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ALC Final Exam Review BORO

Total questions: 132

Worksheet time: 6hrs 51mins

Name
Class
Date
1.
When humans burn fossil fuels, most of the carbon quickly enters the _______ as carbon dioxide
a)
water
b)
atmosphere
c)
sun
d)
air
2.

What process keeps Earth's temperature suitable for life?

a)

Convention currents

b)

Greenhouse Effect

c)

Albedo Effect

d)

Water Cycle

3.
Why does too much carbon dioxide in the atmosphere cause climate change?
a)
It cools our planet
b)
Blocks out UV rays
c)
Traps heat and warms planet
d)
Lets light escape
4.
Which of the following adds oxygen to the atmosphere
a)
forest fires
b)
photosynthesis
c)
weathering of rocks
d)
life processes of animals
5.
Deforestation contributes to the greenhouse gasses by
a)
loss of trees that would otherwise remove carbon dioxide from the air
b)
as trees are cut, they release carbon dioxide
c)
increasing the amount of oxygen in the air
6.
Carbon is stored in
a)
trees and other living things
b)
oceans
c)
underground in soil and fossil fuels
d)
all are correct
7.

Carbon dioxide is absorbed by plants to make what in photosynthesis? (choose all that apply)

a)

oxygen (O2)

b)

carbon (C)

c)

carbohydrates (C6H12O6)

d)

water (H2O)

8.

TRUE or FALSE?

All of the carbon on our planet is continually recycled in the carbon cycle.

a)

True

b)

False

9.
The average temperature of the surface of Earth has increased approximately 1°C in the past century. Which reason best explains this increase in temperature?
a)
lower levels of ozone in the atmosphere
b)
lower levels of nitrogen in the atmosphere
c)
higher levels of carbon dioxide and other greenhouse gases in the atmosphere
d)
higher levels of oxygen in the atmosphere
10.

Which of the following statements is true concerning acids and bases?

a)

acids and bases don't react with each other

b)

acids mixed with bases neutralize each other

c)

acids mixed with bases make stronger bases

d)

acids mixed with bases make stronger acids

11.
When carbon dioxide dissolves from the air into the ocean- the interaction is between...
a)
The atmosphere and geosphere 
b)
The atmosphere and hydrosphere 
c)
The atmosphere and biosphere 
d)
The atmosphere and atmosphere 
12.

Which of the following is not a part of the hydrosphere?

a)

lakes

b)

rivers

c)

fish

d)

rain

13.
When a plants takes carbon dioxide from the air which two spheres are interacting? 
a)
Biosphere and atmosphere 
b)
Geosphere and atmosphere 
c)
Hydrosphere and atmosphere 
d)
Atmosphere and atmosphere 
14.

If the specific heat of water is 4.186 J/g∙°C, how much heat is required to increase the temperature of 1,200 g of water 16 °C? Use the equation q = mc∆T

a)

-80,371.2 J

b)

44,938.6 J

c)

80,371.2 J

d)

112,575.9 K

15.

Copper, Stainless Steel, Carbon Steel, and Zinc were all heated using the same amount energy. What material would be have the LARGEST change in temperature? (Reminder: Specific heat capacity can be described as a substance’s resistance to temperature changes.)

a)

Copper

b)

Carbon Steel

c)

Zinc

d)

Stainless Steel

16.

Copper, Stainless Steel, Carbon Steel, and Zinc were all heated using the same amount of energy. Based on the chart, which material would be have the SMALLEST change in temperature? (Reminder: Specific heat capacity can be described as a substance’s resistance to temperature changes.)

a)

Copper

b)

Carbon Steel

c)

Zinc

d)

Stainless Steel

17.

Letter for heat energy...

a)

q

b)

m

c)

c

d)

ΔT

18.

Letter for specific heat

a)

q

b)

m

c)

c

d)

ΔT

19.

Letter for change in temperature

a)

q

b)

m

c)

c

d)

ΔT

20.

Letter for mass

a)

q

b)

m

c)

c

d)

ΔT

21.

