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Chemistry Second semester Review

Total questions: 161

Worksheet time: 7hrs 19mins

Name
Class
Date
1.

How much KNO3 solute is saturated at 40 degrees?

a)

75

b)

55

c)

65

d)

85

2.

How much C12H22O11 solute is saturated at 40 degrees?

a)

240

b)

220

c)

230

d)

250

3.

How much Ce2(SO4)3 solute is saturated at 80 degrees?

a)

20

b)

15

c)

30

d)

2

4.

How much NaBr solute is saturated at 70 degrees?

a)

110

b)

120

c)

130

d)

140

5.

Which solute is MOST likely a gas?

a)

KNO3

b)

NaNO3

c)

KCl

d)

Ce2(SO4)3

6.

At what temperature can you fully dissolve 140g of NaNO3?

a)

62

b)

73

c)

81

d)

You cannot determine this

7.

At what temperature can you fully dissolve 60g of KNO3?

a)

27

b)

30

c)

37

d)

You cannot determine this

8.

At what temperature can you fully dissolve 120g of NaBr?

a)

70

b)

20

c)

100

d)

You cannot determine this

9.

What type of a solution is 60g NaNO3 at 40ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

10.

What type of a solution is 100g KNO3 at 40ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

11.

What type of a solution is 260g sugar at 50ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

12.

What type of a solution is 25g NaCl at 70ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

13.

What type of a solution is 55g KCl at 70ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

14.
How does a solution become supersaturated?
a)
dissolve lots of solvent in it.
b)
dissolve a little solute in it. 
c)
dissolve more solute than you should be able to. 
d)
dissolve a super amount of solvent in it. 

15-19.

Answer the questions below after watching the video

15.

What does molarity measure?

a)

The weight of solute per liter of solution

b)

The number of moles of solute per liter of solvent

c)

The density of the solution

d)

The volume of solvent per liter

16.

How can the molarity of a solution be determined if the mass of the solute is known?

a)

By measuring the density of the solution

b)

By dividing the mass by the volume of the solvent

c)

By multiplying the mass by the volume of the solution

d)

By converting the mass to moles using molar mass and dividing by the solution volume

17.

What is the effect of dilution on the concentration of a solution?

a)

Changes the molar mass of the solute

b)

Does not change the concentration

c)

Decreases the concentration

d)

Increases the concentration

18.

How is the new concentration after dilution calculated?

a)

By dividing the initial concentration by the final volume

b)

By subtracting the final volume from the initial concentration

c)

By multiplying the initial concentration by the initial volume and dividing by the final volume

d)

By adding the initial and final volumes

19.

What happens to the concentration of a solution if the volume is doubled?

a)

It doubles

b)

It remains the same

c)

It quadruples

d)

It is halved

20.

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

21.

A student is preparing solutions for a laboratory experiment by dissolving solid solutes in liquid solvents. Which action will increase the rate of solubility

a)

lowering the temperature of the solvent

b)

stirring the solute in the solution

c)

increasing the pressure on the solution

d)

increasing the particle size of the solute

22.

Which of the following substances is a heterogeneous substance?

a)

baby oil

b)

rocky road ice cream

c)

salt water

d)

milk

23.

Which of the following substances is a homogeneous solution?

a)

chocolate chip cookie

b)

italian dressing

c)

apple juice

d)

orange juice

24.

Which of the following is the correct formula for calculating molarity?

a)

moles/liters of solution

b)

moles/kg of solvent

c)

# particles/Avogadro's #

d)

theoretical yield/actual yield

25.

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

a)

supersaturated

b)

saturated

c)

unsaturated

26.

When calculating molality, Kg of the following are included in the calculation?

a)

solvent

b)

solute

c)

none of these

d)

solvent & solute

27.

To calculate molality you only need which of the following?

a)

scale

b)

flask

28.

What is the molality of a solution in which 3.0 moles of NaCl is dissolved in 1.5 Kg of water?

a)

2.0 M

b)

0.22 m

c)

135 m

d)

2.0m

29.

