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Chem 1010 Chp 5 Test Review

Total questions: 72

Worksheet time: 18hrs 32mins

Name
Class
Date
1.
P4 + 3O2 --> 2P2O3
a)
Synthesis 
b)
Decomposition
c)
Single displacement
d)
Combustion
2.
Which chemical reaction switches 2 elements?
a)
Double Replacement
b)
Single Replacement
c)
Combustion
d)
Decomposition
3.
A + B = AB
a)
Double Replacement
b)
Synthesis
c)
Combustion
d)
Decomposition
4.
AB + CD = AD + CB
a)
Double Replacement
b)
Single Replacement
c)
Combustion
d)
Decomposition
5.
A + BC = B + AC
a)
Single Replacement
b)
Combustion
c)
Double Replacement
d)
Synthesis
6.
Which chemical reaction takes place when 2 substances react to form a single product?
a)
Decomposition
b)
Double Replacement
c)
Single Replacement
d)
Synthesis
7.
AB = A + B
a)
Decomposition
b)
Single Replacement
c)
Combustion
d)
Synthesis
8.
Fe + H2SO4 --> Fe2(SO4)3 + H2
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Combustion
9.

In the following equation, what are the REACTANTS?

2C3H6+ 9O2 ---> 6CO2 + 6H2O

propane +oxygen ---> carbon dioxide and water

a)

propane and oxygen

b)

carbon dioxide and water

10.

If the total mass of the reactants measures 125 g, what would be the total mass of the products?

a)

125 g

b)

150 g

c)

62.5 g

11.
In a chemical equation, is it true that -
a)
the reactant side and product side can have different numbers of atoms for each element
b)
there can be different elements on the reactant side and the product side
c)
an element or compound must be accompanied by a phase change
d)
the coefficients indicate the number of molecules of each reactant used and the number of molecules of each product made
12.
Is this equation balanced?
a)
yes
b)
no
c)
Not enough information
13.
Predict the products for the this reaction:
K + HCl --> 
a)
KCl + H2
b)
KHCl 
c)
KH + Cl2
d)
KCl + H
14.
Predict the products for the this reaction:
Mg + CuCl2 --> 
a)
MgCl2 + Cu
b)
MgCl + Cu
c)
MgCu + Cl2
d)
CuMg + Cl2
15.
In the reaction of K + AgNO3 what will the products be?
a)
K and AgNO3
b)
Ag and KNO3
c)
NO3 and AgK
d)
No reaction
16.
The symbol for a substance dissolved in water is
a)
(s)
b)
(l)
c)
(g)
d)
(aq)
17.
If an element is diatomic it should have a subscript of___
a)
2, always
b)
2, only when it is by itself
c)
it shouldn't have a subscript, it should have a coefficent
18.
Which of the following equations represents the balanced synthesis reaction of iron (III) and oxygen?
a)
Fe + 3 O2 → Fe2O3
b)
3 Fe + 3 O2 → 2 Fe2O3
c)
2 Fe + O2 → Fe2O3
d)
4 Fe + 3 O2 → 2 Fe2O3
19.
What are the correct formulas and coefficients for the products of the following single-replacement reaction?
Mg + Al(OH)3 →
a)
No Reaction
b)
Al + Mg(OH)3
c)
2 Al + 3 Mg(OH)2
d)
3 Al + MgOH3
20.
What coefficients are needed to correctly balance the equation?
_Bi   +   _O2   →  _Bi2O3
a)
3,2,3
b)
2,3,2
c)
4,3,2
d)
none of these
21.
What must go in the blank space to balance the equation?
4Fe  +  _O2  → 2Fe2O3
a)
1
b)
2
c)
3
d)
4
22.
The Law of Conservation of Mass states
a)
that matter exists in all states and reacts the same
b)
that matter can only be changed into new substances by introducing a catalyst
c)
that matter exists in the same state throughout any chemical change
d)
that matter cannot be created or destroyed and that the mass of the products must equal the mass of the reactants
23.
How many O's are in Al₂(SO₄)₃
a)
4
b)
12
c)
7
d)
24
24.

