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Honors Chemistry Semester 2 Exam Review

Total questions: 114

Worksheet time: 2hrs 55mins

Name
Class
Date
1.

The average kinetic energy of the particles in a sample of matter is measured as the —

a)

kinetic force

b)

thermal rate

c)

reaction rate

d)

temperature

2.

What type of energy is stored in chemical bonds?

a)

Chemical potential energy

b)

Thermal potential energy

c)

Chemical kinetic energy

d)

Thermal kinetic energy

3.

The more kinetic energy there is in a sample of matter, the —

a)

more energy is absorbed as heat

b)

more energy is given off as heat

c)

lower the temperature

d)

higher the temperature

4.

Calculate the heat transferred when 440 g of water cools from 87.2°C to 50.0°C. (C = 4.18 J/g°C)

a)

68000 J

b)

2.83 J

c)

-2.83 J

d)

-68000 J

5.

If 238 J of heat is absorbed by a sample of metal with a mass of 40.7 g, and it raises the temperature from 20.0°C to 32.4°C, what is the specific heat capacity of the metal?

a)

2.34 J/g°C

b)

0.472 J/g°C

c)

6.13 J/g°C

d)

0.163 J/g°C

6.

A sample of iron receives 50.J of heat energy that raises the temperature of the iron 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
7.

If a reaction is endothermic, which statement below best describes the energy of the products and reactants in the reaction?

a)

Energy is given off during the reaction, making the energy of the products greater than the energy of the reactants.

b)

Energy is given off during the reaction, making the energy of the reactants greater than the energy of the products.

c)

Energy is absorbed during the reaction, making the energy of the reactants greater than the energy of the products.

d)

Energy is absorbed during the reaction, making the energy of the products greater than the energy of the reactants.

8.
∆H is positive
a)
endothermic
b)
exothermic
9.
The products contain more energy than the reactants
a)
endothermic
b)
exothermic
10.
Exothermic reactions are reactions that
a)
release heat
b)
do not involve heat
c)
absorb heat
d)
take place instantaneously
11.

If the enthalpy change (ΔH) is negative the reaction is ____.

a)

Endothermic

b)

Exothermic

c)

Neutral

12.
H2 + ½ O2 --> H2O + 285kJ is an example of a(n)
a)
Electrical equation
b)
Heat equation
c)
Thermochemical equation
13.
If ΔH is positive, heat would be shown on the _____ side of the thermochemical equation.
a)
Reactant
b)
Product
14.
C+ O2 --> CO2 + 60kJ, what is the value for ΔH for the reaction?
a)
+60
b)
-60
c)
there is no way to know
15.

The diagram shows  that the reaction is ___________ and the enthalpy change is __________.

a)

endothermic, negative

b)

exothermic, negative

c)

endothermic, positive

d)

exothermic, positive

16.

Calculate the enthalpy of the following reaction: CaCO3 (s) --> CO2(g) + CaO(s)

a)

178.3 kJ

b)

-178.3 kJ

c)

-2235.5 kJ

d)

2235.5 kJ

17.

Enthalpy occurs when chemical reactions use energy to form or break bonds. In general, distinguish how heat energy is related to enthalpy in a chemical reaction. In a reaction —

a)

heat energy is released

b)

heat energy is absorbed

c)

heat energy changes

d)

heat energy is conserved

18.

The diagram shows that the reaction is ___________ and the enthalpy change is __________.

a)

endothermic, negative

b)

exothermic, negative

c)

endothermic, positive

d)

exothermic, positive

19.

The reactants contain more energy than the products

a)

endothermic

b)

exothermic

20.

If a reaction is exothermic, which statement below best describes the energy of the products and reactants in the reaction?

a)

Energy is given off during the reaction, making the energy of the products greater than the energy of the reactants.

b)

Energy is given off during the reaction, making the energy of the reactants greater than the energy of the products.

c)

Energy is absorbed during the reaction, making the energy of the reactants greater than the energy of the products.

d)

Energy is absorbed during the reaction, making the energy of the products greater than the energy of the reactants.

21.

If a reaction is performed in a calorimeter, and the temperature inside the calorimeter decreases, which statement best describes the reaction?

a)

The reaction is endothermic because heat is being absorbed by the reaction.

b)

The reaction is exothermic because heat is being released by the reaction.

22.

If a reaction is performed in a calorimeter, and the temperature inside the calorimeter increases, which statement best describes the reaction?

a)

The reaction is endothermic because heat is being absorbed by the reaction.

b)

The reaction is exothermic because heat is being released by the reaction.

