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Semester 2 Final Review Chem

Total questions: 186

Worksheet time: 5hrs 41mins

Name
Class
Date
1.

Which compound's strongest IMF is London Dispersion Forces (LDF)?

a)

A

b)

B

c)

C

d)

None

2.

Which compound's strongest IMF is Dipole-Dipole (DD)?

a)

A

b)

B

c)

C

d)

None

3.

Which compound's strongest IMF is Hydrogen Bonding (HB)?

a)

A

b)

B

c)

C

d)

None

4.

Which compound would have the highest boiling point?

a)

A

b)

B

c)

C

d)

None

5.

Which compound would have the lowest viscosity?

a)

A

b)

B

c)

C

d)

None

6.

Which compound would evaporate the fastest?

a)

A

b)

B

c)

C

d)

None

7.

Identify the states of matter of each picture- in the order shown.

a)

Liquid, Solid, Gas

b)

Gas, Solid Liquid

c)

Liquid, Gas Solid

d)

Solid, Liquid, Gas

8.

Which beaker has the strongest IMFs?

a)

A

b)

B

c)

C

d)

All the same.

9.

Which beaker has the highest kinetic energy?

a)

A

b)

B

c)

C

d)

All the same.

10.

Which beaker has particles that take the shape and volume of their container? (no definite shape or volume)

a)

A

b)

B

c)

C

d)

All the same.

11.

Which beaker has particles that move enough to allow the substance to flow?

a)

A

b)

B

c)

C

d)

All the same.

12.

If picture 3 was cooled to the point of changing its phase, which picture represents the new state of matter?

a)

A

b)

B

c)

C

d)

All the same.

13.

Which picture shows particles with a definite shape and volume?

a)

A

b)

B

c)

C

d)

All the same.

14.

Which picture shows particles with no definite shape and but a definite volume? (takes the shape of its container but not the volume)

a)

A

b)

B

c)

C

d)

All the same.

15.

What state of matter is present in area 1?

a)

Solid

b)

Liquid

c)

Gas

d)

Triple Point

16.

What state of matter is present in area 2?

a)

Solid

b)

Liquid

c)

Gas

d)

Triple Point

17.

What state of matter is present in area 3?

a)

Solid

b)

Liquid

c)

Gas

d)

Triple Point

18.

What is the boiling point of the substance at 100kPa?

a)

120oc

b)

65oc

c)

87oc

d)

80oc

19.

What is the triple point?

a)

Where all three states of matter exist at the same time.

b)

Where the substance is a gas.

c)

The triple point is where a substance exists in two different phases simultaneously.

d)

It's the point where the substance can transition directly from solid to gas without passing through the liquid phase.

20.

At what pressure will sublimation occur at 30oc?

a)

40 kPa

b)

15 kPa

c)

30 kPa

d)

Will not occur.

21.

At 110 kPa and 20oc, what is the state of matter?

a)

Solid

b)

Liquid

c)

Gas

d)

Triple Point

22.

At what sections is the temperature increasing? Select all that apply.

a)

I

b)

II

c)

III

d)

IV

e)

V

23.

At what sections is a phase change occuring? Select all that apply.

a)

I

b)

II

c)

III

d)

IV

e)

V

24.

What state of matter is occurring at 70oc?

a)

Solid

b)

Liquid

c)

Gas

d)

Boiling

e)

Melting

25.

What is occurring at 100oc?

a)

Solid

b)

Liquid

c)

Gas

d)

Boiling

e)

Melting

26.

What would the change in temperature be for a liquid at 55oc that has heated up and reached the boiling point.

a)

55oc

b)

45oc

c)

100oc

d)

155oc

27.

Which substance would take the longest to heat up?

a)

Silver

b)

Iron

c)

Aluminum

d)

Water

28.

Which substance would take the longest to cool down?

a)

Silver

b)

Iron

c)

Aluminum

d)

Water

29.

