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Stoichiometry Review - Lvl

Total questions: 34

Worksheet time: 4hrs 38mins

Name
Class
Date
1.
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
2.
KNO3 --> KNO2 + O2
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?
a)
1
b)
2
c)
3
d)
4
4.
WO3 + H2 --> W + H2O
What coefficient goes in front of H2?
a)
1
b)
2
c)
3
d)
4
5.
True or False. You must convert grams to moles to do stoichiometry.
a)
True
b)
False
6.
2H2   +   O2  →  2H2O
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.
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
8.
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
9.
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
10.
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
11.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of MgO 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)

None

13.
If you predicted that 1.5 moles of Magnessium are used in a reaction, and you have 2.0 moles of Magnessium, what type of reactant is Magnessium?
a)
Limiting Reactant
b)
Excess Reactant
c)
Fast Reacter
d)
Non-Reactant
14.
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
15.
The Formula to make S'mores is:
2C + 1M + G2 → C2MG2. If you have 5 Marshmallows (M), 9 Chocolate Pieces (C), and 9 Graham Cracker Halves (G), how many S'mores can you make?
a)
5
b)
4
c)
8
d)
42
16.
What is the first thing you must do to solve a stoichiometry problem?
a)
Write a Balanced Equation
b)

Identify known and unknown

c)

Setup problem

d)

Solve for answer

17.
 The equation for Percent Yield:
a)

(theoretical/actual) X 100

b)

(actual/theoretical) X 100

c)

(actual - theoretical)/ theoretical X 100

18.
2H2  +   O2  →  2H2O
How many moles of oxygen are consumed if 8 moles H2 are used?
a)
2
b)
4
c)
6
d)
8
19.
If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the
a)
theoretical yield
b)
mole ratio
c)
actual yield
d)
percentage yield
20.
What is the measured amount of a product obtained from a chemical reaction?
a)
mole ratio
b)
theoretical yield
c)
percentage yield
d)
actual yield
21.
Mole ratios are obtained from the
a)
balanced chemical equation
b)
periodic table
c)
molar mass
22.
What is the mole ratio of H2O to H3PO4 in the following chemical equation?   P4O10 + 6 H2O --> 4 H3PO4 
a)
6:4
b)
4:6
c)
1:3
d)
3:1
23.
Identify the limiting reagent when 6.00 moles HCl combines with 5.00 moles Mg to form MgCl2.
 
1 Mg +  2 HCl --> 1 MgCl2  +  1 H2   
 
a)
Mg
b)
H2
c)
MgCl2
d)
HCl
24.

LiOH + KCl → LiCl + KOH 

I actually produced 6 grams of lithium chloride and I began this reaction with 20 grams of lithium hydroxide. What is my percent yield?

a)
16.9%
b)
5.91%
c)
1.88%
d)
12.3%
25.
Calculate the molar mass of Mg(OH)2.
a)
33.2 g/mol
b)
41.3 g/mol
c)
86.9 g/mol
d)
58.3 g/mol
26.
What is the best definition for subscript?
 
a)
The big number that tells you the number of molecules.
b)
The atomic number
c)
The little number that tells the number of atoms for each element.
27.
What is the best definition for coefficient?
 
a)
The big number that tells you the number of molecules.
b)
The little number that tells the number of atoms for each element.
c)
The atomic number
28.

The reaction A + B ⟶ AB is classified as a _____ reaction.

a)

synthesis

b)

decomposition

c)

single replacment

d)

double replacement

29.

What class of reaction best describes the equation below?

2HI ⟶ H2 + I2

a)

synthesis

b)

decomposition

c)

single replacement

d)

double replacement

30.

What class of reaction best describes the equation below?

Zn + H2S ⟶ ZnS + H2

a)

synthesis

b)

combustion

c)

single replacement

d)

double replacement

31.

What class of reaction best describes the equation below?

CH4 + O2 ⟶ CO2 + H2O

a)

single replacement

b)

double replacement

c)

decomposition

d)

combustion

32.

What class of reaction best describes the equation below?

FeS + HCl ⟶ H2S + FeCl2

a)

synthesis

b)

combustion

c)

single replacement

d)

double replacement

33.
2 NaClO3 (s) --> 2NaCl (s) +3 O2 (g)  
12.00 moles of NaClO3 will produce how many grams of O2?
a)
256 g of O2
b)
576 g of O2
c)
288 g O2
34.
B2H6 + 3O2 -->2 HBO2 + 2 H2O
 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

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