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Chemistry Final Exam Review

Total questions: 166

Worksheet time: 4hrs 18mins

Name
Class
Date
1.
A series of steps used by scientists to solve a problem or answer a question. 
a)
scientific method
b)
recipe
c)
data collection
d)
metric system
2.
Testing a hypothesis often involves a(n):
a)
answer
b)
experiment
c)
problem
d)
safety check
3.

What is the first step in the scientific method?

a)

Data

b)

Conclusion

c)

No Horse Play

d)

Observe a problem

4.
An experiment is conducted to test how different cleats change an athletes running speed.  Six different types of cleats are tested and the 100m run time is recorded.  What is the independent variable?
a)
The type of cleat
b)
The run time
c)
The 100 meters
d)
The athlete
5.

Experiment: Sendel wants to see if taking the backroads to work is faster than taking the highway during rush hour.


In Sendel's driving experiment, what is the control group?

a)

Highway

b)

Backroads

c)

Time she drives to work

d)

Rush hour

6.
A test is set up to test which brand of soda creates the biggest foam explosion when adding a Mentos candy.  Three different sodas were tested. They measured the height of the foam eruption.   What is the dependent variable?
a)
Brand of soda
b)
Number of mentos candies used
c)
Height of foam eruption
d)
Temperature of soda
7.
How would you write 4.3756 x 104 in standard form?
a)
437,560,000
b)
0.00043756
c)
43,756
d)
4,3756
8.
How would you write 0.0005 in scientific notation?
a)
50 x 105
b)
5 x 104
c)
5 x 103
d)
.5 x 103
9.
How many significant figures does the following number have: 0.002040
a)
6
b)
4
c)
3
d)
2
10.

How many significant figures: 450 m

a)

3

b)

2

c)

1

d)

0

11.
Which observation is quantitative?
a)
It is 5 cm long
b)
It is smooth
c)
It looks red
d)
It is dry
12.

The table top is smooth.

a)

Qualitative Observation

b)

Quantitative Observation

13.

15 m = _____ mm

a)

15,000

b)

1,500

c)

0.015

d)

150

14.

762 cL = _____ L

a)

7.62

b)

0.762

c)

76.2

d)

7,620

15.

3.85 hg = _____ cg

a)

38,500

b)

3,850

c)

38.5

d)

0.000385

16.
The students measured length during a science experiement, they got 12 cm. But the actual measurement was 14.25 cm. What was the percent error?
a)
15.79%
b)
18.75%
c)
2.25%
d)
18%
17.
A set of data are all close to each other, but they are not close to the actual value.  This set of data can be described as...
a)
accurate
b)
precise
c)
both precise and accurate
18.
A set of data are all close to each other, and they are close to the actual value.  This set of data can be described as...
a)
accurate
b)
precise
c)
both precise and accurate
19.
How many protons are in Zirconium (Zr) ?
a)
40
b)
91
c)
30
d)
65
20.
A proton is....
a)
A negatively charged subatomic particle
b)
A positively charged subatomic particle
c)
A neutrally charged subatomic particle
d)
The only subatomic particle located in the nucleus
21.
A neutron has a charge of
a)
+2
b)
No charge
c)
-1
d)
+1
22.
What does the atomic mass tell you?
a)
Basically,the number of electrons and protons
b)
The number of neutrons
c)
Basically, the number of protons and neutrons
d)
The number of protons.
23.
An element's identity is determined by the number of
a)
electrons.
b)
protons.
c)
neutrons.
d)
valence.
24.
Which subatomic particles contribute the most to the mass of an atom?
a)
Protons, Neutrons, Electrons
b)
Protons only
c)
Protons and Electrons
d)
Protons and Neutrons
25.
The number of protons is equal to 
a)
the atomic number
b)
the number of neutrons
c)
the energy levels
d)
the periodic table groups
26.