Which substance would be the fastest to heat up?

a)

Silver

b)

Iron

c)

Aluminum

d)

Water

30.

Which beaker is evaporating the fastest?

a)

Beaker I

b)

Beaker II

c)

Beaker III

d)

Beaker IV

31.

Which beaker is evaporating the slowest?

a)

Beaker I

b)

Beaker II

c)

Beaker III

d)

Beaker IV

32.

Which beaker contains a substance with the strongest IMFs?

a)

Beaker I

b)

Beaker II

c)

Beaker III

d)

Beaker IV

33.

Which beaker contains a substance with the weakest IMFs?

a)

Beaker I

b)

Beaker II

c)

Beaker III

d)

Beaker IV

34.

What is the difference between boiling and evaporation?

a)

Boiling and evaporation are essentially the same process, just with different names.

b)

  1. Boiling is a liquid becoming a solid, while evaporation is a liquid into a gas.

c)

  1. Boiling requires heat, while evaporation occurs at room temperature.

d)

Boiling can happen spontaneously

35.

If isopropyl alcohol freezes at −89.5 °C, at what temperature will it melt?

a)

-100*C

b)

0*C

c)

-89.5*C

d)

Not enough information given

36.

If water is boiling at 100oC and you come back later to see the water still boiling, what temperature will the water be?

a)

100oC

b)

120oC

c)

89.5oC

d)

Not enough information is given.

37.

When some hot metal is placed in a calorimeter, what happens to the energy?

a)

It is absorbed by the water

b)

It is released by the water

c)

The metal retains its heat

d)

The energy is released outside the calorimeter

38.

If 50 grams of water at 20°C is mixed with 50 grams of water at 40°C in a calorimeter, what will be the final temperature of the mixture assuming no heat is lost to the surroundings?

a)

20oC

b)

30oC

c)

40oC

d)

60oC

39.

If 50 grams of water at 30°C is mixed with 50 grams of water at 50°C in a calorimeter, what will be the final temperature of the mixture assuming no heat is lost to the surroundings?

a)

20oC

b)

30oC

c)

40oC

d)

60oC

40.

If water at 125oC cools, condenses and cools as water to 50oC, what is the temperature change of the gas?

a)

25oC

b)

75oC

c)

-25oC

d)

-75oC

e)

125oC

41.

If water at 125oC cools, condenses and cools as water to 50oC, what is the temperature change of the water?

a)

50oC

b)

75oC

c)

-50oC

d)

-75oC

e)

125oC

42.

If ice at -20oC heats up, melts and continues heating up to 55oC, what is the temperature change for the ice?

a)

20oC

b)

75oC

c)

-20oC

d)

-75oC

e)

55oC

43.

If ice at -20oC heats up, melts and continues heating up to 55oC, what is the temperature change for the ice?

a)

20oC

b)

55oC

c)

-20oC

d)

-75oC

e)

75oC

44.
For the formula:
 Q= m c ∆T
The  units for specific heat are:
a)
g /J C
b)
°C/g J
c)
kJ/g
d)
J/g°C
45.
What would be the effect on the particles if more heat is supplied to the system?
a)
They would slow down
b)
They would stop moving
c)
They would speed up
d)
There would be no effect
46.
A solution is a ________ mixture. 
a)
heterogeneous 
b)
homogeneous 
c)
dumb 
d)
mixed 
47.
This is the part of the solution that does the dissolving. 
a)
solute
b)
solvent 
c)
salt water 
d)
First Continental Congress 
48.

The ______ is the smaller part of the solution.

a)

solute

b)

solvent

c)

system of a down

49.

This is a mixture that will settle over time if you let it sit.

a)

Suspension

b)

Colloid

c)

Mix - Mix a lot

50.
An unsaturated solution is one that....
a)
contains the maximum amount of dissolved solute.
b)
contains less solute than a saturated solution.
c)
contains more solute than a saturated solution.
d)
is the amount of a substance required to form a saturated solution.
51.
What is the molarity of a 2 liter solution containing 5 moles of NaCl?
a)
2.5
b)
0.4
c)
2.5 moles/liter
d)
10 moles/liter
52.
How many moles of NaCl are present in 6000. ml a 1.5 M NaCl solution?
a)
9 moles NaCl
b)
9000
c)
9
d)
4000  moles NaCl
53.