Identify the given m in problem:

a)

15.75 g

b)

1086.75 J

c)

150°C

d)

unknown (aka ?)

22.

Identify the given ΔT in problem:

a)

15.75 g

b)

1086.75 J

c)

150°C

d)

unknown (aka ?)

23.

Identify the given q in problem:

a)

15.75 g

b)

1086.75 J

c)

150°C

d)

unknown (aka ?)

24.

Identify the given c in problem:

a)

15.75 g

b)

1086.75 J

c)

150°C

d)

unknown (aka ?)

25.

What is the unknown in this problem?

a)

q

b)

m

c)

c

d)

ΔT

26.

Heat always travels from...

a)

Warm to cool

b)

Cool to warm

c)

Warm to warm

d)

Cool to cool

27.
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
28.
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
29.

If two objects have different temperatures when they come in contact, heat will flow from the warmer object to the cooler one UNTIL ____________

a)

one reaches a temperature of zero

b)

they both have an equal temperature

c)

one runs out of energy

30.

For a skillet, used for cooking, do you want a high or low specific heat

a)

High, so that it will need more energy to heat up

b)

Low, so that it will change temperature quickly

31.
A sample of iron receives 50.J of heat energy that raises the temperature of the iron by 25.0°C. If iron has a specific heat of 0.10 J/g°C, what is the mass of the iron sample?  (show your work)
a)
25g
b)
30g
c)
20g
d)
50g
32.
Calorimetry Question:
A piece of metal with a mass of 32.8 g is heated to 100.5°C and dropped into 138.2 g of water at 20.0°C.  The final temperature of the system is 30.2°C.  What is the specific heat capacity of the metal? (show your work)
a)
2.56 J/g°C
b)
0.391 J/g°C
c)
5.29 J/g°C
d)
3.50 J/g°C
33.
A metal cube at temperature of 10°C immersed in a liquid at temperature of 70°C.
What is the temperature of the metal cube when thermal equilibrium is achieved between the cube and the liquid?
a)
Between 10°C and 70°C
b)
More than 70°C
c)
Less than 10°C
d)
Same as the room temperature
34.

A sample of iron receives 50.J of heat energy that raises the temperature of the iron by 25.0°C. If iron has a specific heat of 0.10 J/g°C, what is the mass of the iron sample?

a)

25g

b)

30g

c)

20g

d)

50g

35.

Consider the heat equation,
 q=m⋅c⋅ΔTq=m\cdot c\cdot\Delta T  


If the same amount of heat is added to the same amount of two different materials; the material with the largest specific heat  will have the ________________ temperature change.

a)

largest

b)

smallest

36.

Specific heat of water is 4.18 J/g°C. Specific heat of wood is 1.760 J/g°C What material needs more energy to raise the temperature by 1 degree Celsius?

a)

Water

b)

Wood

c)

Both are same

37.

A metal cube at temperature of 70°C is immersed in water at temperature of 20°C. The final temperature of the mixture will be

a)

Between 20°C and 70°C

b)

More than 70°C

c)

Less than 20°C

d)

Same as the room temperature

38.

A metal cube at temperature of 70°C is immersed in water at temperature of 20°C. The metal _______ heat while the water __________ heat.

a)

gains, loses

b)

loses, gains

39.

If an 85.0 g sample of copper with a specific heat of 0.41 J/g°C is cooled from 45°C to 25°C, how much energy will it lose?

a)

-497 J

b)

-846 J

c)

-697 J

d)

-346 J

40.

Calculate the heat absorbed by 105.0 grams of water when it is heated to cook spaghetti. The initial temperature of the water is 20.0°C, and the final temperature of the water is 99.0°C. The specific heat of water is 4.18 J/g•°C.

a)

8778 J

b)

0.0005 J

c)

34673 J

d)

43451.1 J

41.

A piece of copper alloy with a mass of 85.0 g is heated from 30.0°C to 45°C. In the process, it absorbs 523 J of energy as heat. What is the specific heat of the copper?

a)

0.41 J/g°C

b)

0.73 J/g°C

c)

0.29 J/g°C

d)

0.57 J/g°C

42.