How many neutron are in the atom "K"?

a)

29

b)

19

c)

58

d)

20

27.
What is the atomic mass of Neon?
a)
10
b)
20.18
c)
10.18
d)
30.18
28.
How many electrons does a Copper atom have?
a)
63
b)
29
c)
92
d)
34
29.
What is the atomic number for an element with 41 neutrons and a mass number of 80?
a)
39
b)
41
c)
80
d)
121
30.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

31.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
32.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
33.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
34.
Elements in a ..................have similar chemical properties.  
a)
period
b)
group
c)
row
35.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
36.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
37.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
38.
Which has the greater Electronegativity: 
N or C?
a)
C
b)
N
39.
As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....
a)
decreases
b)
increases
c)
remains the same
d)
none of the above
40.
How many valence electrons are in an atom of K?
a)
3
b)
8
c)
4
d)
1
41.
How many valence electrons are in an atom of Ar?
a)
2
b)
8
c)
4
d)
1
42.
The symbols W, X, Y, and Z represent four elements shown on the outline of a periodic table.
Which element has the highest electronegativity?

a)
W
b)
X
c)
Y
d)
Z
43.
Which of the following is an Alkaline Earth Metal? 
a)
Calcium
b)
Lithium
c)
Phosphorus
d)
Copper 
44.
Which of the following is a transition metal? 
a)
Iron
b)
Oxygen
c)
Neon
d)
Barium
45.
Which of the following is a Noble Gas? 
a)
Krypton
b)
Chlorine
c)
Radium
d)
Gallium
46.
Which of the following is the most reactive group of metals? 
a)
Alkali
b)
Alkaline Earth
c)
Halogen
d)
Transition Metals
47.
Which of the following is the most reactive group of non-metals? 
a)
Alkali
b)
Alkali Earth
c)
Halogen
d)
Noble Gas
48.
Which of the following groups is inert? 
a)
Alkali
b)
Transition Metals
c)
Halogens
d)
Noble Gas
49.
Which of these is a property of metals?
a)
It's malleable
b)
It can't conduct electricity
c)
They are used in food
d)
It's very brittle
50.
Which of these grouping of elements could have the characteristic of brittle?
a)
Metal
b)
Nonmetal
51.
Which of the following is a good conductor of heat?
a)
Metal
b)
Nonmetal
c)
Metalloid
52.
Iron is a good conductor, malleable and magnetic. What type of element is Iron? 
a)
Metal
b)
Nonmetal
c)
Metalloid
d)
Pretty
53.
Silicon is a semiconductor and has properties of both metals and nonmetals. What type of element is Silicon? 
a)
Metal
b)
Nonmetal
c)
Metalloid
d)
Pretty
54.
a)

Metal

b)

Nonmetal

c)

Metalloid

55.
a)

Metal

b)

Nonmetal

c)

Metalloid

56.
a)

Metal

b)

Nonmetal

c)

Metalloid

57.
a)

Metal

b)

Nonmetal

c)

Metalloid

58.
a)

Metal

b)

Nonmetal

c)

Metalloid

59.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
60.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
61.
What is this element?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
62.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
63.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
64.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
65.

What is incorrect about this orbital diagram?

a)

Both arrows in the 2p box should be pointing up

b)

There is nothing incorrect with this diagram

c)

There should be 1 electron (arrow) in the first 2p box and one in the 2nd 2p box

d)

All the arrows should be pointing up.

66.
What is the noble gas configuration for beryllium?
a)
[He]1s2
b)
[He]2s2
c)
[Li]2s1
d)
[Li]2s2
67.
What is the noble gas configuration for Sulfur?
a)
[Ar] 3p4
b)
[He] 3s2 3p4
c)
[Ne] 3s2 3p4
d)
[Na] 3s2 3p4
68.

