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H Chem Tri B Final Exam Review

Total questions: 127

Worksheet time: 5hrs 10mins

Name
Class
Date
1.
What is the first thing you must do to solve a stoichiometry problem?
a)
Write a Balanced Equation
b)
Panic
c)
Write an Unbalanced Equation
d)
Ask for help
2.
KNO3 --> KNO2 + O2
What coefficients are needed to balance the reaction?
a)
2, 2, 1
b)
2, 3, 2
c)
1, 2, 2
d)
1, 3, 1
3.
WO3 + H2 --> W + H2O
What coefficient goes in front of H2?
a)
1
b)
2
c)
3
d)
4
4.

The equation for Percent Yield:

a)

(theoretical/experimental) X 100

b)

(experimental/theoretical) X 100

c)

(experimental - theoretical)/ Predicted X 100

5.

What is a Limiting Reagent?

a)

speeds up a reaction

b)

reactant consumed first

c)

reactant in excess

d)

slows down a reaction

6.

What is a Excess Reagent?

a)

amount you end with

b)

reactant consumed first

c)

reactant in excess

d)

reactant you start with

7.
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
8.
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
9.
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
10.
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
11.
2 KClO3 → 2 KCl + 3 O2
How many moles of oxygen are produced when 6.7 moles of KClO3 decompose completely?
a)
6.7 mol
b)
1.0 mol
c)
10.1 mol
d)
4.5 mol
12.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
13.

What is the measured amount of a product obtained from a chemical reaction?

a)

mole ratio

b)

theoretical yield

c)

percentage yield

d)

actual/experimental yield

14.
Cl2 + 2 KBr → Br2 + 2 KCl
How many grams of potassium chloride can be produced from 356 g of chlorine and 356 g of potassium bromide?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
15.
Fe (s) + S (l) --> FeS (s)  

In the experiment above, 7.62 g of Fe are allowed to react with 8.67 g of S.
How much FeS is formed?
a)
14.8 g
b)
12.2 g
c)
13.7 g
d)
19.9 g
16.
Mole ratios are obtained from the
a)
balanced chemical equation
b)
periodic table
c)
molar mass
17.
9. Complete the equation for the percent yield of a chemical reaction:
Percent yield=(________)÷(________)×100%
a)
actual yield; theoretical yield
b)
theoretical yield; actual yield
18.
What type of reaction is represented 2H2  + O2 = 2H2O?
a)
Decomposition
b)
Combustion
c)
Synthesis
d)
Neutralization
19.
What type of reaction produces carbon dioxide and water?
a)
Neutralization
b)
Synthesis
c)
Decomposition
d)
Combustion
20.
What is stoichiometry?
a)
The study of how the quantities of reactants and products are related in chemical reactions
b)
The study of the speed of reactions
c)
The study of how chemical reactions occur
d)
The study of types of reactions
21.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
22.

What is the percent by mass of a solution made by dissolving 20.0 g of NaCl into 180.0 g of water?

a)

10.0 %

b)

11.1 %

c)

80.0 %

d)

20.0 %

23.

Find the percentage composition of Mg in Mg3(PO4)2.


a)

27.48% Mg

b)

43.11% Mg

c)

16.00% Mg

d)

12.63% Mg

24.

What is the mass percentage of Carbon in Carbon dioxide (CO2)?

a)

27.27%

b)

42.86%

c)

72.73%

d)

72.72%

25.
What are the units in molar mass?
a)
grams
b)
moles
c)
moles/gram
d)
grams/mole
26.
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
27.
Another name for a homogeneous mixture is 
a)
an element.
b)
a solution.
c)
a compound.
28.
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
29.
Which solute is the most soluble at 10 ⁰C?
a)
KI
b)
KClO3
c)
NH4Cl
d)
NH3
30.

You are given a small beaker of solution at room temp. You add a bit of solute to the solution and it dissolves. The solution was:

a)

saturated

b)

unsaturated

c)

concentrated

d)

warm

31.
When one of the parts of the solution is water we call it _________. 
a)
water stuff 
b)
water mixture 
c)
aqua-man
d)
aqueous 
32.
What does it mean to be "Soluble" ?
a)
Capable of being a solid.
b)
To have soul.
c)
Capable of being dissolved.
d)
To sink.
33.
What is the unit for molarity?
a)
mass/liters
b)
moles
c)
liters
d)
moles/liter
34.
A measure of the amount of solute in a given amount of solvent or solution is...
a)
saturated
b)
solubility
c)
concentration
d)
miscible
35.
A saturated 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.
36.

