of O2 in liters that could be
obtained at STP.
2. In the following equation, what volume of hydrogen will produce 0.25 mole of NH3 at standard conditions of
temperature and pressure?
N2(g) + 3 H2(g)  2 NH3(g)
3. When magnesium burns in the presence of oxygen, magnesium oxide is formed. How many moles of
magnesium were burned if at STP, the magnesium was ignited in a 0.50 L container of oxygen gas?