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Review (Chemistry)

Total questions: 20

Worksheet time: 1hrs 1mins

Name
Class
Date
1.

When balancing this equation, Fe + Cl2 → FeCl3, the correct coefficient for Cl2?

a)

1

b)

2

c)

3

d)

4

2.

Chemical reactions

a)

create and destoy atoms

b)

only occurs outside living organisms

c)

occurs only in living organisms

d)

produce new substances

3.

What does this symbol Δ above the arrow mean?

a)

a precipitate is form

b)

heat is supplied

c)

a calalyst is needed

d)

electricity is needed

4.

Balance the following equation: Cr(s) + Fe(NO3)2 (ag) → Fe(s) + Cr(NO3)3 (ag)

a)

2,3,3,2

b)

2,3,2,3

c)

4,6,6,2

d)

1,3,3,1

5.

Chemical equations

a)

give directions for naming compounds

b)

describe only biological changes

c)

describe chemical reactions

d)

show how to write formulas

6.
Which side of a chemical equation is the product side?
a)
Left (before the yields sign)
b)
Right (after the yields sign)
7.
What is a coefficient?
a)
The small number on the right of the chemical symbol.
b)
The large number to the left of a formula.
8.
At the end of chemical reactions, what is the total mass of the reactants compared to the total mass of the products?
a)
the product is doubled
b)
the product is half the mass of the reactants
c)
the mass is the same
d)
the mass changes depending on the reaction
9.
Name the part in red:

H2 + O2 -> H2O
a)
Coefficient
b)
Product
c)
Yield
d)
Subscript
10.

To balance a chemical equation, it may be necessary to adjust the

a)

formulas of the products

b)

subscripts

c)

coefficients

d)

number of products

11.
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
12.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
13.
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
14.
A chemist interested in the efficiency of a chemical reaction would calculate the
a)
mole ratio
b)
rate of reaction
c)
percent yield
d)
energy released
15.
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
16.
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
17.
Mole ratios are obtained from the
a)
balanced chemical equation
b)
periodic table
c)
molar mass
18.
What is the limiting reactant if 10 moles of NH3  react  with 30.0 moles of NO?
4NH3+6NO --> 5N2 + 6H2O
a)
NH3
b)
NO
c)
N2
d)
water
19.
4NH3 + 5O2 --> 4NO + 6H2O
How much excess reactant is leftover after if 6.30g of ammonia react with 1.80g of oxygen? 
a)
9.75 g NH3
b)
4.80 g O2
c)
0.765 g NH3
d)
5.54 g NH3
20.

Compute for the molar mass of FeSO4. Round off your answer to 3 significant figures.

(a)  

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