Which of these will result in the formation of water?

a)

acid + base

b)

acid + metal

c)

acid + salt

d)

acid + nonmetal

25.
Exothermic reactions...
a)
Absorb energy
b)
Release energy
c)
Release Color
d)
Absorb Color
26.
In an endothermic reaction, heat is ,,,
a)
taken in
b)
given out
27.
Is the melting of ice an exothermic or endothermic process?
a)
Exothermic
b)
Endothermic
28.
What kind of reaction is shown in the picture
a)
Endothermic
b)
Exothermic
c)
Explosive
d)
Boring
29.
The energy needed to start a chemical reaction is the _____________________.
a)
Activation Energy
b)
Products
c)
Reactants
d)
Enzymes
30.
What is a substance that is dissolved in another substance? 
a)
solution
b)
solute
c)
solvent
d)
compound
31.
What is a solvent?
a)
The substance that does the dissolving in a solution.
b)
The substance that is being dissolved in a solution.
c)
The mixing of different substances.
d)
The process in which neutral molecules lose or gain electrons
32.
A solution that is considered dilute would be....
a)
Dark in color
b)
Have a strong scent
c)
Have a large amount of solute
d)
Have a small amount of solute
33.
Kool-Aid - Powder, sugar, and water
Identify the solvent 
a)
water
b)
powder
c)
sugar
d)
powder and sugar
34.

What is the molarity of 0.798 mol NaCl in 2.02 L solution?

a)

1.61 M

b)

0.395 M

c)

2,53 M

35.

Calculate the molarity of 1.00 g NaCl dissolved in 100 mL solution

a)

0.171 M

b)

5.85 M

c)

0.01 M

36.

Calculate the moles of HCl present in 330 mL of 0.70 M solution

a)

337 moles

b)

0.231 moles

c)

47.1 moles

d)

0.000231 moles

37.
What is the molarity of a solution which contains 22.41 grams of NaCl in 50.0 mL of solution?  MM = 58.44 g/mol 
a)
0.488 M
b)
7.66 M
c)
7.67 M
d)
0.00767 M
38.
If a compound is aqueous, it means that 
a)
the solute is water 
b)
the solvent is water 
c)
the solution is wet 
d)
the solvent is polar
39.
A 3.5 M KNO3 solution contains 3.5 moles of KNO3 dissolved in
a)
1.0 liter of solution 
b)
1.0 milliliter of solvent 
c)
3.5 liter of solvent 
d)
3.5 milliliter of solution
40.
The most commonly used form of concentration in chemistry is
a)
molarity
b)
molality
c)
percent by volume
d)
percent by mass
41.
Define chemical equilibrium.
a)
A reaction is reversible.
b)
The concentration of the reactants is equal to the concentration of the products.
c)
The rate of a forward reaction is equal to the rate of the reverse reaction.
d)
The reaction stops and no further change in concentration occurs.
42.
What are the units for molar mass?
a)
grams
b)
amu
c)
grams/mole
d)
liters
43.

What is the molar mass of Ca(OH)2

a)

74.094 g/mol

b)

210.0g/mol

c)

98.9g/mol

d)

219.9g/mol

44.
The number 6.02 x 1023 is called...
a)
Obama's number
b)
Bohr's number
c)
Trump's number
d)
Avogadro's number
45.

What is the percent composition by mass of sulfur (S) in the compound MgSO4?

a)

20.22%

b)

19.85%

c)

26.64%

d)

28.64%

46.

At STP, the volume of 1 mole of H2 gas is

a)

14.0 L

b)

22.4 L

c)

40.0 L

d)

1.0 L

47.

Calculate the mass in grams of 7.57 mol of BaSO4

a)

1798.23 g BaSO4

b)

233.3 g BaSO4

c)

1766.08 g BaSO4

d)

389.68 g BaSO4

48.
How many moles are there in 12.7g of CaF2?
a)
0.20 mol
b)
1,000.76 mol
c)
6.14 mol
d)
0.16 mol
49.

What mass in grams of solute is needed to prepare 0.250 L of 0.287 M K2Cr2O7?

a)

21.1 g K2Cr2O7

b)

32.5 g K2Cr2O7

c)

.250 g K2Cr2O7

d)

2.81 g K2Cr2O7

50.
Classify
CH4 + O2 → CO2 + H2O 
a)
single replacement
b)
double replacement
c)
synthesis
d)
combustion
51.
CH4 + 2 O2 → CO2 + 2 H2O
How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?
a)
13.7 mol
b)
2.75 mol
c)
6.11 mol
d)
6.85 mol
52.