A solution that has more than the maximum amount of solute dissolved in the solvent is called __________________.

a)

saturated

b)

supersaturated

c)

unsaturated

d)

suspension

54.

When sugar is dissolved in water, the ______ is the solute.

a)

sugar

b)

water

55.

When you have added as much solute as can dissolve in the solvent, the solution is called:

a)

concentrated

b)

supersaturated

c)

saturated

d)

unsaturated

56.

The formula M1V1 = M2V2 is used when:

a)

dissolving a solute in a solvent

b)

diluting a solution

c)

reacting an acid with a base

d)

determining the pH of an acid

57.
How many grams of K2Cr2O7, are soluble in 100 g of water at 95 ºC?
a)
83 grams
b)
75 grams
c)
40 grams
d)
12 grams
58.
Which substance is MOST soluble at 0 ºC?
a)
KI
b)
NaNO3
c)
NaCl
d)
Ce2(SO4)3
59.
When 50 grams of KCl is dissolved in 100 grams of water at 50 ºC, the solution can be correctly described as:
a)
supersaturated
b)
unsaturated
c)
saturated
60.
When 20 grams of KNO3 is dissolved in 100 grams of water at 80 ºC, the solution can be correctly described as:
a)
supersaturated
b)
saturated
c)
unsaturated
61.
The amount of solute actually dissolved in a given amount of solvent.
a)
dilution
b)
concentration
c)
saturated solution
d)
supersaturated mixture
62.
What does it mean to dilute a solution?
a)
lower the concentration of solute per solvent
b)
increase the concentration of solute per solvent
63.

This type of mixture has large enough particles that you can see the different types of particles.

a)

Homogeneous

b)

Heterogeneous

c)

Colloid

d)

Solution

64.

A colloid mixture does not have particles large enough to settle to the bottom, but they are large enough to

a)

be filtered out of the solution.

b)

be pulled out by hand.

c)

float to the top.

d)

scatter light waves.

65.

A mixture with such small particles that you cannot see the individual particles.

a)

Suspension

b)

Sublimation

c)

Heterogeneous

d)

Homogeneous

66.

Which of the following examples is a Heterogeneous mixture?

a)

Tap Water

b)

Beach Sand

c)

Vanilla Cake Mix

d)

Bottle of Cola

67.

Which of the following examples is a Homogeneous mixture?

a)

Tap Water

b)

Beach Sand

c)

Chocolate chip cookie

d)

Mud water

68.

Which of the following examples is a Suspension?

a)

Mud water

b)

Well water

c)

milk

d)

Fog

69.

Which of the following types of solutions has more room to dissolve solute?

a)

supersaturated

b)

saturated

c)

unsaturated

70.

Which of the following will produce crystals if cooled or disturbed?

a)

unsaturated solution

b)

saturated solution

c)

supersaturated solution

d)

all of the above

71.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
72.
Molarity is measured in
a)
moles per kg
b)
mols per L
c)
moles per kJ
d)
moles per mL
73.

Which solution is more concentrated?

Solution 1:

500 mL of water

100 g of salt


Solution 2:

500 mL of water

90 g of salt

a)

Solution 1

b)

Solution 2

c)

They have the same concentration

d)

I have no idea

74.

Which solution is more diluted?

Solution 1:

1000 mL of water

60g of salt


Solution 2:

500 mL of water

60 g of salt

a)

Not enough information to tell

b)

Solution 1

c)

Solution 2

d)

They are equally diluted

75.

