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Chemistry Spring Review

Total questions: 96

Worksheet time: 3hrs 12mins

Name
Class
Date
1.
How many protons are in this atom?
a)
3
b)
4
c)
6
d)
10
2.
How many neutrons are in this isotope of Uranium?
a)
235
b)
92
c)
327
d)
143
3.
How are these isotopes different?
a)
Different atomic numbers
b)
Different number of protons
c)
Different number of neutrons
d)
Different number of electrons
4.
What process is modeled with this equation?
a)
alpha decay
b)
beta decay
c)
fission
d)
fusion
5.
Which nuclear process is shown in the picture?
a)
fission
b)
fusion
c)
alpha decay
d)
beta decay
6.
What happens to the atomic number during alpha decay?
a)
The atomic number decreases by 4
b)
The atomic number increases by 1
c)
The atomic number decreases by 2.
d)
The atomic number stays the same.
7.

In order of most to least penetrating radiation we have

a)

Alpha , Beta, Gamma

b)

Beta , Gamma , Alpha

c)

Gamma, Beta, Alpha

d)

Gamma, Alpha, Beta

8.
The half life of Thorium-234 is 24 days. What fraction of the element remains after 96 days
a)
1/2
b)
1/4
c)
1/8
d)
1/16
9.
Which type of nuclear radiation is being emitted here?
a)
Alpha
b)
beta
c)
gamma 
d)
none
10.

Complete the nuclear equation and determine the type of decay that is occurring in this reaction.

a)

alpha

b)

beta

c)

gamma

d)

none

11.
The time taken for half of an amount of radioactive atoms to decay.
a)
Nuclear fusion
b)
Full-life
c)
Dead time
d)
Half-life
12.

The nuclear process occurring at a nuclear power plant involves splitting large atoms into smaller atoms & neutrons is called....

a)

Nuclear fusion

b)

Nuclear fission

c)

Combustion

d)

Multiplication

13.
What type of decay is this?
7534Se + 0-1e --> 7533As
a)
Electron Capture
b)
Positron Emission
c)
Alpha Decay
d)
Beta Decay
14.
The technetium-99 isotope has a half-life of 6.0 hours. If 100.0 mg were injected into a patient how much remains after 18 hours?
a)
33.0 mg
b)
12.5 mg
c)
.33 mg
d)
15.8 mg
15.
What would two different isotopes of an atom have in common?
a)
Number of neutrons 
b)
Number of protons
c)
Atomic weight 
d)
Atomic mass
16.
What element is the ?
a)
Ag-115
b)
Cd-115
c)
Pd-115
d)
Not Listed
17.
Balance the following equation:
146C --> 0-1e + ________
a)
145B
b)
146C
c)
147N
d)
42He
18.
What type of reaction is this?
a)
alpha
b)
beta
c)
gamma
d)
quiet
19.
Has the highest penetrating power.  Can penetrate our body.  Even several cm thick of lead or several meters thick of concrete cannot stop all of it.
a)
Alpha
b)
Beta
c)
Gamma
20.
Has the lowest penetrating power.  Can only penetrate 0.05 mm into the body and can be stopped by a piece of paper or clothing.
a)
Alpha
b)
Beta
c)
Gamma
21.
What is the symbol for an alpha particle?
a)
42He
b)
0-1e
c)
0+1 e
d)
10n
22.
In a nuclear reactor what slows down neutrons?
a)
Control Rods
b)
Moderator
c)
Sheilding
d)
The brakes
23.
Detects radiation by counting electric pulses carried by gas atoms ionized by radiation
a)
Geiger-Muller counter
b)
Scintillation counter
c)
Film badge
d)
Radioactive detective
24.
Scientist involved with discovery of radioactivity.
a)
Albert Einstein
b)
Ernest Rutherford
c)
Marie Curie
d)
Isaac Newton
25.
If you start out with 100 grams of a radioisotope, how much remains after 2 half-lives?
a)
100 grams
b)
75 grams
c)
50 grams
d)
25 grams
26.
What fuel does the US typically use in fission reactors?
a)
Hydrogen
b)
Carbon
c)
Uranium
d)
Plutonium
27.
What product of fission is necessary in order to establish a chain reaction?
a)
alpha particle
b)
two or more neutrons
c)
two or more protons
d)
gamma rays
28.
How long do spent fuel rods remain dangerously radioactive?
a)
tens of thousands of years
b)
several years
c)
they aren't radioactive
d)
impossible to determine
29.
Why do we need neutron absorption in a nuclear reactor?
a)
it recycles the fuel
b)
it increases heat absorption
c)
it speeds up a reaction
d)
it slows down a reaction
30.