An electrolyte is...

a)

The rapid, random movement of particles in colloidal dispersion.

b)

A substance that dissociates/ionizes into ions in water and conducts electric current.

c)

A substance that dissolves in water and does not conduct electric current.

d)

The solution process when water is the solvent.

37.
A nonelectrolyte is...
a)
The rapid, random movement of particles in colloidal dispersion.
b)
A substance that dissolves in water and conducts electric current.
c)
A substance that dissolves in water and does not conduct electric current.
d)
The solution process when water is the solvent.
38.
The substance dissolved in a solution is called ... 
a)
colloid
b)
solution
c)
solute
d)
solvent
39.
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
40.
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
41.
What is it about the water molecule that makes it a great solvent?
a)
water demonstrates polarity; a partial charge on each side of the molecule
b)
due to its molecular formula
c)
it has a liner molecular shape
d)
due to it's non-polar molecular structure
42.
What is the correct formula to solve for the Molarity of a solution that has .4 moles of HCl in 9.5 L of solution?
a)
M = 9.5 L / .4 mol
b)
M1V1=M2V2
c)
M = .4 mol / 9.5 L
d)
none of the other choices
43.
A sample of 0.0255 mol potassium hydroxide, KOH, was dissolved in water to yield 10.0 mL of
solution.  Which amount would you need to change to solve for molarity?
a)
change .0255 moles to grams
b)
change 10 mL to L
c)
change both values to grams and L
d)
leave it as it is
44.
Find the molarity of 186.55 g of sucrose, C12H22O11 (MM = 342) in 250 mL of water.
a)
2.18 M
b)
0.746 M
c)
1.18 M
d)
0.545 M
45.
How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?
a)
1074 mol
b)
0.069 mol
c)
1.07 mol
d)
62.7 mol
46.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
47.
Which of the following has the most NaCl (MM = 58.44)?
a)
100 mL of a 1.8 M solution
b)
50 mL of a 4.1 M solution
c)
9.35 grams
d)
1 mole
48.
How many mL of 10.8M HCl are required to make 100.0 mL of 3.00M acid?
a)
27.8 mL
b)
27.78 mL
c)
2.8 mL
d)
278 mL
49.

Identify if the following solution would be saturated, unsaturated, or supersaturated: 103 g KBr at 70'C.

a)

Unsaturated

b)

Saturated

c)

Supersaturated

50.

How could you change a saturated solution to an unsaturated solution?

a)

Add solvent

b)

Add solute

51.

A ______________ solution contains more dissolved solute than a saturated solution at the same temperature.

a)

saturated

b)

supersaturated

c)

suspended

d)

unsaturated

52.

An aqueous solution is:

a)

any liquid with another compound dissolved in it.

b)

an ionic compound with water dissolved in it.

c)

water with another compound dissolved in it.

d)

none of the above

53.

Which of the following compounds is SOLUBLE?

a)

copper carbonate

b)

calcium carbonate

c)

potassium carbonate

d)

strontium carbonate

54.

In writing the chemical equation for a precipitation reaction, what abbreviation of the physical state must appear with one of the products?

a)

(s)

b)

(g)

c)

(l)

d)

(w)

55.

What would be the formula of the precipitate that forms when Pb(NO3)2 (aq) and K2SO4 (aq) are mixed?

a)

K(NO3)2

b)

PbSO4

c)

PbK2

d)

H2O

56.

Considering the following precipitation reaction:

Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq)

What is the correct complete ionic equation?

a)

Pb2+ + (NO3)2- + 2K+ + 2I- → PbI2(s) + 2K+ + 2NO3-

b)

Pb2+ + 2NO3- +2K+ + I- → PbI2(s) + 2K+ + NO3-

c)

Pb2+ + 2NO3- + 2K+ + 2I- → PbI2(s) + 2K+ + 2NO3-

d)

Pb2+ + 2NO3- + 2K+ + 2I- → Pb2+ + 2I- + 2K+ + 2NO3-

57.