As we dilute a solution.....

a)

The volume increases and the molarity (M) increases

b)

The volume increases and the molarity (M) decreases

c)

The volume decreases and the molarity (M) increases

d)

The volume decreases and the molarity (M) decreases

76.
What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250 mL?
a)
15.9 M
b)
0.636 M
c)
0.642 M
d)
1.59 M
77.

What volume, in milliliters, of 10.0 M NaOH is needed to prepare 300.0 mL of 2.00 M NaOH by dilution?

a)

0.067 mL

b)

60.0 mL

c)

100 mL

d)

125 mL

78.

Which beaker has the lowest concentration?

a)

Beaker A

b)

Beaker B

c)

Beaker C

d)

Beaker D

79.

Which beaker has the highest concentration?

a)

Beaker A

b)

Beaker B

c)

Beaker C

d)

Beaker D

80.

Beaker D is diluted, which beaker represents this change?

a)

Beaker A

b)

Beaker B

c)

Beaker C

81.

PCl5 + ___ H2O → ___ HCl + H3PO4

a)

4, 5

b)

1, 6

c)

3, 8

d)

2,2

82.

__ Al + __ FeO → Al2O2 + __ Fe

a)

1, 1, 2

b)

2,1,2

c)

2, 2, 2

d)

2,4,2

83.
 Mg  +  ___ HCl  →   MgCl2  +   H2
a)
1
b)
2
c)
3
d)
4
84.
Which side of a chemical equation is the reactant side?
a)
Left (before the yields sign)
b)
Right (after the yields sign)
85.
Which side of a chemical equation os the product side?
a)
Left (before the yields sign)
b)
Right (after the yields sign)
86.
Which problem is balanced?
a)
PbO2 + 2H2
b)
SO2 + H20 --> H2SO4
c)
2Na + 2H2O --> 2NaOH + H2
87.
Balance this equation.
_SnO2 +_H2-->_Sn +_H2O
a)
1,1,2,1
b)
1,2,1,1
c)
1,2,1,2
d)
1,2,2,1
88.
Balance this equation.
_CF4 + _Br2 -- _CBr4 + _F2
a)
2,1,2,1
b)
1,2,2,1
c)
1,2,1,2
d)
2,2,2,2
89.
What is the little number after an element in a chemical equation called.
Example: H2
a)
Coefficient 
b)
Subscript
c)
Atom
d)
Equation
90.
What does the Law of Conservation of Mass state?
a)
Matter cannot be gained or lost in a chemical reaction.
b)
Matter can only be lost in a chemical reaction.
c)
Matter can only be gained in a chemical reaction.
d)
Matter can be gained and lost in a chemical reaction. 
91.
Is the equation balanced?: 2H2O + O2 --> 4MgO + 3Fe
a)
Yes
b)
No
92.
Balance this equation
_Al +_HCl --> _H2 +_AlCl3
a)
2, 6, 3, 2
b)
it is already balanced
c)
4, 12, 3, 4
d)
2, 1, 4, 5
93.
Balance this equation.
_CH4 + _O2 --> _CO2 + _H2O
a)
1,2,1,1
b)
2,1,2,1
c)
1,2,1,2
d)
0,2,0,2
94.
Balance this equation.
_CF4 + _Br2 -- _CBr4 + _F2
a)
2,1,2,1
b)
1,2,2,1
c)
1,2,1,2
d)
2,2,2,2
95.
Is this equation balanced?
a)
yes
b)
no
c)
Not enough information
96.
How many atoms of aluminum are on each side of the following equation: 4Al + 3O2 --> 2Al2 O3
a)
2
b)
6
c)
1
d)
4
97.
When balancing equations a ____ can be placed to the left of a formula of a substance to make the equations balanced
a)
charge
b)
subscript
c)
random number
d)
coefficient
98.
How many atoms of carbon (C) are in C6H12O6?
a)
3
b)
6
c)
12
d)
24
99.