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

30.

The concentration of a mixture can be increased in which of the following ways?

a)

Heating the mixture

b)

Adding more water “solvent”

c)

Adding more powder “solute”

d)

Stirring the mixture

31.

air is a 

a)

compound

b)

element

c)

heterogeneous mixture

d)

solution

32.

Another name for a homogeneous mixture is 

a)

an element.

b)

a solution.

c)

a compound.

33.

If water is a polar molecule, then which of the following must be nonpolar

a)

sugar

b)

salt

c)

oil

d)

juice

34.

Electrolytes

a)

don't conduct electricity

b)

conduct electricity

35.

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

36.

Since "like dissolves like", water and oil will not mix because

a)

both of them are polar

b)

both of them are nonpolar

c)

oil is polar and water is nonpolar

d)

oil is nonpolar and water is polar

37.

What is the molarity of a 2 liter solution containing 5 moles of NaCl?

a)

5.0

b)

0.4

c)

2.5 moles/liter

d)

10 moles/liter

38.

How many liters would you need to get 0.5 moles if you had a 0.1M solution?

a)

0.05 liters

b)

0.2 liters

c)

5 liters

d)

2 liters

39.

Molarity is ...

a)

grams of solute/deciliters of solvent.

b)

grams of solute/liters of solution.

c)

moles of solute/liters of solution.

d)

moles of solute/milliliters of solvent.

40.

Which sweet tea would you expect to taste the sweetest?

a)

1M

b)

3M

c)

3.1M

d)

2.5M

41.

Which law states that energy cannot be created nor destroyed, but it can be transformed or transferred?

a)

Dalton's Law

b)

Law of conservation of energy

c)

Hess's Law

d)

E=mc^2

42.

What happens when kinetic energy increases?

a)

Temperature increases.

b)

Temperature decreases.

c)

Temperature is not affected by kinetic energy.

43.

A liquid has _________ temperature than a solid.

a)

Higher

b)

Lower

44.

A gas has ________ kinetic energy than a liquid.

a)

more

b)

less

45.

A sample of a compound has a mass of 30 g and a specific heat of 0.258 J/g*K. If its temperature drops 40 K, how much heat was released? ( q=mcΔTq=mc\Delta T  )

a)

309.6 J

b)

-309.6 J

c)

465 J

d)

-465 J

46.

A sample of a compound has a mass of 77 g and a specific heat of 0.885 J/g*K. In order to increase the temperature by 25 degrees Celsius, how much heat must be added? ( q=mcΔTq=mc\Delta T  )

a)

-3.48 J

b)

3.48 J

c)

1704 J

d)

-1704 J

47.

When water evaporates, the process is...

a)

endothermic

b)

exothermic

48.

When wood is burned in a campfire, the process is...

a)

endothermic

b)

exothermic

49.

For an exothermic reaction, ΔH\Delta H  is...

a)

negative

b)

positive

50.

For an endothermic reaction, ΔH\Delta H  is...

a)

negative

b)

positive

51.

In the following reaction, A + 2B --> 3C, ΔH = 640 kJ\Delta H\ =\ 640\ kJ  . How much energy is needed to react 4 moles of A?

a)

2560 kJ

b)

1280 kJ

c)

1920 kJ

d)

3840 kJ

52.

In the following reaction, 2A + 2B --> C, ΔH=−60 kJ\Delta H=-60\ kJ  . What is the ΔH\Delta H  when 6 moles of A are reacted?

a)

-180 kJ

b)

-360 kJ

c)

180 kJ

d)

360 kJ

53.

In an exothermic reaction, heat is a...

a)

product

b)

reactant

54.

In an endothermic reaction, heat is a...

a)

product

b)

reactant

55.

If you touch an exothermic reaction, it will feel...

a)

hot

b)

cold

56.

If you touch an endothermic reaction, it will feel...

a)

hot

b)

cold

57.