Which of the following statements about writing molecular, complete and net ionic equations is FALSE?

a)

A molecular equation is a chemical equation showing the complete, neutral formulas for every compound in a reaction

b)

A complete ionic equation is a chemical equation showing all of the species as they are actually present in solution.

c)

A net ionic equation is an equation showing only the species that actually participate in the reaction.

d)

A spectator ion remains unchanged in the reaction and appears on both sides of the equation.

e)

All of the statements are true

58.

Which of the following compounds is INSOLUBLE?

a)

magnesium phosphate

b)

magnesium sulfate

c)

magnesium iodide

d)

magnesium nitrate

e)

none of the above

59.

What is the net ionic equation for the precipitation reaction between BaCl2 and Na2SO4?

a)

BaCl2(aq) + Na2SO4(aq) --> BaSO4(s) + 2NaCl(aq)

b)

Na+(aq) + Cl-(aq) --> NaCl(s)

c)

Ba2+(aq) + SO42-(aq) --> BaSO4(s)

d)

Ba2+(aq) + 2Cl-(aq) + 2 Na+(aq) + SO42-(aq) --> BaSO4(s) + 2Cl-(aq) + 2Na+(aq)

60.

When solutions of two ionic compounds are combined and a solid forms, the process is called

a)

hydration

b)

solvation

c)

dissociation

d)

precipitation

61.

Which of the following pairs of solutions produces a precipitate when combined?

a)

Cu(NO3)2 and NaCl

b)

Fe(NO3)3 and MgCl2

c)

Cu(NO3)2 and K2CO3

d)

CaCl2 and NaNO3

62.

Identify the spectator ion(s) in the equation: 2Ag+(aq) + 2NO3–(aq) + 2Na+(aq) + S2–(aq) --> Ag2S(s) + 2Na+(aq) + 2NO3–(aq)

a)

2Ag+(aq) + 2NO3–(aq)

b)

2Na+(aq) + 2NO3–

c)

2Na+(aq) + S2–(aq)

d)

Ag2S(s) + 2Na+(aq

63.
A neutralization reaction will always produce...
a)
water & salt
b)
water
c)
salt
d)
water & carbon
64.
If there is excess hydrogen ions, the solution will be...
a)
acidic
b)
basic
65.
If there is excess hydroxide ions, the solution will be...
a)
acidic
b)
basic
66.
Zn(OH)2 is an example of a...
a)
acid
b)
base
c)
salt
67.
H3PO4 is an example of a ...
a)
acid
b)
base
c)
salt
68.
Identify the salt in the following equation:
Zn(OH)2 + HNO3   ---> H2O  + Zn(NO3)2
a)
Zn(OH)2
b)
HNO3
c)
H2O
d)
Zn(NO3)2
69.
At what pH is a solution neutral?
a)
0
b)
7
c)
14
70.

Which of the following is NOT a property of bases.

a)

Bitter

b)

Makes OH- in solution.

c)

pH below 7

d)

pH above 7

71.

Which of the following are NOT properties of acids?

a)

sour

b)

bitter

c)

pH below 7

d)

creates H3O+ ions in a solution.

72.

What range of values on the pH scale represent solutions with a higher ratio of hydronium (H3O+) ions?

a)

0-14

b)

below 7

c)

7

d)

above 7

73.

When found in food, acids often taste ________.

a)

Sour

b)

Bitter

c)

Salty

d)

Slippery

74.

Pure water (H2O) has a pH of 7 and would be classified as...

a)

a base

b)

a neutral substance

c)

both an acid and a base

d)

an acid

75.