A metal cube with a mass of 55grams at temperature of 85°C is immersed in 150grams of water at temperature of 20°C. The metal and water then reach a final temperature of 23oC. What is the specific heat of the metal?

a)

0.55 J/goC

b)

2120 J/goC

c)

11.4 J/goC

d)

4.18 J/goC

e)

0.75 J/goC

43.

What are the two factors to look for when determining if the reaction is at equilibrium?

a)

Forward reaction rate is faster than the reverse and concentrations of reactants and products are equal

b)

Forward and reverse reaction rates are equal and concentrations of reactant and products are constant

c)

Forward and reverse reaction rates are equal and concentrations of reactants and products are equal

d)

Forward reaction rate is faster than the reverse and concentrations of reactants and products are equal

44.

Select all of the statements that are always correct about dynamic equilibrium

a)

established when the product and reactant concentrations are equal

b)

achieved when the forward and reverse reaction rates are same

c)

established when the concentration of reactants is unchanging

d)

achieved when the forward and reverse reactions stop occurring

45.

At what time did the reaction establish equilibrium?

a)

t1

b)

t2

c)

t3

d)

t4

46.

Given the equation representing a reaction:

N2O4(g) ⇌ 2NO2(g)


Which statement describes this reaction at equilibrium?

a)

The concentration of N2O4(g) must equal the concentration of NO2(g).

b)

The concentration of N2O4(g) and the concentration of NO2(g) must be constant.

c)

The rate of the forward reaction is greater than the rate of the reverse reaction.

d)

The rate of the reverse reaction is greater than the rate of the forward reaction.

47.

The statement that if a system at equilibrium is disturbed, the reaction will proceed in one direction or another in order to reestablish equilibrium, is known as:

a)

the principle of equilibrium

b)

Priestley’s principle

c)

Le Chatelier’s principle

d)

Faraday’s principle

e)

the law of mass action

48.

Consider the reversible reaction

N2 (g) + O2 (g) + 181 kJ (energy) ⇌ 2NO (g). Adding O2 will...

a)

shift the equilibrium left and increase [NO]

b)

shift the equilibrium right and increase [NO]

c)

shift the equilibrium left and decrease [NO]

d)

shift the equilibrium right and decrease [NO]

49.

Consider the reversible reaction

N2 (g) + O2 (g) + 181 kJ ⇌ 2NO (g).

If N2 is removed...

a)

the equilibrium will shift right, creating more products.

b)

the equilibrium will shift right, creating more reactants.

c)

the equilibrium will shift left, creating more products.

d)

The equilibrium will shift left, creating more reactants.

50.

Consider the reversible reaction

N2 (g) + O2 (g) + 181 kJ (energy) ⇌ 2NO (g). Which change will increase the amount of N2 at equilibrium?

a)

increasing the temperature

b)

adding a catalyst.

c)

decreasing the temperature.

d)

adding O2

51.

Consider the reversible reaction:

CO (g) + 2H2 (g) ⇌ CH3OH (g) + energy. Cooling the reaction mixture will ___.

a)

shift the equilibrium to the right and increase [CH3OH]

b)

shift the equilibrium to the left and increase [CH3OH]

c)

shift the equilibrium to the left and decrease [CH3OH]

d)

shift the equilibrium to the right and decrease [CH3OH]

52.

2SO2(g)+O2(g) ⇌ 2SO3(g) + Heat


Adding SO2(g) will

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase rate of reaction

d)

have no change

53.

2SO2(g)+O2(g) ⇌ 2SO3(g) + Heat


Increasing the temperature will...

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase pressure

d)

have no change

54.

2SO2(g) + O2(g) ⇌ 2SO3(g) + Heat


Removing O2(g) will

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase pressure

d)

have no change

55.

2SO2(g)+O2(g) ⇌ 2SO3(g) + Heat


Adding SO3(g) will

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase K

d)

have no change

56.

CoCI42- +6H2O →Co(H2O)62+ + 4CI-.