The graph is showing an ____________ reaction.

a)

exothermic

b)

endothermic

58.

The graph is showing an _________ reaction

a)

endothermic

b)

exothermic

59.

CO2 can be made using the following chemical equation:

2CO + O2 --> 2CO2

Find ΔHreaction\Delta H_{reaction}  if the heat of formation of CO is -99 kJ/mol and the heat of formation of CO2 is -393.5 kJ/mol.

a)

-589 kJ/mol

b)

589 kJ/mol

c)

294.5 kJ/mol

d)

-294.5 kJ/mol

60.

In our coffee cup calorimetry experiment, we dropped a piece of hot metal into cool water. The heat lost by the metal was ___________ the heat gained by the water.

a)

equal to

b)

greater than

c)

less than

61.

O2(g) + 2 H2 (g) → 2 H2O (g) + EnergyO_2\left(g\right)\ +\ 2\ H_2\ \left(g\right)\ \rightarrow\ 2\ H_2O\ \left(g\right)\ +\ Energy  

a)

endothermic

b)

exothermic

62.

6 CO2+ 6 H2O + Energy → C6H12O6 + 6 O26\ CO_2+\ 6\ H_2O\ +\ Energy\ \rightarrow\ C_6H_{12}O_6\ +\ 6\ O_2

a)

endothermic reaction

b)

exothermic reaction

63.

Describe the substance between letters C and D. 

a)

Gas

b)

Liquid

c)

Melting

d)

Evaporating

64.

Between which points is the temperature of the substance remaining constant?

a)

A-B only. 

b)

A-B, C-D, E-F

c)

B-C only. 

d)

B-C, D-E

65.

True or false: melting and freezing occur at the same temperature.

a)

True

b)

False

66.

Describe what is happening between letters D and E. 

a)

Gas

b)

Liquid

c)

Melting

d)

Evaporating

67.

Describe the substance between letters E and F. 

a)

Gas

b)

Liquid

c)

Melting

d)

Evaporating

68.

How do you calculate Enthalpy of a reaction?

a)

ΔH = ΔHproducts - ΔHreactants

b)

ΔT = q / mC

c)

ΔG = ΔH - TΔS

d)

E = mc2

69.

The SI unit of heat and energy is the ________.

a)

calorie

b)

heat

c)

joule

d)

watt

70.

Temperature is a measure of average [blank] energy of individual atoms.

a)

heat

b)

potential

c)

mechanical

d)

kinetic

71.

 _?_  is the amount of energy required to raise the temperature of 1 gram of any substance 1oC.

a)

Specific heat

b)

A calorie

c)

Thermal energy

d)

Conduction

72.

As 120 g of hot milk cools in a mug, it transfers 20,000 J of heat to the environment. What is the temperature change of the milk? The specific heat of milk is 2.6 J/g·°C. (Q=mcΔT)

a)

64 °C

b)

1.56 °C

c)

640 °C

d)

cannot be determined

73.

How much heat does an aluminum block absorb if 10.00 grams are heated from 25.0oC to 50.0oC? The specific heat of aluminum is 0.900J/goC

a)

450

b)

-450

c)

225

d)

-225

74.

____ reactions usually feel cold.

a)

endothermic

b)

exothermic

75.

During an endothermic reaction in a beaker if we are part of the surroundings and touched the beaker, it would feel _______. 

a)

Warm

b)

Cold

76-80.

Answer the questions below after watching the video

76.

What does molarity measure?

a)

The weight of solute per liter of solution

b)

The number of moles of solute per liter of solvent

c)

The density of the solution

d)

The volume of solvent per liter

77.

How can the molarity of a solution be determined if the mass of the solute is known?

a)

By measuring the density of the solution

b)

By dividing the mass by the volume of the solvent

c)

By multiplying the mass by the volume of the solution

d)

By converting the mass to moles using molar mass and dividing by the solution volume

78.