An acid that releases only one Hydrogen (H+) ion.

a)

Monoprotic Acid

b)

Diprotic Acid

c)

Triprotic Acid

d)

Amphoteric

31.

A substance that can either act as an acid or base

a)

Monoprotic Acid

b)

Diprotic Acid

c)

Triprotic Acid

d)

Amphoteric

32.

What specific substance has the ability to act as an acid or base

a)

Hydronium Ion

b)

Hydroxide Ion

c)

Water

d)

Ammonia

33.

The product that results when a base accepts a proton.

a)

Conjugate Base

b)

Conjugate Acid

c)

Conjugate pair

d)

Amphoteric

34.

It is a reaction between a Brønsted-Lowry acid and water.

a)

Autoionization

b)

Base Ionization

c)

Acid Ionization

d)

Water Ionization

35.

In this type of reaction, a substance ionizes when one molecule of the substance reacts with another molecule of the same substance.

a)

Autoionization

b)

Base Ionization

c)

Acid Ionization

d)

Water Ionization

36.

They are proton (Hydrogen ion) donors according to _____.

a)

Acid - Bronsted Lowry

b)

Base - Bronsted Lowry

c)

Acid - Lewis

d)

Base - Lewis

e)

Acid - Arrhenius

37.

They are substances that ionize (break off) in an aqueous solution to produce hydroxide (OH-) ions in solution according to _____.

a)

Acid - Bronsted Lowry

b)

Base - Bronsted Lowery

c)

Acid - Arrhenius

d)

Base - Arrhenius

e)

Acid - Lewis

38.

They are proton (Hydrogen ion) acceptors according to ______.

a)

Acid - Bronsted Lowry

b)

Base - Bronsted Lowery

c)

Acid - Arrhenius

d)

Base - Arrhenius

e)

Acid - Lewis

39.

They are - substances that ionize (break off) in an aqueous solution to produce hydrogen (H+) ions

a)

Acid - Lewis

b)

Base - Bronsted Lowery

c)

Acid - Arrhenius

d)

Base - Arrhenius

e)

Acid - Lewis

40.

They are electron-pair acceptors according to _____.

a)

Acid - Arrhenius

b)

Base - Arrhenus

c)

Acid - Bronsted Lowry

d)

Base - Bronsted Lowry

e)

Acid - Lewis

41.

What is the Conjugate Acid in the reaction below:

NH4+ + H2O → NH3 + H3O+

a)

NH4+

b)

H2O

c)

NH3

d)

H3O+

42.

What is the Acid in the reaction below:

NH4+ + H2O → NH3 + H3O+

a)

NH4+

b)

H2O

c)

NH3

d)

H3O+

43.

What is the Base in the reaction below:

C2O42– + HC2H3O2 ↔ HC2O4– + C2H3O2–

a)

C2O42–

b)

HC2H3O2

c)

HC2O4–

d)

C2H3O2–

44.

What is the Conjugate Base in the reaction below:

C2O42– + HC2H3O2 ↔ HC2O4– + C2H3O2–

a)

C2O42–

b)

HC2H3O2

c)

HC2O4–

d)

C2H3O2–

45.

What is the Base in the reaction below:

NH4+ + H2O → NH3 + H3O+

a)

NH4+

b)

H2O

c)

NH3

d)

H3O+

46.

What is the Acid in the reaction below:

C2O42– + HC2H3O2 → HC2O4– + C2H3O2–

a)

C2O42–

b)

HC2H3O2

c)

HC2O4–

d)

C2H3O2–

47.

What is the Conjugate Base in the reaction below:

NH4+ + H2O → NH3 + H3O+

a)

NH4+

b)

H2O

c)

NH3

d)

H3O+

48.

An Arrhenius base:

a)

donates H+

b)

accepts H+

c)

produces H+

d)

produces OH-

49.

An Arrhenius acid:

a)

donates H+ to another substance

b)

accepts H+ from another substance

c)

produces H+

d)

produces OH-

50.