What would happen when H2O is added?

a)

Position of equilibrium will shift to left (and become more blue)

b)

Position of equilibrium will shift to right (and become more pink)

c)

Keq will increase as H2O is added

d)

Position of equilibrium will shift to left to reduce the added H2O

57.

Heat + 1 N2O4 → 2 NO2


What will happen when the temperature is increased?

a)

Position of equilibrium will shift to left and become lighter in color

b)

Position of equilibrium will shift to right and become more brown

c)

No change in position of equilibrium

d)

Position of equilibrium will shift to right and become lighter in color

58.

CoCI42- +6H2O →Co(H2O)62+ + 4CI- + Heat


What will happen when the temperature is increased?

a)

Position of equilibrium will shift to left and become more blue

b)

Position of equilibrium will shift to right and become more pink

c)

No change in position of equilibrium

d)

Position of equilibrium will shift to left and become more pink

59.
The rate of a chemical reaction is NOT affected by which of the following:
a)
temperature
b)
concentration
c)
particle size (surface area)
d)
All of these affect reaction rates
60.
Products will form faster if____________
a)
the particle size of the reactants are larger.
b)
temperature is decreased.
c)
concentration of the reactants are increased.
d)
the reaction is not stirred.
61.
A ______________ is a substance that increases the rate of a reaction without being used up during the reaction. 
a)
catalyst
b)
product
c)
reactant
d)
solute
62.

Which of the following will lower the rate

of reaction?

a)

adding an enzyme to the reaction

b)

decreasing the temperature from 40°C to

10°C

c)

breaking a chunk of calcium up into

smaller pieces

d)

increasing the amount of solute

dissolved in a solution

63.

According to the graph, it can be concluded that

a)

As reaction progresses, the concentration of product will reduce and the reactant will increase

b)

As reaction progresses, the concentration of product and reactant will reduce

c)

As reaction progresses, the concentration of product and reactant will increase

d)

As reaction progresses, the concentration of product will increase, the reactant will reduce

64.

Which group of particles shows that increasing surface area increases collisions among particles?

a)

Left side

b)

Right side

c)

Cannot be determined by either picture

65.
The following graph shows two different reaction pathways for the same overall reaction at the same temperature. Which pathway is slower and why?
a)
Red, because the activation energy is larger
b)
Blue, because the activation energy is lower
c)
both reaction progress at the same rate
66.

Which line shows the effect of a catalyst on activation energy?

a)

The blue line

b)

The green line

c)

none of the lines

d)

both lines

67.

Raising the temperature speeds up the rate of a chemical reaction by increasing

a)

The effectiveness & frequency of collisions

b)

The effectiveness of collisions only

c)

The frequency of collisions only

d)

none of these

68.

Food spoilage is a huge problem in the USA. If you were a food scientist, what would you propose grocery stores do to prevent food from spoiling?

a)

add a catalyst to all food products

b)

lower the temperature inside the store

c)

make sure the food is cut-up into small pieces

69.

H2(g)+Cl2(g)⇌2HCl(g)

The forward reaction is exothermic. What will happen to the equilibrium if the temperature is increased?

a)

equilibrium shifts right

b)

equilibrium shifts left

c)

You cannot predict the effect

d)