What is the effect of dilution on the concentration of a solution?

a)

Changes the molar mass of the solute

b)

Does not change the concentration

c)

Decreases the concentration

d)

Increases the concentration

79.

How is the new concentration after dilution calculated?

a)

By dividing the initial concentration by the final volume

b)

By subtracting the final volume from the initial concentration

c)

By multiplying the initial concentration by the initial volume and dividing by the final volume

d)

By adding the initial and final volumes

80.

What happens to the concentration of a solution if the volume is doubled?

a)

It doubles

b)

It remains the same

c)

It quadruples

d)

It is halved

81.

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

82.

A student is preparing solutions for a laboratory experiment by dissolving solid solutes in liquid solvents. Which action will increase the rate of solubility

a)

lowering the temperature of the solvent

b)

stirring the solute in the solution

c)

increasing the pressure on the solution

d)

increasing the particle size of the solute

83.

Which of the following substances is a heterogeneous substance?

a)

baby oil

b)

rocky road ice cream

c)

salt water

d)

milk

84.

Which of the following substances is a homogeneous solution?

a)

chocolate chip cookie

b)

italian dressing

c)

apple juice

d)

orange juice

85.

Which of the following is the correct formula for calculating molarity?

a)

moles/liters of solution

b)

moles/kg of solvent

c)

# particles/Avogadro's #

d)

theoretical yield/actual yield

86.

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

a)

supersaturated

b)

saturated

c)

unsaturated

87.

When calculating molality, Kg of the following are included in the calculation?

a)

solvent

b)

solute

c)

none of these

d)

solvent & solute

88.

To calculate molality you only need which of the following?

a)

scale

b)

flask

89.

What is the molality of a solution in which 3.0 moles of NaCl is dissolved in 1.5 Kg of water?

a)

2.0 M

b)

0.22 m

c)

135 m

d)

2.0m

90.

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

91.

The concentration of a mixture can be increased in which of the following ways?

a)

Heating the mixture

b)

Adding more water “solvent”

c)

Adding more powder “solute”

d)

Stirring the mixture

92.

air is a 

a)

compound

b)

element

c)

heterogeneous mixture

d)

solution

93.

Another name for a homogeneous mixture is 

a)

an element.

b)

a solution.

c)

a compound.

94.

If water is a polar molecule, then which of the following must be nonpolar

a)

sugar

b)

salt

c)

oil

d)

juice

95.

Electrolytes

a)

don't conduct electricity

b)

conduct electricity

96.

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

97.

Since "like dissolves like", water and oil will not mix because

a)

both of them are polar

b)

both of them are nonpolar

c)

oil is polar and water is nonpolar

d)

oil is nonpolar and water is polar

98.

What is the molarity of a 2 liter solution containing 5 moles of NaCl?

a)

5.0

b)

0.4

c)

2.5 moles/liter

d)

10 moles/liter

99.

How many liters would you need to get 0.5 moles if you had a 0.1M solution?

a)

0.05 liters

b)

0.2 liters

c)

5 liters

d)

2 liters

100.

Molarity is ...

a)

grams of solute/deciliters of solvent.

b)

grams of solute/liters of solution.

c)

moles of solute/liters of solution.

d)

moles of solute/milliliters of solvent.

101.

Which sweet tea would you expect to taste the sweetest?

a)

1M

b)

3M

c)

3.1M

d)

2.5M

102.

PV=nRT


If volume goes down, pressure goes _____.

a)

up

b)

down

103.

PV=nRT


If temperature goes up, pressure goes _____.

a)

up

b)

down

104.

What assumption is NOT made about ideal gases?

a)

The identity of the gas does not matter.

b)

Particles are in constant motion.

c)

Particles do not interact except during collisions.

d)

Particles have significant volume.

105.

What assumption is NOT made about ideal gases?

a)

The identity of the gas does not matter.

b)

Particles are in constant motion.

c)

Particles do not interact except during collisions.

d)

Particles have significant volume.

106.

What variable describes the force exerted by a gas on its container?

a)

Pressure

b)

Temperature

c)

Volume

d)

Moles

107.

