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Chemistry Semester 2 Final Revu

Total questions: 93

Worksheet time: 4hrs 41mins

Name
Class
Date
1.

For the reaction...
SO2(g) + O2(g) <−>  SO3(g)
If the concentration of SO2(g)  is increased, the equilibrium of the reaction will ___________.

a)

shift to the left

b)

shift to the right

c)

not shift

2.

For the reaction...
energy +  N2(g)  +  O2(g)  <−>  2NO(g)
If  O2(g) is removed, the  concentration of N2 will _______.

a)

increase

b)

decrease

c)

remain the same

d)

double

3.

For the reaction...
heat  +  N2(g)  +  O2(g)  <−>  2NO(g)
If the heat is removed to the chemical system, the equilibrium will _______.

a)

shift to the left

b)

shift to the right

c)

not shift

4.

For the reaction...
N2 (g) +  3 H2 (g) <−> 2 NH3 (g)

If the pressure in the system is increased,  which substance will increase in concentration?

a)

N2

b)

H2

c)

N2 and H2

d)

NH3

5.

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 are equal

b)

Forward and reverse reaction rates are equal and concentrations are constant

c)

Forward and reverse reaction rates are equal and concentrations are equal

d)

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

6.

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.

7.

How does a catalyst affect a reaction at equilibrium?

a)

It makes the reaction shift right

b)

It makes the reaction shift left

c)

It doesn't affect the equilibrium position

8.

As a reaction proceeds, the concentration of reactants will _______ and the concentration of products will ________.

a)

increase, decrease

b)

increase, increase

c)

decrease, decrease

d)

decrease, increase

9.

Why does a catalyst increase the rate of reaction?

a)

it produces extra energy for the reactants

b)

it increases the speed of the reactant particles

c)

it increases the frequency of particle collisions

d)

it reduces the activation energy of the reaction 

10.

Which of the following increase the reaction rate?

a)

less surface area

b)

lower temperature

c)

an inhibitor

d)

increased concentration

11.

Why don't all collisions between particles cause a reaction? (Select 2 answers)

a)

the particles also need to collide with a catalyst

b)

not all the particles collide with enough energy

c)

not all the particles collide at a high enough temperature

d)

the particles need to collide with the right orientation

12.

Why does a higher temperature increase the rate of a reaction?

a)

it increases both the frequency and energy of particle collisions

b)

it only increases the frequency of particle collisions

c)

it only increases the energy of particle collisions

d)

it reduces the activation energy of the reaction

13.

Which has more surface area?

a)

Large chunks of chalk

b)

Cube of sugar

c)

Powdered sugar

d)

Small chunks of sugar

14.

Why does a higher concentration increase the rate of reaction?

a)

it increases the amount of reactants

b)

it lowers the activation energy

c)

it increases the energy of particle collisions

d)

it increases the frequency of particle collisions

15.

Exothermic reactions...

a)

Absorb energy

b)

Release energy

c)

Release Color

d)

Absorb Color

16.

Have you ever eaten sherbet sweets candy? They fizz in your mouth and your tongue feels cold. Why do you think that is?

a)

It is an exothermic reaction

b)

It is an endothermic reaction

c)

It is made of ice

d)

It is dissolving your mouth

17.

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

18.

If a chemical reaction is EXOTHERMIC, the temperature of the surroundings would....

a)

Stay the same

b)

Increase

c)

Decrease

19.

Is photosenthysis an Exothermic or an Endothermic reaction?

a)

Endothermic

b)

Exothermic

20.

What energy is stored and waiting to be used?

a)

Kinetic Energy

b)

Potential Energy

21.

Boyle's PV law : When _______ is held constant, the pressure and volume of a gas are ________ proportional

a)

temperature, equally

b)

temperature, inversely

c)

mass, equally

d)

mass, inversely

22.

Pressure is

a)

defined as the mass that an object exerts when at rest.

b)

not a measurable in gases.

c)

defined as the number of moles of substance divided by the mass of the substance.

d)

created by the force of the gas particles impacting the walls of the container.