The reactants in a neutralization reaction are always...

a)

salt and water

b)

an acid and a base

c)

a neutral solution

d)

carbon dioxide and oxygen

76.
Turns litmus blue.
a)
Acids
b)
Bases
c)
Salts
d)
All
77.

Acids are __________, which means they "eat away" at other materials.

a)

transitional metal

b)

alkaline

c)

flammable

d)

corrosive

78.
Which of the following solutions is most basic?
(HINT...be careful! Acidity and basicity are determined by the point measured on the pH scale. And don't forget [H+] = 10-pH)
a)
[H+] = 1 x 10-11
b)
[OH-] = 1 x 10-4
c)
[H+] = 1 x 10-2
d)
[OH-]= 1 x 10-13
79.
The pH of a solution is 4.00.  What is the hydroxide ion concentration?
(HINT...pH + pOH = 14 and
[OH-] = 10-pOH)
a)
[OH-] = 1 x 10-4
b)
[OH-] = 1 x 10-6
c)
[OH-] = 1 x 10-10
d)
[OH-] = 1 x 10-14
80.
What is the pH of a solution with a hydrogen ion concentration of 1.0 x 10-8 M?
(HINT...use the calculator...
pH = -log [H+] )
a)
-8
b)
6
c)
8
d)
14
81.
What is the pH of a solution that has a [H+] of 2.5 x 10-5?
a)
4.60
b)
5.0
c)
2.5
d)
7
82.
What is the pOH of a solution where the [OH-] is 7.3 x 10-2 M?
a)
-1.14
b)
2.0
c)
1.14
d)
7.3
83.
What is the [OH-] if the [H+] is 1.0 x 10-3M?
a)
1.0 x 10-3 M
b)
6.02 x 10-23 M
c)
1.0 x 10-14 M
d)
1.0 x 10-11 M
84.

Identify the acid listed below:

a)

KOH

b)

H2O

c)

H2SO4

d)

NaCl

85.

If a solution has a [H+] of 1.0 x 10 -5, what is the [OH-]?

a)

1.0 x 10 -9

b)

1.0 x 10 -5

c)

1.0 x 10 -14

d)

1.0 x 10 -7

86.

If HF and KOH react, which salt would be produced?

a)

KF

b)

HOH

c)

FOH

d)

HK

87.

During a titration, 20. mL of 0.50 M HF is used to neutralize 10. mL of NaOH. What is the concentration of the base?

a)

1.0 M NaOH

b)

0.25 M NaOH

c)

400 M NaOH

d)

10 M NaOH

88.

A student collects the following data during a titration. Calculate the concentration of acid:

Volume of Acid: 20. mL HCl

Concentration of NaOH: 1.0 M NaOH

Initial Buret Reading of NaOH: 1.70 mL

Final Buret Reading: 32.20 mL

a)

1.6 M HCl

b)

1.5 M HCl

c)

0.085 M HCl

d)

0.66 M HCl

89.

You need a pH of 6.2; you have a pH of 5.1. Do you need to add an acid or a base?

a)

A base.

b)

An acid.

90.

You need a pH of 7; you have a pH of 11.2. What should you add?

a)

A base.

b)

An acid.

91.

Which chemical is a proton donor?

a)

Acid

b)

Base

92.

After a chemical reaction, the beaker feels cold to the touch. This is likely a ____________ reaction.

a)

negative

b)

positive

c)

endothermic

d)

exothermic

93.

This type of reaction releases thermal energy to its surroundings.

a)

endothermic

b)

exothermic

c)

decomposition

d)

synthesis

94.

When the pH of a solution changes from 6 to 4, the solution becomes

a)

2 times less acidic

b)

2 times more acidic

c)

100 times less acidic

d)

100 times more acidic

95.
Combining substances to form a new substance
a)
Displacement
b)
Synthesis
c)
Decomposition
d)
Oxidation
96.
Breaking down a substance into simpler substances
a)
Displacement
b)
Synthesis
c)
Decomposition
d)
Oxidation
97.
What type of reaction is the equation C + O2 → CO2?
a)
Synthesis Reaction
b)
Decomposition Reaction
c)
Single Displacement Reaction
d)
Double Displacement Reaction
98.
What type of reaction is the equation 2NaCl →2Na +Cl2?
a)
Synthesis Reaction
b)
Decomposition Reaction
c)
Single Displacement Reaction
d)
Double Displacement Reaction
99.
Cu + 2Ag(NO3) → 2Ag + Cu(NO3)
a)
Synthesis Reaction
b)
Decomposition Reaction
c)
Single Displacement Reaction
d)
Double Displacement Reaction
100.
Consider the chemical equation CH4 + 2 O2 → CO2 + 2 H2O. In this equation, CH4 is a
a)
product
b)
reactant
c)
displacement
101.
Si + S8 --> Si2S4
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
102.
Pb(NO3)2 --> PbO + NO2 + O2
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Combustion
103.

