Chemistry 2013
Ms. Lewis
Name____________________ GN____
Date _________
Total Points Possible: 20 pts.
Stoichiometry Worksheet
Mole to Mole Conversions
(3 pts.)
1. Given the equation:
N2 + 3 H2 ---> 2 NH3
If we have 2.00 mol of N2 reacting with sufficient H2, how many moles of NH3 will be
produced?
Suppose 6.00 mol of H2 reacted with sufficient nitrogen. How many moles of ammonia would be
produced?
We want to produce 2.75 mol of NH3. How many moles of nitrogen would be required?
Grams to Mole Conversions
1. Convert 25.0 grams of KMnO4 to moles. (1 pt.)
2. Calculate how many moles are in 17.0 grams of H2O2 (1 pt.)
3. Calculate the moles present in:
(1 point each)
a. 2.00 grams of H2O
b. 75.57 grams of KBr
c. 100. grams of KClO4
Mole to Grams Conversions
(1 point each)
1. Calculate how many grams are in 0.700 moles of H2O2
2. Convert 2.50 moles of KClO3 to grams.
Grams to Grams Conversions
(2 pts. each)
1. How many grams of chlorine can be liberated from the decomposition of 64.0 g. of AuCl3 by
this reaction:
2 AuCl3 ---> 2 Au + 3 Cl2
2. Calculate the mass of AgCl that can be prepared from 200. g of AlCl3 and sufficient AgNO3,
using this equation: 3 AgNO3 + AlCl3 --> 3 AgCl + Al(NO3)3
Limiting Reagents
(3 pts. each)
1. Consider the reaction:
2Al + 3I2 ------> 2 AlI3
Determine the limiting reagent and the theoretical yield of the product if one starts with:
a) 1.20 mol Al and 2.40 mol iodine.
b) 1.20 g Al and 2.40 g iodine
c) How many grams of Al are left over in part b?
2. 15.00 g aluminum sulfide and 10.00 g water react until the limiting reagent is used up. Here is
the balanced equation for the reaction:
Al2S3 + 6 H2O ---> 2Al(OH)3 + 3 H2S
(A) Which is the limiting reagent?
(B) What is the maximum mass of H2S which can be formed from these reagents?
(C) How much excess reagent remains after the reaction is complete?