23.

When the temperature of matter increases the particles...

a)

speed up and move closer

b)

speed up and move farther apart

c)

slow down and move closer together

d)

slow down and move farther apart

24.

Which of the following would increase the (gas) pressure of a system?

a)

Increase the Temperature

b)

Pump in more gas

c)

Decrease the volume

d)

All of these

25.

In order to convert to Kelvin, you add ______ to the Celsius measurement.

a)

372

b)

273

c)

237

d)

732

26.

If I initially have 4.0 L of a gas at a pressure of 1.1 atm, what will the volume be if I increase the pressure to 3.4 atm?

a)

1.29 L

b)

12.36 L

c)

1.29 atm

d)

12.36 atm

27.

A sample of sulfur dioxide occupies a volume of 652 mL at 313 K and 150 kPa. What volume will the sulfur dioxide occupy at STP?


STP = 273 K, 101.3 kPa

a)

1682.6 mL

b)

20.7 mL

c)

492.3 mL

d)

842.1 mL

28.

Solve the following problem:

What is the volume of a balloon if it contains 3.2 moles of helium at a temperature of 20⁰C and 1.2 atm? (Use PV = nRT, with R = .0821 L atm/mol K)

a)

106.55 K

b)

53.3 L

c)

293 K

d)

64.15 L

29.

Which type of ion does a base produce when it is dissolved in water?

a)

oxide, O2-

b)

hydronium, H3O+

c)

proton, H+

d)

hydroxide, OH-

30.

Which type of ion does an acid produce when it is dissolved in water?

a)

oxide, O2-

b)

oxygen, O

c)

hydronium, H3O+

d)

hydroxide, OH-

31.

A neutral substance would have pH of...

a)

8

b)

7

c)

6

d)

14

32.

An extremely strong base would have a pH of...

a)

1

b)

7

c)

9

d)

14

33.

A weak base would have a pH of...

a)

8

b)

7

c)

6

d)

14

34.

An extremely strong acid would have a pH of...

a)

1

b)

7

c)

9

d)

14

35.

A weak acid would have a pH of...

a)

1

b)

7

c)

6

d)

14

36.

Which of the following is true about acids and bases?

a)

The lower the pH, the higher the concentration of H+ (H3O+)

b)

the higher the pH, the higher the concentration of H+ (H3O+)

c)

The lower the pH, the more neutral the solution

d)

The higher the pH, the weaker the base

37.

Which one of the following statements about strong acids is TRUE?

a)

Strong acids are 100% ionized in water.

b)

The conjugate base of a strong acid is a strong base.

c)

Strong acids are very concentrated acids.

d)

Strong acids produce solutions with a higher pH than weak acids. 

38.

Conducts electricity (has electrolytes)

a)

acid

b)

base

c)

both an acid and a base

39.

When electrons are shared a ________ bond is formed

a)

Ionic

b)

Covalent

c)

Metallic

40.

Which part of the atom is responsible for chemical bonding?

a)

Core Electrons

b)

Valence Electrons

c)

Protons

d)

Neutrons

41.

A ____________ bond exists between a metal and a nonmetal.

a)

Ionic

b)

Covalent

42.

Metals form ions by _____________ electrons, nonmetals form ions by   ___________ electrons. 

a)

losing, gaining

b)

gaining, losing

c)

 losing, losing

d)

gaining, gaining

43.

Which of the following statements is correct? 

a)

Metals tend to gain electrons and become positive. 

b)

Metals tend to lose electrons and become negative.

c)

Metals tend to lose electrons and become positive

d)

Metals tend to gain electrons and become negative.

44.

How many valence electrons do most atoms need to have a complete outer shell and be energetically stable?

a)

1

b)

8

c)

10

d)

5

45.

Ionic Bonding involves...

a)

The transfer of protons

b)

The transfer of nuetrons 

c)

The transfer of electrons

d)

None Of the above

46.