The two sides of a chemical equation are called?

a)

Reactants (left) and Products (right)

b)

Ingredients (left) and Product (right)

c)

Cations and Anions

d)

Reactants (left) and Results (right)

100.
How many atoms are there TOTAL in:
H2SO4
a)
6
b)
5
c)
7
d)
3
101.
How many nitrogen atoms does NH3 have?
a)
1
b)
2
c)
3
d)
4
102.
How many oxygen atoms are in this chemical formula?
a)
6 oxygen atoms
b)
2 oxygen atoms
c)
3 oxygen atoms
d)
4 oxygen atoms
103.

This picture is an example of burning a hydrocarbon which is what type of reaction?

a)

Combustion

b)

Synthesis

c)

Endothermic

d)

Decomposition

104.

Which of the following is an example of a synthesis reaction?

a)

AX -> A + X

b)

A + X -> AX

c)

ABC -> A + B + C

d)

CH + 02 -> CO2 + H2O

105.

Which of the following is an example of a decomposition reaction?

a)

AX -> A + X

b)

A + X -> AX

c)

A + B + C -> ABC

d)

CH + O2 -> CO2 + H20

106.

Which type of reaction has the following general pattern?

ABC → A + B + C

a)

synthesis

b)

combustion

c)

decomposition

d)

endothermic

107.

Identify the type of reaction:

Ca + O2 --> CaO

a)

Decomposition

b)

Synthesis

c)

Endothermic

d)

Combustion

108.

Predict the products :

C3H8 + O2 -->

a)

CH4

b)

CO2

c)

H2O

d)

H2

109.

Predict the products:

Al + Cl2 -->

a)

AlCl

b)

AlCl2

c)

AlCl3

110.

What type of chemical rxn this?

Mg + O2 --> MgO

a)

Decomposition

b)

Combustion

c)

Synthesis

d)

Single Replacement

111.

What type of reaction involves the production of CO2 and H2O usually?

a)

Synthesis

b)

Decomposition

c)

Combustion

d)

Activity Series

112.
NO2 →N2 + O2
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Combustion
113.
_P4+_O2 →  _P2O3
a)
3 P4+1 O2 → 2 P2O3
b)
1 P4+1 O2 → 2 P2O3
c)
1 P4+ 3 O2 → 2 P2O3
d)
1 P4+ 2 O2 → 3 P2O3
114.
What is the product when rubidium and oxygen gas react?
a)
RbO2
b)
Rb2O
c)
RbO
d)
Rb2O2
115.
Predict the products for the following reactants.
Mg + I2 --> 
a)
MgI
b)
MgI2
c)
Mg + I2
d)
Mg2I
116.

Predict the product of the following synthesis reaction.

Fe (III) + O2 -->

a)

Fe2O3

b)

Fe3O3

c)

Fe3O2

d)

FeO

117.

If an element is diatomic it should have a subscript of___

a)

1, always

b)

2, only when it is an element

c)

it shouldn't have a subscript, it should have a coefficent

d)

2, when bonded in a compound

118.

Predict the products for the decomposition of aluminum oxide, Al2O3 →

a)

Al + O2

b)

O + Al2

c)

Al2 + O3

d)

Al + O

119.
What is the molar mass of C6H12O6?
a)

180.18 g/mol

b)

180.12 g/mol

c)

180.24 g/mol

d)

