WorksheetsStoichiometry
Total questions: 25
Worksheet time: 1hrs 3mins
Name
Class
Date
1.
What is the first thing you must do to solve a stoichiometry problem?
a)
Write a Balanced Equation
b)
Panic
c)
Write an Unbalanced Equation
d)
Ask for help
2.
KNO3 --> KNO2 + O2
What coefficients are needed to balance the reaction?
What coefficients are needed to balance the reaction?
a)
2, 2, 1
b)
2, 3, 2
c)
1, 2, 2
d)
1, 3, 1
3.
O2 + CS2 --> CO2 + SO2
What coefficient would go in front of the O2?
What coefficient would go in front of the O2?
a)
1
b)
2
c)
3
d)
4
4.
WO3 + H2 --> W + H2O
What coefficient goes in front of H2?
What coefficient goes in front of H2?
a)
1
b)
2
c)
3
d)
4
5.
WO3 + H2 --> W + H2O
What coefficient goes in front of H2?
What coefficient goes in front of H2?
a)
1
b)
2
c)
3
d)
4
6.
2H2 + O2 → 2H2O
How many moles of water can be produced if 8 moles H2 are used?
How many moles of water can be produced if 8 moles H2 are used?
a)
4 moles
b)
8 moles
c)
16 moles
d)
2 moles
7.
2H2 + O2 → 2H2O
How many moles of oxygen are consumed if 8 moles H2 are used?
How many moles of oxygen are consumed if 8 moles H2 are used?
a)
2
b)
4
c)
6
d)
8
8.
What is a Limiting Reagent?
a)
speeds up a reaction
b)
what you run out of first
c)
what you have left over
d)
slows down a reaction
9.
What is a Excess Reagent?
a)
amount you end with
b)
what you run out of first
c)
what you have left over
d)
what you start with
10.
You need 2 pieces of bread, 1 tablespoon of peanut butter and 2 tablespoons of jelly to make a sandwich. If you have 10 pieces of bread, 4 tablespoons of peanut butter and 20 tablespoons of jelly, what is the limiting reactant?
a)
bread
b)
jelly
c)
peanut butter
d)
sandwich
11.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of Mg to moles Fe?
a)
3mol Mg / 2 mol Fe
b)
2 mol Mg/ 3 mol Fe
c)
1 mol Fe/ 2 mol Fe
d)
3 mol MgO / 2 mol Fe
12.
Use the equation 2 Al + 3 Cl2 ---> 2 AlCl3. If 2 moles of aluminum and 2 moles of chlorine are reacted, identify the limiting reactant.
a)
AlCl3
b)
Cl2
c)
Al
d)
Gary Busey
13.
Carbon and Oxygen combine to form CO2. If 10g of Carbon combines with Oxygen to produce 20g of CO2 and 10g of Oxygen combines with Carbon to produce 15g of CO2, How many grams of CO2 are produced from 10g of Carbon and 10g of Oxygen?
a)
20g of CO2
b)
15g of CO2
c)
17.5g of CO2
d)
25g of CO2
14.
When does a chemical reaction stop?
a)
When the lab is finished
b)
When the excess reactant is used up
c)
When the limiting reactant is used up
d)
Chemical reactions never stop
15.
How many moles are in 19.82 g Mg?
a)
1.226mol Mg
b)
481.7mol Mg
c)
1.000mol Mg
d)
0.82 mol Mg
16.
2CO + O2 −-> 2CO2
How many liters of carbon dioxide are produced from 10L of carbon monoxide?
How many liters of carbon dioxide are produced from 10L of carbon monoxide?
a)
10
b)
20
c)
1
d)
5
17.
2Al + 6HCl --> 2AlCl3 + 3H2
Aluminium reacts with hydrochloric acid. How many grams of aluminum are necessary to produce 11 L of hydrogen gas at STP?
a)
13
b)
8.8
c)
0.99
d)
1.0
18.
How many particles are in a mole?
a)
602
b)
602 million
c)
602 moles
d)
6.02 x 1023
19.
1 mole of any gas at STP has a volume of ______________________.
a)
22.4 liters
b)
44.2 liters
c)
6.02 x 1023 liters
d)
2.4 liters
20.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron (Fe) can be made from 6 moles H2?
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron (Fe) can be made from 6 moles H2?
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
21.
Balance this reaction: ____ RbNO3 + ____ BeF2 ----> ____ Be(NO3)2 + ____ RbF
a)
1,1,1,1
b)
1,2,1,1
c)
2,1,1,2
d)
2,1,2,1
22.
How many liters of N2, at STP, will react with 53.0 g H2 to form ammonia?
N2 + 3H2 --> 2NH3
a)
396 L
b)
17.6 L
c)
196 L
d)
588 L
23.
How many liters of SO2 will be produced from 55.0 L of O2 at STP?
2H2S + 3O2 --> 2SO2 + 2H2O
a)
55.0 Liters
b)
36.7 Liters
c)
18398 Liters
d)
2.45 Liters
24.
In a chemical reaction, the mass of reactants ___.
a)
is less than the mass of products
b)
is greater than the mass of products
c)
has no relationship to the mass of products
d)
is equal to the mass of products
25.
B2H6 + 3O2 -->2 HBO2 + 2 H2O
What mass of O2 will be needed to burn 36.1 g of B2H6?
What mass of O2 will be needed to burn 36.1 g of B2H6?
a)
13.8 g O2
b)
3.86 mol of O2
c)
124 g O2
100 %