The Acid-Base classification system that defined any chemical species that accepts a pair of electrons as an acid, and a base is a chemical species that donates a pair of electrons.

a)

Bronsted-Lowry

b)

Arrhenius acid-base

c)

Lewis acid-base

d)

Monoprotic and Polyprotic Acids

51.
A gas that has a pressure of 2 atm and a volume of 10 L.  What would be the new volume if the pressure was changed to 1 atm?
a)
P1/T1 = P2/T2
b)
P1V1 = P2V2
c)
V1/n1 = V2/n2
d)
PV = nRT
52.
A sample of a gas has a volume of 852 mL at 298 K. What temperature is necessary for the gas to have a volume of 945 mL?
a)
Pt = P1 + P2 + P3 + ...
b)
P1V1 = P2V2
c)
V1/T1 = V2/T2
d)
P1V1/T1 = P2V2/T2
53.
If a nitrogen gas occupies a volume of 500 ml at a pressure of 0.971atm. What volume will the gas occupy at a pressure of 1.50 atm?  
a)
P1V1 = P2V2
b)
PV = nRT
c)
P1/T1 = P2/T2
d)
V1/n1 = V2/n2
54.
Determine the number of moles in a container of gas at STP with a volume of 99.2 L. 
a)
V1/n1 = V2/n2
b)
PV = nRT
c)
P1/T1 = P2/T2
d)
V1/T1 = V2/T2
55.
A container is filled with H2, and H2O. What is the partial pressure of H2 when the pressure of water is 17 kPa. The total pressure of the gases is 750 kPa.
a)
P1V1 = P2V2
b)
Pt = P1 + P2 + P3 +...
c)
P1/T1 = P2/T2
d)
V1/n1 = V2/ n2
56.
A container is filled with H2, and H2O. What is the partial pressure of H2 when the pressure of water is 17 kPa. The total pressure of the gases is 750 kPa.
a)
P1V1 = P2V2
b)
Pt = P1 + P2 + P3 +...
c)
P1/T1 = P2/T2
d)
V1/n1 = V2/ n2
57.
A sample of gas with a volume of 30.0 mL at 25.0oC is heated to 50.0oC.  What is the new volume of the gas?
a)
P1V1 = P2V2
b)
P1/T1 + P2/T2
c)
PV = nRT
d)
V1/T1 = V2/T2
58.
If the pressure exerted by a gas at 298 K in a volume of 0.044 L is 3.81 atm, how many moles of gas are present?
a)
P1/T1 = P2/T2
b)
PV = nRT
c)
V1/n1 = V2/n2
d)
P1V1 = P2V2
59.
A gas fills a balloon at a temperature of 27 oC and 1 atm of pressure. What will the pressure of the balloon be if the gas is heated to 127 oC?
a)
P1V1 = P2V2
b)
PV = nRT
c)
P1/T1 = P2/T2
d)
V1/T1 = V2/T2
60.
A 220.0 mL sample of helium gas is in a cylinder at 105 kPa and 275 K. The piston is pushed in until the sample has a new temperature of 310 K and new pressure of 150 kPa. What is the new volume of the gas? 
a)
P1V1/T1 = P2V2/T2
b)
PV = nRT
c)
P1V1 = P2V2
d)
Pt = P1 + P2 + P3 + ...
61.
A gas is at a pressure of 12 atm, a volume of 23 L, and a temperature of 200K. If the pressure is raised to 14 atm,  and the temperature is increased to 300K. What is the new volume of the gas?
a)
P1V1/T1 + P2V2/T2
b)
PV = nRT
c)
P1V1 = P2V2
d)
P1/T1 = P2/T2
62.
If the total pressure is 0.99 atm, and the partial pressure of carbon dioxide and hydrogen sulfide is 0.05 atm and 0.02 atm respectively.  What will be the partial pressure of the remaining air?
a)
P1V1 = P2V2
b)
Pt = P1 + P2 + P3 + ...
c)
PV = nRT
d)
P1/T1 = P2/T2
63.
What is the correct formula for Boyle's Law?
a)
V1/T1=V2/T2
b)
P1V1=P2V2
c)
P1/T1=P2/T2
d)
PV=nRT
64.
Which of the following temperatures is appropriate to convert 25oC into the Kelvin scale?
a)
373K
b)
272K
c)
372K
d)
273K
65.
What would you expect to see if temperature increased if you were using Charles's Law?
a)
volume would decrease proportionally
b)
volume would increase proportionally
c)
pressure would increase proportionally
d)
pressure would decrease proportionally
66.
Gay-Lussac's law shows the directly proportional relationship between which two variables?
a)
pressure-temperature
b)
volume-temperature
c)
volume-pressure
d)
temperature-number of moles
67.
Which gas law would best be used when there are no variables being held constant?
a)
Boyle's Law
b)
Charles's Law
c)
Ideal Gas Law
d)
Combined Gas Law
68.
Using Gay-Lussac's 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
69.
What is 50 C in Kelvin?
a)
223
b)
323
c)
100
d)
50
70.
In order to convert to Kelvin, you add ______ to the Celsius measurement.
a)
372
b)
273
c)
237
d)
732
71.
In the ideal gas law, which variable represents the gas constant?
a)
n
b)
R
c)
T
d)
V
72.
100 degrees Celsius is equal to _______ Kelvin. 
a)
0 K
b)
273 K
c)
173 K
d)
373 K
73.
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)
Avogadro's Number
74.
Balance the following reaction :
 