What reaction has the following general formula:
 CxHy + O2 −>CO2 + H2OC_xH_y\ +\ O_2\ ->CO_{2\ }+\ H_2O  

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

104.

What type of reaction is the following:
 2KI −> 2K + I22KI\ ->\ 2K\ +\ I_2  

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

105.

What type of reaction is the following:
 C11H24+17O2−> 11CO2 + 12H2OC_{11}H_{24}+17O_2->\ 11CO_2\ +\ 12H_2O  

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

106.

What type of reaction is the following:
 2C4H10 +13O2 −> 8CO2+10H2O2C_4H_{10}\ +13O_2\ ->\ 8CO_2+10H_2O 

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

107.
CaCO3 ----> CaO + CO2
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
108.

MgCl2 + Li2CO3 ----> MgCO3 + 2 LiCl

a)

Synthesis

b)

Neutralization

c)

Single displacement

d)

Precipitation

e)

No Reaction

109.

All chemical equations must be balanced because of the Law of Conservation of Mass. This law 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

110.

The following reaction is classified as:

Zn(OH)2 + HNO3 ---> H2O + Zn(NO3)2

a)

Synthesis

b)

Single Replacement

c)

Precipitation

d)

Neutralization

e)

No Reaction

111.

Which process involves the transfer of electrons?

a)

double replacement

b)

neutralization

c)

oxidation-reduction

d)

sublimation

112.

During an oxidation-reduction reaction, the number of electrons gained is

a)

equal to the number of electrons lost

b)

equal to the number of protons gained

c)

less than the number of electrons lost

d)

less than the number of protons gained

113.

In a redox reaction, there is a conservation of

a)

mass, only

b)

charge, only

c)

both mass and charge

d)

neither mass nor charge

114.

During which process does an atom gain one or more electrons?

a)

transmutation

b)

reduction

c)

oxidation

d)

neutralization

115.

When a lithium atom forms an Li+ ion, the lithium atom

a)

gains a proton

b)

gains an electron

c)

loses a proton

d)

loses an electron

116.

Defined as the loss of electrons.

a)

oxidation

b)

reduction

c)

redox

d)

OIL RIG

117.

Defined as the gain of electrons.

a)

oxidation

b)

redox

c)

reduction

d)

LEO GER

118.
In order to convert to Kelvin, you add ______ to the Celsius measurement.
a)
372
b)
273
c)
237
d)
732
119.
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
120.
The following graph shows ____ relationship. 
a)
Direct
b)
Inverse
121.
In the ideal gas law, which variable represents the gas constant?
a)
n
b)
R
c)
T
d)
V
122.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm (make sure you use the correct R value).
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
123.

A sample of gas at a constant pressure with a volume of 30.0 mL at 25.0oC is heated to 50.0oC. What is the new volume of the gas?

a)

60.0 mL

b)

15.0 mL

c)

27.5 mL

d)

32.5 mL

124.
A sample of oxygen gas has a volume of 150.0 mL when its pressure is .947 atm. What will the volume of the gas be if it is lowered to a pressure of 0.658 atm and the temperature remains constant?
a)
72 mL
b)
144 mL
c)
216 mL
d)
288 mL
125.
Three gases, Ar, N2 and H2 are mixed in a sealed container. Ar has a pressure of 255 torr, N2 has a pressure of 228torr and H2 has pressure of 752torr. What is the total pressure in the container?
a)
483torr
b)
270torr
c)
1235torr
126.
Determine the number of moles in a container of gas at STP with a volume of 99.2 L. 
a)
2222.08 moles
b)
4.43 moles
c)
22.4 moles 
d)
76.8 moles
127.
Determine the initial temperature of a random gas when the initial volume is 2.2 L and it is cooled to 88K with a volume of 0.85 L. 
a)
0.029 K
b)
0.021 K
c)
227.76 K
d)
34 K

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