23.
Which has a pH below 7?
a)
Acid
b)
Base
24.
Which has a pH above 7?
a)
Acid
b)
Base
25.
Which has a bitter taste?
a)
Base
b)
Acid
c)
flagella
d)
cila
26.
Which of the following statements about acids is true?
a)
They taste sweet.
b)
They taste sour.
c)
They have a pH between 8-14.
27.
What is the pH of water?
a)
11
b)
4
c)
7
28.
Which has a slippery texture?
a)
Acid
b)
Base
29.
Turns litmus red
a)
Acids
b)
Bases
c)
All
30.
Turns litmus blue.
a)
Acids
b)
Bases
c)
Salts
d)
All
31.
Which is the stronger acid?
a)
pH 1
b)
pH 4
c)
pH 8
d)
pH 13
32.
Which range of numbers represent basic solution?
a)
0-6
b)
7
c)
8-14
d)
3-9
33.
A solution with a pH of 7 is________
a)
increasing
b)
neutral
c)
decreasing
d)
apple juice
34.
Acids react with
a)
water to produce bases and salts
b)
salts to produce bases and water
c)
neither bases, salts nor water
d)
bases to produce salts and water
35.

A substance is found to have the following characteristics:


Very bitter taste

Feels slippery to the touch

Produces OH- ions when dissolved in water


In what category would the substance be classified?

a)

acid

b)

base

c)

enzyme

d)

fatty acid

36.

HF is...

a)

an acid

b)

a base

c)

a salt

d)

an ionic compound

37.

Releases hydrogen in an aqueous solution.

a)

Arrhenius base

b)

Bronsted-Lowry base

c)

Arrhenius acid

d)

Bronsted-Lowry acid

38.

KOH is ...

a)

an acid

b)

a base

c)

a salt

d)

an ionic compound

39.

What is the pH of a solution where the [H+] is 1.0 x 10-11?

a)

11

b)

13

c)

14

d)

1

40.

What is the [H+] if the pH is 4.0?

a)

1.0 x 10-10 M

b)

1.0 x 10-4 M

c)

1.0 x 10-14 M

d)

1.0 x 10-7 M

41.

What completely ionizes in solution?

a)

Weak acids

b)

Strong acids

c)

Strong Salts

d)

Neutral salts

42.

Milk is a very weak acid. What might its pH value be?

a)

6.5

b)

7.8

c)

4.2

d)

12.2

43.

The higher the concentration of negative (hydroxide) ions in the solution, the stronger the base is.

a)

True

b)

False

44.

Which of the following pH values represents a base?

a)

2.1

b)

4.6

c)

6.8

d)

8.1

45.

The strongest bases have pH values close to

a)

0

b)

14

c)

7

d)

5

46.

Releases hydroxide ions in an aqueous solution.

a)

Arrhenius base

b)

Bronsted-Lowry base

c)

Arrhenius acid

d)

Bronsted-Lowry acid

47.

Donates protons (hydrogen ions)

a)

Arrhenius base

b)

Bronsted-Lowry base

c)

Arrhenius acid

d)

Bronsted-Lowry acid

48.

Accepts protons (hydrogen ions)

a)

Arrhenius base

b)

Bronsted-Lowry base

c)

Arrhenius acid

d)

Bronsted-Lowry acid

49.

A researcher is trying to conduct an experiment that requires a solution with a high concentration of hydronium ions. There are several solutions in the stock room they can choose from, which includes two bottles of hydrochloric acid and two bottles of acetic acid with varying molarities. Hydrochloric acid is a strong acid, and acetic acid is a weak acid.


Which of the following solutions would have the highest concentration of hydronium ion (H3O+)?

a)

1x10-5 M HCl

b)

1x10-5 M HCH3COO

c)

1.0 M HCl

d)

1.0 M HCH3COO

50.

Which of the following are true about strong acids?

a)

They are strong electrolytes

b)

They dissociate completely in solution

c)

They lose their protons more easily

d)

All of the above

51.

What does pH measure?

a)

Electron concentration

b)

Neutron concentration

c)

Hydroxide ion concentration

d)

Hydrogen ion concentration

52.

For two acids of equal concentration, the stronger acid has — 

a)

a higher concentration of hydroxide ions

b)

a higher pH

c)

a higher concentration of hydrogen ions

d)

a stronger bond

53.