According to Boyle's Law, what happens if the volume of a gas is decreased?

a)

Pressure decreases

b)

Temperature decreases

c)

Temperature increases

d)

Pressure increases

108.

What variable describes the force exerted by a gas on its container?

a)

Pressure

b)

Temperature

c)

Volume

d)

Moles

109.

What is directly proportional to volume according to Charles's Law?

a)

Pressure

b)

Temperature

c)

Moles

d)

Mass

110.

PV = nRT


If the temperature goes up, volume must go ____.

a)

up

b)

down

111.

What must be constant when applying Charles's Law?

a)

Mass

b)

Moles

c)

Pressure

d)

Volume

112.

According to Boyle's Law, what happens if the volume of a gas is decreased?

a)

Pressure decreases

b)

Temperature decreases

c)

Temperature increases

d)

Pressure increases

113.

What is the value of zero degrees Kelvin known as?

a)

Boiling point

b)

Freezing point

c)

Absolute zero

d)

Room temperature

114.

PV=nRT


If the number of moles (n) goes up, temperature must go ____.

a)

up

b)

down

115.

What does Avogadro's law state about equal volumes of gases?

a)

They have the same temperature.

b)

They exert the same force.

c)

They contain the same number of molecules.

d)

They have the same pressure.

116.

What is directly proportional to volume according to Charles's Law?

a)

Pressure

b)

Temperature

c)

Moles

d)

Mass

117.

What does the ideal gas law allow you to calculate?

a)

The pressure of a gas at any volume

b)

The number of moles of gas given pressure, volume, and temperature

c)

The temperature of a gas at any pressure

d)

The volume of a gas at any temperature

118.

What must be constant when applying Charles's Law?

a)

Mass

b)

Moles

c)

Pressure

d)

Volume

119.

What is the value of zero degrees Kelvin known as?

a)

Boiling point

b)

Freezing point

c)

Absolute zero

d)

Room temperature

120.
Neon occupies a volume of 2.80 L at -35°C. What volume will it occupy at 43°C?
a)
3.44 L
b)
4.1 L
c)
2.65 L
d)
3.7 L
121.

What does Avogadro's law state about equal volumes of gases?

a)

They have the same temperature.

b)

They exert the same force.

c)

They contain the same number of molecules.

d)

They have the same pressure.

122.
What is 50 C in Kelvin?
a)
223
b)
323
c)
100
d)
50
123.

What does the ideal gas law allow you to calculate?

a)

The pressure of a gas at any volume

b)

The number of moles of gas given pressure, volume, and temperature

c)

The temperature of a gas at any pressure

d)

The volume of a gas at any temperature

124.
Gas laws involve what three variables?
a)
Solid Liquid Gas 
b)
Speed Velocity Acceleration 
c)
Elements Compounds Mixtures 
d)
Pressure Temperature Volume 
125.
According to the Combined Gas Law, pressure and volume are inversely related which means that
a)
When pressure increases, volume increases
b)
When pressure decreases, volume decreases
c)
When pressure increases, volume decreases
d)
When pressure doubles, volume triples
126.
According to the Combined Gas Law, volume and temperature are directly related. This means that
a)
When volume increases, temperature increases
b)
When volume increases, temperature decreases
c)
When volume double, pressure triples
d)
When volume doubles, volume is reduced by 1/2
127.
If 6L of gas at 293K is compressed to 4L, what is the new temperature? 
a)
195K
b)
439.5K
c)
0.082K
d)
12.2K
128.
4L of a gas is contained at 300 kPa and 200K. What will its volume be in L at 140 kPa and 100K?
a)
4.3L
b)
4.8L
c)
6.2L
d)
8.5L
129.
Using Combined Gas Law, if the pressure of a gas starts out at 200kPa and increases to 600kPa, what would the initial temperature be if it ended up at 300K?
a)
50K
b)
200K
c)
400K
d)
100K
130.
The energy of an object as it is in motion is defined as
a)
Kinetic Theory
b)
Kinetic energy
c)
Potential energy
d)
Electric energy
131.
When a cold tire is inflated to a certain pressure and then is warmed up due to friction with the road, the pressure increases. This happens because the
a)
air molecules hit the walls of the tire less frequently
b)
rubber in the tires reacts with oxygen in the atmosphere
c)
air molecules speed up and collide with the tire walls more often
d)
air molecules diffuse rapidly through the walls of the tire.
132.