CaC₂(s)   +   H₂O(l)   -->   C₂H₂(g)   +   Ca(OH)₂(aq)
a)
1,2,2,2
b)
1,2,1,1
c)
2,1,1,1
d)
2,1,2,1
75.
What is the mole ratio of H2O to H3PO4 in the following chemical equation?   P4O10 + 6 H2O --> 4 H3PO4 
a)
6:4
b)
4:6
c)
1:3
d)
3:1
76.
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)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
77.
2Al + 3H2SO4 -> Al2(SO4)3 + 3H2
How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with aluminum?
a)
0.85 g
b)
290 g
c)
450 g
d)
870 g
78.
For the reaction represented by the equation Cl2 + 2KBr → Br2 + 2KCl, how many grams of potassium chloride can be produced from 356 grams potassium bromide?
a)
749 g
b)
225 g
c)
479 g
d)
814 g
79.

A student burns 1.50 mol C3H8 according to the following reaction:

C3H8 + 5O2 → 3CO2 + 4H2O

How many grams of carbon dioxide are produced?

a)

44.0 g

b)

66.1 g

c)

132 g

d)

198 g

80.
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
81.
2NaClO3 (s) → 2NaCl (s) + 3O2 (g)  
12.00 moles of NaClO3 will produce how many grams of O2?
a)
256 g of O2
b)
576 g of O2
c)
288 g O2
82.
Cl2 + 2KBr → Br2 + 2KCl
How many grams of potassium chloride (KCl) can be produced from 356 g of potassium bromide (KBr)?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
83.
The limiting reactant
a)
slows the reaction down
b)
is used up first
c)
is the reactant that is left over
d)
controls the speed of the reaction
84.
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
85.
CH4 + 2H2O --> CO2 + 4H2
What is the limiting reactant when 20g CH4 react with 15g H2O?
a)
CH4
b)
H2O
c)
CO2
d)
H2
86.
Fe + S --> FeS
If 7.62g Fe react with 8.67g S, what is the limiting reactant?
a)
Fe
b)
S
c)
FeS
d)
none 
87.
SO2 + PCl5 --> SOCl2 + POCl3
How much SOCl2 is produced when 16.2g SO2 react with 13.7g PCl5? 
a)
7.87g
b)
30.1g
c)
26.4g
d)
19.8g 
88.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
89.
When reacting Na with Cl2, we calculated that the theoretical yield should be 12.5 grams. Our actual yield was 13.0 grams. What is the percent yield?
a)
100%
b)
104%
c)
96%
d)
1.04
90.
When you use a balanced chemical equation to calculate the amount of a product on paper it is referred to as the 
a)
experimental value
b)
theoretical value
c)
true amount
d)
percent yield
91.
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
92.
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
93.
If the percentage yield for a chemical reaction is 80.0%, the 
a)
actual yield is 80.0g for every theoretical yield of 100g.
b)
actual yield is 80 times as much as the theoretical yield.
c)
theoretical yield is 80 times as much as the actual yield. 
d)
theoretical yield is 80.0 g for every actual yield of 100g.
94.
The excess reactant
a)
.
b)
is used up first
c)
is the reactant that is left over
d)
.
95.
Mole ratios are obtained from the
a)
balanced chemical equation
b)
periodic table
c)
molar mass
96.
Stoichiometry is based on the law of conservation of
a)
charge
b)
mass
c)
reactants
d)
volume

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