Covalent compounds

a)

Share electrons

b)

transfer electrons

c)

contain a sea of electrons

d)

conduct electricity

47.

Predict the bond that will form between Be and F.

a)

Ionic

b)

Covalent

48.

Predict the bond that will form between Se and Cl.

a)

Ionic

b)

Covalent

49.

What is the correct Lewis Dot Structure for NH3, and how many bonds does the N atom form in this compound?

a)

5 bonds

5 bonds

b)

3 bonds

3 bonds

c)

3 bonds

3 bonds

d)

4 bonds

4 bonds

50.

Which is the correct molecular structure for carbon dioxide CO2?

a)
b)
c)
d)
51.

H2O has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

52.

Click on all the properties of Ionic Bonds.

a)

Brittle

b)

High Melting Point

c)

Hard

d)

Conducts electricity when dissolved in water

e)

Conducts electricity when melted (molten)

53.

Check all properties of covalent bonds.

a)

Low Melting Points

b)

Do not conduct electricity

c)

Generally softer

d)

Shares electrons

54.

Electronegativity (a)   as you go down a group.

55.

What does electronegativity do as you go across a period?

a)

decrease

b)

no pattern

c)

stay the same

d)

increase

56.

Do noble gases have electronegativity values?

a)

yes

b)

no

57.

A neutral atom of Fluorine has 9 protons and 9 electrons. Gaining an electron would turn fluorine into ​ (a)   and would ​ (b)   because the ​ (c)   ​ between electrons have increased.

Choose from the below words

an ion

increase its radius

repulsive forces

an isotope

a new element

decrease its radius

attractive forces

58.

Which is smaller?

a)

NaNa

b)

Na+Na^+

59.

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

60.

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

61.

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

62.

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

63.

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

64.

Balance this equation:

​ (a)   Fe + ​ (b)   O2 --> ​ (c)   Fe2O3

Choose from the below words

4

3

2

1

0

65.

Balance this equation:

​ (a)   FeCl2 + ​ (b)   Cl2 --> ​ (c)   FeCl3

Choose from the below words

2

1

3

4

66.

Balance this equation:

​ (a)   CH4 + ​ (b)   O2 --> ​ (c)   CO2 + ​ (d)   H2O

Choose from the below words

2

1

3

4

1
2
67.

How many moles are in 3.01 x 1022 atoms of magnesium? (atoms to moles = divide by 6.02 x 10^23)

a)

0.05 moles

b)

1.81 x 1046 moles

c)

5.00 x 1021 moles

d)

5 moles

68.

What is the mass of 0.89 mol of CaCl2?

a)

111 grams

b)

0.008 grams

c)

98.9 grams

d)

67.22 grams

69.

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

70.

What is the transfer of heat by movement of liquids or gases?

a)

Radiation

b)

Convection

c)

Conduction

d)

Heat

71.

What is a transfer of heat energy by electromagnetic waves?

a)

Radiation

b)

Convection

c)

Conduction

d)

Heat

72.

What is the transfer of heat by direct contact?

a)

Convection

b)

Electromagnetic waves

c)

Radiation

d)

Conduction

73.

Hot coffee is stirred with a spoon; the spoon gets hot due to __________.

a)

conduction

b)

convection

c)

radiation

74.

Near the ceiling of a room the air is warmer; the warm air rises because of __________.

a)

conduction

b)

convection

c)

radiation

75.

Carole owns a two story house with a heating and cooling unit on each floor. In the winter she mostly uses the downstairs unit to heat the house because the volume of warm air __________ and __________, warming the whole house through __________.

a)

expands and rises, convection

b)

expands and sinks, conduction

c)

contracts and rises, conversion

d)

contracts and sinks, conduction

76.

In heat transfer, heat always flows from the _______________ substance to the _______________ substance.

a)

warmer, cooler

b)

cooler, warmer

77.

If two objects have different temperatures, 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

78.