no change

70.
At what time the reaction reached equilibrium?
a)
t1
b)
t2
c)
t3
d)
t4
71.
At what time (in seconds) is equilibrium established?
a)
0 seconds
b)
1 second
c)
5 seconds
d)
10 seconds
72.
Which of the following is NOT true at equilibrium?
a)
The forward and reverse reactions proceed at the same rate.
b)
The concentrations of reactants and products do not change.
c)
The concentration of the reactants is equal to the concentration of the products.
d)
The forward and reverse reactions continue to occur.
73.
Which conversion factor should be used for the following question " How many molecules are there in 4.00 moles of glucose, C6H12O6? 
a)
1 mole = 78.12 g
b)
1 mole = 22.4 L 
c)
1 mol = 6.02x 1023 particles 
d)
more than one
74.
Which conversion factor should be used to solve the following, "How many moles in 28 grams of CO2?"
a)
1 mol = 22.4 L 
b)
1 mol = 44.01 g
c)
1 mol = 6.02x1023 atoms
d)
more than one
75.
The number 6.02 x 1023, which is the number of particles found in a mole. 
a)
molar mass
b)
mole
c)
Avogadro's number
d)
hydrate
76.
How many moles are in 16.94g of water?
a)
16.94 mol H2O
b)
0.9401 mol H2O
c)
305.3 mol H2O
d)
1.063 mol H2O
77.
How many molecules are in 9.44 moles of AlCl3?
a)
5.68 molec AlCl3
b)
5.68x1024 molec AlCl3
c)
0.705 molec AlCl3
d)
1.25x1023 molec AlCl3
78.
How many molecules of sugar (C6H12O6) are in a mole?
a)
24 molecules
b)
180 molecules
c)
180 g
d)
6.02 x 1023 molecules
79.
Which of the following dimensional analysis setups will correctly convert 27.76g of Li to atoms of Li?
a)
A
b)
B
c)
C
d)
D
80.
How many moles are in 19.82 g Mg? 
a)
1.226mol Mg
b)
481.7mol Mg
c)
1.000mol Mg
d)
 0.8156 mol Mg
81.
Which of the following dimensional analysis setups will correctly convert 4.00x1023atoms of cobalt to moles of cobalt? How many moles of colbalt are there?
a)
setup B : 0.6644mol Co
b)
setup A: 2.41x1047mol Co
c)
setup A : 0.664mol Co
d)
setup B: 2.41x1047mol Co
82.
How many moles are in 3.01 x 1022 atoms of magnesium?
a)
0.050 moles
b)
1.81 x 1046 moles
c)
5.00 x 1021 moles
d)
5.00 moles
83.
Which has more atoms, 12.0 mol of C or 12.0 mol of Ca?
a)
12.0 mol C
b)
12.0 mol Ca
c)
They are equal
84.
What is the molar mass of AuCl3?
a)
96 g
b)
130 g
c)
232.5 g
d)
303.3 g
85.
What is the molar mass of table salt (NaCl)?
a)
116.886 g/mol
b)
35.453 g/mol
c)
22.990 g/mol
d)
58.443 g/mol
86.
What is the molar mass of one molecule of Nitrogen N2?
a)
14.01 amu
b)
14.01 g
c)
28.02 g
d)
28.02 amu
87.
What is the mass of one mole of aluminum?
a)
26.982 g
b)
13 g
c)
53.985 g
d)
14 g
88.

How many moles are in 15 grams of Lithium?

a)

2.14

b)

0.47

c)

105

d)

7

89.

How many grams are in 2.4 moles of Sulfur?

a)

76.8

b)

0.075

c)

13.3

d)

32

90.
4.0 moles of H2O would have what mass?
a)
72 g
b)
23 g
c)
68 g
d)
4.5 g
91.

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

92.

How many molecules of water are in a 821.3 g sample?

a)

45.58 molecules

b)

8.232 x 1025 molecules

c)

8.909 x 1027 molecules

d)

2.744 x 1025 molecules

93.

What is the mass of 4.98 x 1024 atoms of Zn?

a)

541 g

b)

8.27 g

c)

.122 g

d)

4.59 x 1046 g

94.

How many moles of sodium chloride are in a 321.8 g sample?

a)

18810 moles

b)

3.315 x 1024 moles

c)

5.507 moles

d)

4.767 moles

95.

How many formula units of calcium chloride are in a 25.69 g sample?

a)

1.394 x 1023 F.U.'s

b)

2851 F.U.'s

c)

.2315 F.U.'s

d)

3.845 x 1025 F.U.'s

96.

how many atoms are contained in a 456 g sample of carbon dioxide?

a)

10.34 atoms

b)

6.237 x 1024 atoms

c)

1.871 x 1025atoms

d)

2.079 x 1024 atoms

97.