180.06 g/mol

120.
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
121.
4 Al + 3 O2 –> 2 Al2O3  How much aluminum would be needed to completely react with 45 grams of O2?
a)
1.05 moles
b)
3.75 moles
c)
1.875 grams
d)
1.875 moles
122.
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
123.
Cl2 + 2KBr → Br2 + 2KCl
How many grams of potassium chloride (KCl) can be produced from 356 g of potassium bromide (KBr)?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
124.
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
125.
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
126.
C5H12O (l) combusts in air.  How many grams of water are produced when 56.44 grams of C5H12O combusts?
a)
69.21 g H2O
b)
55.44 g H2O
c)
20.55 g H2O
d)
35.46 g H2O
127.
What is decomposition?
a)
putting substances together
b)
breaking substances apart
c)
element replacing another element in a compoud
d)
burning of a subtance
128.
Which of the following is an example of a synthesis reaction:
a)
2 H2O → 2 H2 + O2 
b)
2 Na + Cl2 → 2 NaCl
c)
CH4 + 2 O2 → 2 H2O + CO2
d)
2 HCl + Zn → ZnCl2 + H2
129.
What do the coefficients tell us in a chemical equation?
a)
The number of atoms within the compound or element.
b)
The ratio of elements/compounds in the balanced equation.
130.
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
131.
Why must chemical equations be balanced?
a)
So that the equation doesn't explode
b)
The reaction won't happen until it is balanced
c)
Matter cannot be created or destroyed, merely rearranged
d)
None of these
132.
What must go in the blank space to balance the equation?
4Fe  +  _O2  → 2Fe2O3
a)
1
b)
2
c)
3
d)
4
133.
What is H2O in the following equation:
 
2 H2 + O2 → 2 H2O
a)
Ion
b)
Product
c)
Reactant
d)
Unbalanced
134.

D represents

a)

Potential Energy of Products

b)

Potential Energy of Reactants

c)

Change in Enthalpy

d)

Activation Energy

135.

A represents

a)

Potential Energy of Products

b)

Potential Energy of Reactants

c)

Change in Enthalpy

d)

Activation Energy

136.

B represents

a)

Potential Energy of Products

b)

Potential Energy of Reactants

c)

Change in Enthalpy

d)

Activation Energy

137.

When balancing an equation, you can NEVER change the...

a)

Coefficients

b)

Subscripts

138.

The small number after an element is called a...

a)

Reactants

b)

Products

c)

Coefficient

d)

Subscript

139.

The molecules and atoms on the right side of the arrow are called...

a)

Reactants

b)

Products

c)

Coefficient

d)

Subscript

140.

The molecules and atoms on the left side of the arrow are called...

a)

Reactants

b)

Products

c)

Coefficient

d)

Subscript

141.

The large number in front of a molecule is called then....

a)

Reactants

b)

Products

c)

Coefficient

d)

Subscript

142.

This reaction is an example of....

a)

Synthesis

b)

Decomposition

c)

Combustion

d)

Single Replacement

e)

Double Replacement

143.

This reaction is an example of....

a)

Synthesis

b)

Decomposition

c)

Combustion

d)

Single Replacement

e)

Double Replacement

144.

This reaction is an example of....

a)

Synthesis

b)

Decomposition

c)

Combustion

d)

Single Replacement

e)

Double Replacement

145.

Baking a cake is a...

a)

Chemical change

b)

Physical change

146.

Mixing salt and water is a...

a)

Chemical change

b)

Physical change

147.
Which of the following is a sign that a chemical reaction has occurred?
a)
change in shape
b)
melting
c)
formation of a gas
d)
dissolving
148.
How many Al atoms are in this compound?         4Al2O3
a)
2
b)
8
c)
6
d)
4
149.
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
150.

How do we make a dilution?

a)

Add more solute

b)

Remove solute

c)

Remove solvent

d)

Add more solvent

151.

As we dilute a solution.....

a)

The volume increases and the molarity (M) increases

b)

The volume increases and the molarity (M) decreases

c)

The volume decreases and the molarity (M) increases

d)

The volume decreases and the molarity (M) decreases

152.

Balance this equation ​ (a)   N2 + ​ (b)   H2 --> ​ (c)   NH3

Choose from the below words
1
3
2
153.

Balance this equation. _CF4 + _Br2 → _CBr4 + _F2

a)

3,1,2,1

b)

1,2,1,2

c)

2,2,2,2

154.
Which of the following equations are correctly balanced?
a)

12CO2 +H2O --> C6H12O6 + O2

b)

CO2 + 9H2O --> C6H12O6 + O2

c)

CO2 + H2O --> 3C6H12O6 + O2

d)

6CO2 + 6H2O --> C6H12O6 + 6O2

155.
What is the molar mass of C6H12O6?
a)

180.18 g/mol

b)

180.12 g/mol

c)

180.24 g/mol

d)

180.06 g/mol

156.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
157.
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
158.
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
159.
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
160.