If the pressure in a balloon remains constant what happens to the balloon's volume as the temperature of the air increases?

a)

the volume decreases and the balloon shrivels up or shrinks

b)

the volume increases and the balloon expands

c)

the volume stays the same and the balloon stays the same size

133.

Each of the flasks shown above have different volumes (they are different sizes) but the temperature of each flask is the same. In which flask will the pressure be the highest?

a)

Flask 1

b)

Flask 2

c)

Flask 3

d)

Flask 4

134.

Which equation would you use to solve the following problem:

"The volume of of 300 mL of gas at 1 atm is decreased to 100 mL. What is the new pressure?"

a)

P1V1 = P2V2

b)

V1/T1 = V2/T2

c)

(P1V1)/T1 = (P2V2)/T2

d)

None of the above

135.

Which equation would you use to solve the following problem:

"A gas occupies 2 L of space at 0 C. What will its volume be at 100 C?"

a)

P1V1 = P2V2

b)

V1/T1 = V2/T2

c)

(P1V1)/T1 = (P2V2)/T2

d)

None of the above

136.

A tank of helium is full with a pressure of 4.5 atm at 298K. What is the temperature of the tank when the pressure drops to 2 atm?

a)

670.5K

b)

0.007K

c)

132.4K

d)

2682K

137.

1.70 atm, a sample of gas takes up 4.25L. If the pressure in the gas is increased to 2.40 atm, what will the new volume be?

a)

0.167 L

b)

6.00 L

c)

3.01 L

d)

0.332 L

138.

Which of the following is an assumption of the kinetic-molecular theory of gases?

a)

Collisions between gas particles are inelastic.

b)

Gases consist of closely spaced particles.

c)

Gas particles move around in an orderly manner.

d)

The temperature of a gas depends on the average kinetic energy of the gas particles.

139.

A student sprays perfume in the back of the classroom, eventually a student in the front of the class can smell the perfume. This is an example of....

a)

Effusion

b)

Diffusion

c)

Osmosis

d)

Thermal Expansion

140.

A container with a volume if 1.0 L is occupied by a gas at a pressure of 1.5 atm at 25°C. By changing the volume, the pressure of the gas increases to 6.0 atm as the temp is raised to 100.°C. What’s the new volume?

a)

1.45 L

b)

5.4 L

c)

0. 31 L

d)

504.7 L

141.

The pressure in an automobile tire is 2.3 atm at 27°C. At the end of a journey on a hot, sunny day the pressure has risen to 2.6 atm. What is the temp of the air in the time assuming the volume has not changed?

a)

60 K

b)

650 K

c)

273 C

d)

339 K

142.

What is the molar mass of Cl2?

a)

17 g/mol

b)

35.5 g/mo;

c)

71.0 g/mol

d)

89 g/mol

143.

In a chemical reaction, the mass of reactants ___.

a)

is less than the mass of products

b)

is greater than the mass of products

c)

has no relationship to the mass of products

d)

is equal to the mass of products

144.

What is the molar mass of C6H12O6?

a)

180.15

b)

180.36

c)

180.00

d)

180.06

145.

This recipe makes 3 dozen cookies. How many eggs are needed to make 3 dozen cookies?

a)

2 eggs

b)

1 teaspoon vanilla extract

c)

1 cup butter

d)

2 cups semisweet chocolate chips

e)

1 cup packed brown sugar

146.