Students are testing the strengths of two unknown acidic solutions with the same molarity. They examine the strengths of their solutions with a conductivity probe made from a circuit and exposed electrodes of a light bulb. The students place the electrodes into each solution and observe the brightness of the bulb. Their observations are recorded in the data table. The brightness of the bulb is based on the number of dissociated ions in the corresponding solution. Which solution from the data table above most likely contains a strong acid?

a)

Solution 1 is a strong acid due to a large number of dissociated ions.

b)

Solution 1 is a strong acid due to a small number of dissociated ions.

c)

Solution 2 is a strong acid due to a large number of dissociated ions.

d)

Solution 2 is a strong acid due to a small number of dissociated ions.

54.

Predict the missing product in the acid-base reaction. 

HCl + NaOH → H2O + ______

a)

HNa

b)

ClOH

c)

NaCl

d)

CO2

55.

When nitric acid is dissolved into ammonia, the ammonia will accept the hydrogen to create ammonium.

HNO3(aq) + NH3 → NH4+(aq) + NO3-(aq)

What type of acid is nitric acid?

a)

Arrhenius base

b)

Bronsted-Lowry acid

c)

Arrhenius acid

d)

Bronsted-Lowry base

56.

Potassium hydroxide dissociates in water to produce hydroxide ions.

 KOH(s) +H2O(l) → K+(aq) + OH-(aq)

Given the information above, how is potassium hydroxide categorized?

a)

Both a Bronsted-Lowry base and an Arrhenius base

b)

An Arrhenius base but not a Bronsted-Lowry base

c)

Neither an Arrhenius base nor a Bronsted-Lowry base

d)

A Bronsted-Lowry base but not an Arrhenius base

57.

What is the pH of a solution with a hydrogen ion concentration of 1.3 x 10-11 M?

a)

11.1

b)

10.9

c)

1.3

d)

0.11

58.

A sample of fruit juice is found to have a hydrogen ion concentration of 2.87 x 10-4 M. What would the pH be?

a)

2.87

b)

3.54

c)

4.58

d)

8.16

59.

The dissolved substance is called the:

a)

solvent

b)

solute

c)

neither of the above

d)

all of the above

60.

Electrolytes are solutions that:

a)

conduct electricity

b)

do not conduct electricity

c)

are insulators

d)

none of the above

61.

True or False: Like dissolves like is a good rule of thumb to predict the solubility of substances.

a)

True

b)

False

62.

Pressure causes the solubility of a gas to:

a)

increase

b)

decrease

c)

none of the above

63.

True or False: Water is a universal solvent because of its polarity.

a)

True

b)

False

64.
In the above picture, a powder is about to be poured into the liquid. Which of the following should be done to make this powder dissolve faster?

a)
stir the powder in the liquid
b)
freeze the mixture
c)
add more powder to the liquid
d)
store the mixture in a dark place
65.
When a certain amount of solvent cannot hold any more solute it is called a ________ solution.
a)
Diluted
b)
Saturated
66.
Solution where more solute can still be dissolved at the given temperature. 
a)
Saturated
b)
Unsaturated
c)
Supersaturated
d)
Homogeneous solution
67.
Which solute is the most soluble at 10 ⁰C?
a)
KI
b)
KClO3
c)
NH4Cl
d)
NH3
68.

According to the solubility curve, how many grams of SO2 is needed to produce a saturated solution at 50 ⁰C?

a)
5 g
b)
10 g
c)
20 g
d)
39 g
69.

According to the graph above, which salt has a solubility curve which resembles the behavior of gasses in solution?

a)
Ce2(SO4)3
b)
KClO3
c)
 K2Cr2O7
d)
KNO3
70.
This solution would be considered
a)
Unsaturated
b)
Supersaturated
c)
Saturated
d)
Undefined
71.
This graph represents a(n) ___ solution
a)
saturated
b)
supersaturated
c)
unsaturated
d)
undefined
72.

What will happen to the ability of a gas to dissolve in a liquid if the temperature increases?

a)

solubility of the gas increases

b)

solubility of the gas decreases

c)

solubility of the gas is not affected

d)

Solubility of the gas increases or decreases

73.

If I make a solution by adding water to 27.72 g of methanol (CH3OH) until the final volume of the solution is 275 mL, what is the molarity of methanol in this solution?

a)

5.66 M CH3OH

b)

3.13 M CH3OH

c)

0.77 M CH3OH

d)

2.19 M CH3OH

74.