48.86 g of cobalt is equal to how many moles of cobalt?

a)

2879 moles

b)

8.291 moles

c)

.8291 moles

d)

.829 moles

161.

In an endothermic reaction, energy is _________.

a)

absorbed

b)

released

162.

____ reactions usually feel cold.

a)

endothermic

b)

exothermic

163.

_____ reactions usually feel hot!

a)

endothermic

b)

exothermic

164.

Solid --> liquid --> gas is what type of reaction?

a)

endothermic

b)

exothermic

c)

catalytic

d)

inhibited

165.

gas --> liquid --> solid is what type of reaction?

a)

endothermic

b)

exothermic

c)

catalytic

d)

inhibited

166.

Endo means in or _______.

a)

absorbed

b)

released

167.

Exo means out or ________.

a)

absorbed

b)

released

168.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
169.

What is the Heat of Reaction ΔH\Delta H  for this reaction?

a)

-200 KJ

b)

200 KJ

c)

400 KJ

d)

-300 KJ

170.

How much activation energy is needed for this reaction?

a)

300 KJ

b)

500 KJ

c)

400 KJ

d)

100 KJ

171.

What type of reaction is this?

a)

Exothermic

b)

Endothermic

c)

Energy Producing

d)

No way to tell

172.

What kind of equation is this: 2KI + MgCl2 + 200KJ ----> 2KCl + MgI2

a)

Endothermic

b)

Exothermic

173.
What would be the effect on the particles if more heat is supplied to the system?
a)
They would slow down
b)
They would stop moving
c)
They would speed up
d)
There would be no effect
174.

How can you tell this reaction is exothermic: MgO + CaS ----> CaO + MgS + 200 KJ

a)

Energy is written on the reactants side

b)

Energy is being released

c)

Energy is being absorbed

175.

if more heat energy is released in making bonds in the products than is taken in when breaking bonds in the reactants

a)

Exothermic

b)

Endothermic

c)

Exotermic

d)

Endotermic

176.

The potential energy diagram of a reaction is shown. Which statement below is correct relating to this reaction?

a)

#1 represents the enthalpy change for this exothermic reaction.

b)

#2 represents the enthalpy change for this endothermic reaction.

c)

#3 represents the enthalpy change for this endothermic reaction.

d)

#4 represents the enthalpy change for this exothermic reaction.

177.
When you dropped a hot metal sample into room temperature water in the lab what happened?
a)
the heat from the metal traveled into the water
b)
the cool from the water traveled into the hot metal
c)
both of the other answers are correct
178.

When heat flows from system to the surroundings that is an example of an ________________ process.

a)

exothermic

b)

endothermic

179.

Heat flows from _______ to _________.

a)

warm to cool

b)

cool to warm

180.

When a bond is being formed, energy must be....

a)

absorbed

b)

released

181.

When a bond is being broken, energy must be....

a)

absorbed

b)

released

182.
What is a limiting reactant?
a)
the reactant that determines how much product can be made
b)
the reactant that is in excess
c)
the product that you can make the most of
d)
the amount of reactants that react with each other
183.
Fe + S --> FeS
If 7.62g Fe react with 8.67g S, what is the limiting reactant?
a)
Fe
b)
S
c)
FeS
d)
none 
184.
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
185.

When reacting Na with Cl2, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

a)

90.4%

b)

104%

c)

96.15%

d)

1.04%

186.

2Fe2O3 + 3C → 4Fe + 3CO2

You add 28 grams of carbon. You find the actual yield to be 81.2 grams of CO2. What is the percent yield of CO2? (Hint: calculate theoretical yield of CO2 first)

a)

58.83%

b)

308%

c)

6435%

d)

79.14%

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