How much butter is needed for 2 cups of chocolate chips?

a)

2 eggs

b)

1 teaspoon vanilla extract

c)

1 cup butter

d)

2 cups semisweet chocolate chips

e)

1 cup packed brown sugar

147.

How many eggs would we need to make 9 dozen cookies? (This recipie makes 3 dozen)

a)

6 eggs

b)

5 eggs

c)

4 eggs

d)

2 eggs

e)

1 egg

148.

How much brown sugar would I need if I had ½ cup white sugar?

a)

2 eggs

b)

1 teaspoon vanilla extract

c)

1 cup butter

d)

2 cups semisweet chocolate chips

e)

1 cup packed brown sugar

149.

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

How many moles of Aluminum oxide do you have if you have 2 moles of Al?

a)

3 mole

b)

2 mole

c)

1 mole

d)

0.5 mole

150.

In the equation 2 Al2O3 --> 4 Al + 3 O2, what is the mole ratio of aluminum to oxygen?

a)

10:6

b)

3:4

c)

4:3

d)

2:3

151.

N2 + 3H2 → 2NH3

What is the mole ratio between Nitrogen and Ammonium in the above reaction?

a)

1 moles NH3 / 2 moles N2

b)

2 moles NH3 / 1 moles N2

c)

2 moles N2 / 3 moles NH3

d)

1 moles N2 / 3 moles NH3

152.
_BaS + _PtF2 → _BaF2 + _PtS
a)
1 BaS + 1 PtF2 → 1 BaF2 + 1 PtS
b)
4 BaS + 2 PtF2 → 1 BaF2 +  1 PtS
c)
1 BaS + 2 PtF2→ 2 BaF2 +  2 PtS
d)
1 BaS + 3 PtF2 →1 BaF2 +  2 PtS
153.
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
154.

How many moles are in 32 grams of Oxygen (O)?

a)

3

b)

2

c)

1

d)

4

155.

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

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

a)

15

b)

18

c)

20

d)

24

156.

Using the following equation:

Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)

How many moles of iron (Fe) can be made from 6 moles H2?

a)

4 moles Fe

b)

6 moles Fe

c)

9 moles Fe

d)

2 moles Fe

157.

All alkali metals react with water to produce hydrogen gas and the corresponding alkaline metal hydroxide. A typical reaction is that between lithium and water :

2Li(s) + 2H2O(l) →2LiOH(aq) + H2(g)

Calculate the mass of H2 gas formed when 40.0 g of Li react with water

a)

4.21 g

b)

7.31 g

c)

5.80 g

d)

4.42 g

158.
A formula with the lowest whole # ratio of elements in a compound is called
a)
Molecular Formula
b)
Chemical Formula
c)
Empirical Formula 
d)
Distance Formula
159.

What is the empirical formula for C4H6?

a)

CH

b)

CH3

c)

C2H3

d)

C4H6

160.

What is the empirical formula for N2S3?

a)

NS

b)

N3S2

c)

N2S3

d)

N1S1.5

161.

Si2F6

Choose the correct empirical formula...

a)

SiF

b)

Si2F6

c)

SiF3

d)

Si6F2

162.

C2F6

Choose the correct empirical formula...

a)

CF

b)

C2F6

c)

C6F2

d)

CF3

163.
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.
164.
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
165.
A chemical formula that shows the actual # and kinds of atoms present in one molecule of a compound is called_________
a)
ionic formula
b)
covalent formula
c)
empirical formula
d)
molecular formula
166.

C2H6O

Which is the correct empirical formula

a)

CHO

b)

C2H6O

c)

C4H14O2

d)

None

167.

How many "C" are in CO2

a)

2

b)

1

c)

0

d)

3

168.

How many Carbons "C" are in C18H34O3

a)

18

b)

34

c)

3

d)

37

169.

Which molecular formula only has 12 hydrogens "H"?

a)

C4H10 (butane)

b)

C5H12 (pentane)

c)

C12H22O11 (sugar)

d)

C8H10N4O2 (caffeine)

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