Which of the following is the best example of radiation?

a)

The ocean breeze

b)

The sun heating your body on the beach

c)

Eating ice cream

d)

A wave knocking over a sandcastle

79.

As water in a freezer turns into ice, ___________.

a)

the water absorbs energy from the air in the freezer.

b)

the water absorbs the coldness from the air in the freezer.

c)

the freezer air absorbs heat from the water.

d)

the water neither absorbs nor releases energy

80.

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

81.

What is the specific heat of an unknown substance if 100.0 g of it at 200.0 °C reaches an equilibrium temperature of 27.1 °C when it comes in contact with a calorimeter of water.  The water weighs 75. g and had an initial temperature of 20.00 °C?  (Specific heat of water is 4.18 J/g°C) (show your work)

a)

0.111 J/g°C

b)

1.29 J/g°C

c)

0.129 J/g°C

d)

22225.85 J

82.

The specific heat of aluminum is 0.21 cal/g°C.  How much heat(Q) is released when a 10 g piece of aluminum foil is taken out of the oven and cools from 100° to 50°?

a)

105 J

b)

10.5 J

c)

1.05 J

d)

50 J

83.

Which line segment represents the substance only in the solid state?

a)

AB‾\overline{AB}  

b)

BC‾\overline{BC}  

c)

CD‾\overline{CD}  

d)

DE‾\overline{DE}  

84.

Select all line segments in which the temperature stays constant.

a)

AB‾\overline{AB}  

b)

BC‾\overline{BC}  

c)

CD‾\overline{CD}  

d)

DE‾\overline{DE}  

e)

EF‾\overline{EF}  

85.

What is the boiling point of this substance?

a)

100 oC

b)

60 oC

c)

-60 oC

d)

20 oC

86.

What can be concluded by comparing the lengths of the melting and boiling lines?

a)

It takes more energy to vaporize the sample than it does to melt it.

b)

It takes more energy to increase the temperature of the gas than the liquid.

c)

The substance stays at the boiling point for a short time.

d)

The substance prefers the gas phase over the other phases.

87.

Look at the slopes at each part of the graph. What can be concluded by comparing the slope of heating the liquid (water) versus that of the slope for ice or steam? (Choose all correct answers.)

a)

More energy is required to heat up water than it does to heat up ice or steam.

b)

Less energy is required to heat up water than it does to heat up ice or steam.

c)

cwater > cice and cwater > csteam

d)

cwater < cice and cwater < csteam

88.

Select all line segments in which the temperature is changing.

a)

AB‾\overline{AB}  

b)

BC‾\overline{BC}  

c)

CD‾\overline{CD}  

d)

DE‾\overline{DE}  

e)

EF‾\overline{EF}  

89.

Which line segment represents the heat of fusion (ΔHfus)?

a)

AB‾\overline{AB}  

b)

BC‾\overline{BC}  

c)

CD‾\overline{CD}  

d)

DE‾\overline{DE}  

e)

EF‾\overline{EF}  

90.

Which line segment represents the heat of vaporization (ΔHvap)?

a)

AB‾\overline{AB}  

b)

BC‾\overline{BC}  

c)

CD‾\overline{CD}  

d)

DE‾\overline{DE}  

e)

EF‾\overline{EF}  

91.

Select all line segments in which the kinetic energy is changing.

a)

AB‾\overline{AB}  

b)

BC‾\overline{BC}  

c)

CD‾\overline{CD}  

d)

DE‾\overline{DE}  

e)

EF‾\overline{EF}  

92.

Select all line segments in which the potential energy is changing.

a)

AB‾\overline{AB}  

b)

BC‾\overline{BC}  

c)

CD‾\overline{CD}  

d)

DE‾\overline{DE}  

e)

EF‾\overline{EF}  

93.

Select all line segments in there are phase changes.

a)

AB‾\overline{AB}  

b)

BC‾\overline{BC}  

c)

CD‾\overline{CD}  

d)

DE‾\overline{DE}  

e)

EF‾\overline{EF}  

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