What would be the mass of 9.76 x 1022 formula units of SrCl2?

a)

.1622 g

b)

25.7 g

c)

20.0 g

d)

.3589 g

98.

A sample of AlCl3 contains a total of 4.515 x 1027 atoms of chlorine. What must be the mass of this sample?

a)

2.500 x 105 g

b)

1.000 x 106 g

c)

18.75 g

d)

3.333 x 105 g

99.

Which of the following statements regarding the mole is INCORRECT?

a)

A mole is a unit of quantity equal to 6.02 x 1023 particles.

b)

The number of particles in a mole is known as Avogadro’s number.

c)

A mole of particles of an element is numerically equal to the atomic mass of the element.

d)

none of the above

100.

The mass of one mole of an element is equal to

a)

its atomic number from the periodic table, but in amus.

b)

its atomic mass from the periodic table, but in amus.

c)

its atomic mass from the periodic table, but in grams.

d)

its atomic number from the periodic table, but in grams.

101.

How many formula units are in 2.5 moles of NaCl?

a)

1.5 x1024 formula units

b)

1.5 formula units

c)

4.2 formula units

d)

4.2 x10-24 molecules

102.

Shivani measures out 6.0 moles of epsom salt (MgSO4) to put in her bath. How many grams of MgSO4 went in the bath?

a)

3.6 x 1024 g

b)

720 g

c)

0.050 g

d)

340 g

103.
How many molecules are there in 31.8 moles of water?
a)
5.28 x 10-23 molecules
b)
1.91 x 1025 molecules
c)
5.28x 10-25
d)
1.91 x 1022
104.

Determine the mass of 4.20 moles of C6H12

a)

353 g

b)

0.0499 g

c)

337 g

d)

2.53 x 1024 g

105.

What is the mass of 1.2 x 1024 atoms of C?

a)

2.0 grams

b)

24 grams

c)

0.17 grams

d)

1.4 x 1025 grams

106.

Calculate the number of atoms in 0.0340 g Zn.

a)

5.20 x 10-4 atoms Zn

b)

3.13 x 1023 atoms Zn

c)

3.13 x 1020 atoms Zn

d)

2.05 x 1022 atoms Zn

107.

How many grams are in 1.2 moles of neon?

a)

0.059 grams

b)

7.2 x 1023 grams

c)

2.0 x 10-24 grams

d)

24 grams

108.

How many moles are in 98.3 grams of aluminum hydroxide, Al(OH)3?

a)

1.26 moles

b)

0.8 moles

c)

7,670 moles

d)

1.63 x 10-22 moles

109.
How many formula units are there in 2.45 moles potassium chloride?
a)
4.07 x 10-24 
b)
1.47 x 1024 
c)
1.47
d)
4.07
110.

To melt the ice, Juan throws 455 g of calcium chloride, CaCl2 on his sidewalk. How many moles of CaCl2 did he throw?

a)

50,500 moles

b)

4.10 moles

c)

7.56 x 10-22 moles

d)

111 moles

111.

Each answer has a letter before it. Keep a tally of how many of each letter you correctly answer. When you have completed the quiz, the total number for each letter is your KEY

a)

I understand

b)

Yes, I get it

c)

I've got my pen and paper ready

d)

I won't forget to write down the letters

112.

N2 + 3H2 → 2NH3

What is the mole ratio between N2 and NH3 in the above reaction?

a)

A - 1 moles NH3 / 2 moles N2

b)

B - 2 moles NH3 / 1 moles N2

c)

C - 2 moles N2 / 3 moles NH3

d)

D - 1 moles N2 / 3 moles NH3

113.

Which of the following represent a mole ratio between silver nitrate and copper(II) nitrate in the following reaction:

2AgNO3 + Cu --> Cu(NO3)2 + 2Ag

a)

A - 2 mol AgNO3 / 2 mol Ag

b)

B - 2 mol Ag / 2 mol AgNO3

c)

C - 2 mol AgNO3 / 2 mol Cu(NO3)2

d)

D - 2 mol AgNO3 / 1 mol Cu(NO3)2

114.