What volume in Liters of CO2 is formed when 3.7 L of C6H14 is burned.

2 C6H14 (g) + 19 O2 (g) --------- 12 CO2 (g) + 14 H20 (g)

a)

.38 L CO2

b)

22.2 L CO2

c)

5.4 L CO2

d)

12 L CO2

53.
When solute dissolves into a solvent it is called a _____________.
a)
mixture
b)
solution
c)
element
54.
The image shown is an example of a ___________.
a)
solution
b)
mixture
c)
gas
d)
plasma
55.

M (molarity) is a unit of

a)

temperature

b)

concentration

c)

volume

d)

pressure

56.

The ability to dissolve in water.

a)

Insoluble

b)

Soluble

c)

Dilute

d)

Concentrated

57.

Unable to dissolve in water.

a)

Molarity

b)

Concentrated

c)

Diluted

d)

Insoluble

58.

A solution that has large amount of solute and a small amount of solvent is considered...

a)

Diluted

b)

Soluble

c)

Concentrated

d)

Insoluble

59.

Solutions in which water is the solvent are called....

a)

Concentrated

b)

Diluted

c)

Aqueous

d)

Heterogenous

60.
Magnesium can be burned in air to produce solid magnesium oxide.
a)
2Mg(s) + O2(g)→ 2MgO(s)
b)
Mg(s) + O(g) → MgO(s)
c)
2Mg(s) + CO2(g) → 2MgO(s) + C(s)
d)
2Mg(s) + O2(g) → Mg2O2(s)
61.
Write a complete balanced reaction for the following.
Calcium metal reacts with oxygen gas to form a solid
a)
2 Ca (s) + O2 (g) --> 2 CaO (s)
b)
2 Ca (s) + 2 O (g) --> 2 CaO (s)
c)
Ca (s) + O2 (g) --> 2 CaO (s)
d)
Ca (s) + O2 (g) -->  CaO2 (s)
62.

An amount of substance the contains the same number of units as there are atoms.

a)

Mole

b)

Molar Mass

c)

Products

d)

Reactants

63.

The quantitative relationship between reactants and products in a chemical reaction.

a)

Molar Mass

b)

Law of conservation of mass

c)

Stoichiometry

d)

Molarity

64.

Uses symbols and formulas to represent elements in a chemical change.

a)

Chemical notation

b)

Chemical formula

c)

Chemical change

d)

Chemical equation

65.

Elements or compounds found to the right of the arrow in a chemical equation.

a)

Reactants

b)

Products

c)

Catalyst

d)

Coefficent

66.

According to the energy diagram shown above, the chemical reaction in the forward direction is

a)

exothermic because it absorbs energy

b)

exothermic because it releases energy

c)

endothermic because it absorbs energy

d)

endothermic because it releases energy

67.

What is the percent by volume concentration of 78.9 ml of acetone in 1550 ml of an acetone-water solution?

a)

5.6 %

b)

4.8 %

c)

2.4 %

d)

3.7 %

68.
How would this reaction be classified?
2Na + Cl2 → 2NaCl + 25kJ energy
a)
Exothermic
b)
Endothermic
c)
Isothermic
d)
None of the above
69.
What is true of the reaction described below?
Br2 + Cl2 + 30.0 J of energy  → 2BrCl
a)
It is exothermic because energy was released.
b)
It is endothermic because energy is absorbed.
c)
It is exothermic because energy is absorbed.
d)
It is endothermic because energy is released.
70.

Which of these diagram correctly represent an endothermic reaction?

a)
b)
c)
d)
71.
What mass of P4 must be reacted to produce 5905 kJ of energy?
P4 + 6Cl2 --> 4PCl3 + 2439 kJ
a)
25.43 g
b)
563.0 g
c)
2.421 g
d)
300.0 g
72.

ΔH stands for?

a)

A phase change

b)

A change in energy

c)

A change in moles

d)

A change in mass

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