What is the molarity of a solution in which 0.45 g of sodium nitrate is dissolved in 265 mL of solution

a)

1.70 M NaNO3

b)

0.76 M NaNO3

c)

0.02 M NaNO3

d)

2.55 M NaNO3

75.
How many L of a 14 M stock solution must beused to make 250 mL of a 1.75 M solution? M1V1=M2V2
a)
0.031 L
b)
31.3 L
c)
2000 L
d)
10.2 L
76.

How many moles of solution will result when 15.0 L of H2SO4 is used to make a 0.20 M solution?

a)
75 moles
b)
7 moles
c)
3 moles
d)
0.013 moles
77.
You place electrodes in a solution and this happens! The solution must be:
a)
nonelectrolyte & covalent bond
b)
nonelectrolyte & ionic bond
c)
electrolyte & covalent bond
d)
electrolyte & ionic bond
78.
You place electrodes in a solution and this happens! This solution must be:
a)
electrolyte & ionic bond
b)
electrolyte & covalent bond
c)
nonelectrolyte & ionic bond
d)
nonelectrolyte & ionic bond
79.

Which of the following compounds is soluble?

a)

AgCl

b)

Pb(OH)2

c)

Na2CO3

d)

Co2O

e)

None of the above

80.

Which of the following compounds is insoluble?

a)

NaCl

b)

Ba(OH)2

c)

Na2SO4

d)

Fe2O3

e)

none of the above

81.

If 500 mL of a 12 M solution is left out for a week and some of the water evaporates leaving behind 350 mL of solution. What is the final molarity?

a)

21M

b)

17M

c)

8.4M

d)

5.6M

e)

1.2M

82.

Why is water sometimes called the “universal solvent?”

a)

The adhesion level in H2O is very high.

b)

Many substances dissolve in H2O

c)

The density of H2O is 1.0 g/cm3.

d)

The hydrogen bonding of H2O is very low.

83.

Electrolytes are important to the body because they contribute to basic functions such as muscle contraction. Electrolyte ions, such as sodium and magnesium, must be balanced correctly in order to maintain bodily functions. What property of water allows it to act as carrier for these ions? 

a)

Polarity

b)

Viscosity

c)

Shape

d)

Density

84.

Students are asked to make statements about the solubility graph above.  Which student does the best job of communicating the general features of the graph?

a)

Student A.  Most salts require 100 grams of water in order to dissolve completely.

b)

Student B.  Table salt has the average solubility of all salts.

c)

Student C.  The solubility of most salts increases with increasing temperature.

d)

Student D.  Most curves show a decreasing slope as the temperature rises.

85.

The solubility rules for various salts in water indicate most salts of _______ are not soluble in water.

a)

Li+

b)

Ag+

c)

K+

d)

Na+

86.

A solution in which more solute is dissolved than is typically soluble at a given temperature is —

a)

unsaturated

b)

saturated

c)

supersaturated

d)

diluted

87.

A solution that contains the maximum amount of solute that is soluble at a given temperature is said to be —

a)

unsaturated

b)

saturated

c)

supersaturated

d)

diluted

88.

Which of the following is the best way to determine if an aqueous solution of sodium acetate (NaC2H3O2) is supersaturated?

a)

Add water to the solution.

b)

Measure the temperature of the NaC2H3O2.

c)

Filter all the NaC2H3O2 out of the solution.

d)

Add a crystal of NaC2H3O2 to the solution.

89.

What will happen to the ability of a solid to dissolve in a liquid if the temperature increases?

a)

Solubility of the solid always increases

b)

Solubility of the solid always decreases

c)

Solubility of the solid usually increases

d)

Solubility of the solid usually decreases

90.

Which of the following would increase the rate of dissolution of a solid in a solution?

a)

Cool the solid and the solution

b)

Cool only the solid

c)

Dry up the solvent

d)

Stir the solid and solution

91.

Water can dissolve many substances because ―

a)

it has the molecular formula H2O

b)

it has a linear molecular shape

c)

it has a nonpolar molecular structure

d)

it has a partial charge on each side of its molecules

92.

In Flint, Michigan, toxic lead metal was found in the water and it needs to be filtered out in order for the city to have clean and safe drinking water.  A company is proposing a solution where they mix negative ions into the water to bond with the Pb+2 ions and form an insoluble solid that can be filtered out. Which of the following compounds contains ions that could be used in order to form a precipitate with lead?

a)

NaNO3

b)

K2SO4

c)

HC2H3O2

93.