4NH3 + 5O2-->4NO + 6H2O

What is the total number of moles of H2O produced when 12 mole of NH3 is completely consumed?

a)

A - 15

b)

B - 18

c)

C - 20

d)

D - 24

115.

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

What is the total number of moles of water needed to make 2.5 moles of C6H12O6?

a)

A - 2.5

b)

B - 6

c)

C - 12

d)

D - 15

116.

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)

A - 4 moles Fe

b)

B - 6 moles Fe

c)

C - 9 moles Fe

d)

D - 2 moles Fe

117.

N2 + 3H2 → 2NH3

How many moles of hydrogen are needed to react with 2 moles of nitrogen?

a)

A - 6

b)

B - 2

c)

C - 3

d)

D - 1

118.

2H2 + O2 → 2H2O

How many moles of water can be produced if 8 moles H2 are used?

a)

A - 4 moles

b)

B - 8 moles

c)

C - 16 moles

d)

D - 2 moles

119.

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)

A - 4 moles Fe

b)

B - 6 moles Fe

c)

C - 9 moles Fe

d)

D - 2 moles Fe

120.

Given the reaction: 4Al + 3O2 --> 2Al2O3

How many moles of Aluminum oxide, Al2O3, can you produce if you have 2 moles of Al?

a)

A - 3 mole

b)

B - 2 mole

c)

C - 1 mole

d)

D - 0.5 mole

121.

N2 + 3H2 −-> 2NH3

How many moles of ammonia are produced when 3 moles of nitrogen react with hydrogen?

a)

A - 6 moles ammonia

b)

B - 1.5 moles ammonia

c)

C - 9 moles ammonia

d)

D - 9 moles hydrogen

122.

Using the following equation:

Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)

How many moles of water can be made from 6 moles H2?

a)

A - 4 moles Fe

b)

B - 6 moles Fe

c)

C - 9 moles Fe

d)

D - 2 moles Fe

123.

Mole ratios are obtained from the

a)

A - balanced chemical equation

b)

B - periodic table

c)

C - molar mass

124.

What is the mole ratio of H2O to H3PO4 in the following chemical equation? P4O10 + 6 H2O --> 4 H3PO4

a)

A - 6:4

b)

B - 4:6

c)

C - 1:3

d)

D - 3:1

125.

What is the other name for the mole?

a)

A - El Ocho

b)

B - Guacamole

c)

C - Avogadro's number

d)

D - De Wey

126.

2 KClO3 → 2 KCl + 3 O2

How many moles of oxygen are produced when 6.7 moles of KClO3 decompose completely?

a)

A - 6.7 mol

b)

B - 1.0 mol

c)

C - 10.1 mol

d)

D - 4.5 mol

127.

When does a chemical reaction stop?

a)

A - When the lab is finished

b)

B - When both of the reactants are used up

c)

C - When one of the reactants is used up

d)

D - Chemical reactions never stop

128.

2 KClO3 → 2 KCl + 3 O2

How many moles of KCl are used when 6.7 moles of KClO3 decompose completely?

a)

A - 6.7 mol

b)

B - 1.0 mol

c)

C - 10.1 mol

d)

D - 4.5 mol

129.

S8 + 12 O2 → 8 SO3


How many moles of S8 is needed to react with 3 moles of O2?

a)

A - 0.25

b)

B - 1

c)

C - 4

d)

D - 36

130.

N2 + 3H2 → 2NH3


How many moles of N2 is needed to produce 3.5 moles of NH3?

a)

A - 1

b)

B - 1

c)

D - 1.75

d)

C - 3

131.

2 C2H6 + 7 O2 → 4 CO2 + 6 H2O


How many moles of CO2 is produced when 17.5 moles of O2 reacts fully?

a)

A - 4

b)

B - 7

c)

C - 10

d)

D - 30.63

132.

4 Fe + 3 O2 → 2 Fe2O3


How many moles of Fe is needed to react with 9.75 moles of O2?

a)

A - 3

b)

B - 4

c)

C - 13

d)

D - 39

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