Which type of solution has achieved equilibrium between solute and solvent if the solute is still visible after mixing?

a)

An unsaturated solution

b)

A saturated solution

c)

A supersaturated solution

d)

A dilute solution

94.

Which of the following would decrease the rate of solution when dissolving a solid in water?

a)

Raise the temperature of the solution

b)

Crush the solid before mixing

c)

Stir the solution after mixing

d)

Use a single cube of solid

95.

Which of the following would result in being able to dissolve a greater amount of gas in a solution?

a)

Cool the gas and solution

b)

Make the gas an electrolyte

c)

Heat the gas and solution

d)

Decrease the pressure of the solution

96.

What is the new pressure of 210 mL of a gas that is compressed to 70 mL when the original pressure was 3.0 atm and the temperature is held constant?

a)

100 atm

b)

0.90 atm

c)

1.0 atm

d)

9.0 atm

97.

What is the volume of 1 mole of gas at Standard Temperature and Pressure (STP)?

a)

22.4 L

b)

2.4 L

c)

.24 L

d)

.024 L

98.

Solid sodium carbonate, Na2CO3, reacts with sulfuric acid, H2SO4, to produce CO2 gas according to the following equation:

Na2CO3(s) + H2SO4(aq) → CO2(g) + H2O(l) + Na2SO4(aq)

During an experiment to produce carbon dioxide gas, a student recorded the following data:

Pressure CO2 = 708.1 mm Hg

Volume CO2 = 29.65 mL

Temperature CO2= 25.5 °C

How many moles of CO2 were produced? (Ideal Gas Constant is 62.4)

a)

0.00113 mol CO2

b)

0.857 mol CO2

c)

0.846 mol CO2

d)

888 mol CO2

99.

A sample of a gas in a rigid container at 30.0°C and 5.00 atm has its temperature increased to 40.0°C. What will be the new pressure?

a)

1.50 atm

b)

2.67 atm

c)

5.17 atm

d)

6.04 atm

100.

The volume of a gas is 100.0 mL at 20.0 K. What will be the new temperature if the gas is compressed to 20.0 mL under constant pressure?

a)

100 K

b)

10.0 K

c)

4.00 K

d)

5.00 K

101.

The volume of a sample of oxygen is 200.0 mL when the pressure is 3.000 atm and the temperature is 37.0 oC (310K). What is the new temperature if the volume increases to 400.0 mL and the pressure decreases to 2.000 atm?

a)

49.33 oC or 322.33K

b)

140.3 oC or 413.3K

c)

209.8 oC or 482.8K

d)

413.0 oC or 686K

102.

Which of the following is not one of the postulates of the kinetic molecular theory for ideal gases?

a)

The collisions between particles are elastic.

b)

The particles attract and then repel each other.

c)

The particle size is very small compared to the space between the particles.

d)

The particles are in constant random motion.

103.

According to the kinetic molecular theory of gases, the pressure of the gas is due entirely to the ―

a)

size of the gas particles compared to the size of its container

b)

mass of the gas particles compared to the size of its container

c)

force of the collisions of the gas particles with the walls of the container

d)

moles of gas particles within the walls of the container

104.

According to the kinetic molecular theory, which statement best describes the motion of gas particles?

a)

Gas particles are stationary.

b)

Gas particles are only in motion when a gas is heated.

c)

Gas particles are in continuous, random motion.

d)

Gas particles move together in the same direction.

105.
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
106.
2H2  +   O2  →  2H2O
How many moles of oxygen are consumed if 8 moles H2 are used?
a)
2
b)
4
c)
6
d)
8
107.
What is a Limiting Reagent?
a)
speeds up a reaction
b)
what you run out of first
c)
what you have left over
d)
slows down a reaction
108.
What is a Excess Reagent?
a)
amount you end with
b)
what you run out of first
c)
what you have left over
d)
what you start with
109.
For the Balanced Reaction: 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
110.
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
111.
Use the equation 2 Al + 3 Cl2 ---> 2 AlCl3.  If 2 moles of aluminum and 2 moles of chlorine are reacted, identify the limiting reactant.
a)
AlCl3
b)
Cl2
c)
Al
d)
Gary Busey
112.
If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the
a)
theoretical yield
b)
mole ratio
c)
actual yield
d)
percentage yield
113.
What is the measured amount of a product obtained from a chemical reaction?
a)
mole ratio
b)
theoretical yield
c)
percentage yield
d)
actual yield
114.

To convert from kg to grams you ______.

a)

Multiply by 1000

b)

Divide by 1000

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