USE THE PERIODIC TABLE

How many valence electrons does Phosphorus have?

a)

31

b)

5

c)

15

d)

4

69.
How many valence electrons are found in atoms of group 14?
a)
4
b)
3
c)
14
d)
16
70.
What do these isotopes of carbon all have in common?
a)
neutrons & mass number
b)
atomic number and neutrons
c)
atomic number and electrons
d)
protons, atomic number, and mass number
71.
How many neutrons in C-14?
a)
6
b)
7
c)
14
d)
8
72.

Bromine-80 has how many neutrons?

a)

41

b)

42

c)

44

d)

45

73.

Rubidium has two common isotopes, 85Rb and 87Rb. If the abundance of 85Rb is 72.2% and the abundance of 87Rb is 27.8%, what is the average atomic mass of rubidium?

a)

85.468 amu

b)

37 amu

c)

85.6 amu

d)

86.4 amu

74.

There are two primary isotopes found in any sample of copper: copper-63 and copper-65. The isotope 65Cu composes 69.2% of the sample and 63Cu comprises the other 30.8%. Based on this data, what is the atomic mass of copper?

a)

29 amu

b)

63.546 amu

c)

64.4 amu

d)

63.6 amu

75.

A covalent bond forms when atoms ___________ electrons.

a)

gain

b)

share

c)

increase

d)

transfer

76.
Which type of bond has a transfer of an electron from on atom to another?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
77.

Why do atoms bond?

a)

They typically don't bond

b)

To add or take away energy levels

c)

To have a full valence shell.

d)

To have a full inner shell

78.

Ionic bonding is between a

a)

nonmetal and nonmetal

b)

metal and nonmetal

c)

metal and metal

d)

Depends on the situation

79.

CaCl2 is an example of what type of bond?

a)

Covalent

b)

Metallic

c)

Ionic

80.
Which of the following is ionic?
a)
NO2
b)
MgO
c)
CO
d)
CH4
81.

What charge would a potassium (K) ion have?

a)

+1

b)

-1

c)

+2

d)

-2

82.
If an atom loses two electrons what charge will it have?
a)
+ 2
b)
 - 2
c)
+1
d)
-1
83.

13. What elements generally make a covalent bond?

a)

metal and nonmetal

b)

2 or more nonmetals

c)

metal

d)

none of the above

84.

Conducts electricity well when melted or dissolved

a)

Ionic compounds

b)

Covalent compounds

85.

Poor electrical conductivity

a)

Ionic compounds

b)

Covalent compounds

86.

Generally high melting & boiling points

a)

Ionic compounds

b)

Covalent compounds

87.

Generally low melting and boiling points

a)

Ionic compounds

b)

Covalent compounds

88.

What is the charge, or oxidation number, for elements in Group 2?

a)

-2

b)

+2

c)

-3

89.

What is the charge, or oxidation number, for elements in Group 17?

a)

+ 1

b)

-7

c)

-1

90.

What is the charge, or oxidation number, for elements in Group 13?

a)

+ 3

b)

-5

c)

+13

91.
Nonmetals tend to 
a)
gain electrons
b)
lose electrons
92.
Metals tend to 
a)
gain electrons
b)
lose electrons
93.
The proper formula for magnesium hydroxide:
a)
MgOH
b)
Mg2OH
c)
Mg(OH)2
d)
Mg2OH2
94.
Name the following ionic compound: LiNO3
a)
lithium nitrate
b)
lithium III nitrate
c)
lithium nitride
d)
lithium oxide
95.
Name the following ionic compound: BeCl2
a)
beryllium chlorine
b)
beryllium II chloride
c)
beryllium chloride
d)
beryllium dichloride
96.
The chemical formula of lead (IV) nitrate is
a)
PbN₄
b)
PbNO₃₄
c)
Pb(NO₃)₄
d)
Pb₃NO₄
97.
The chemical formula of iron (III)bromide is
a)
FeBr
b)
Fe(III)Br
c)
FeBr₃
d)
Fe₂Br₃
98.
What is the formula for calcium phosphide?
a)
CaP
b)
Ca2P3
c)
Ca3P2
d)
Ca2P
99.
What is the formula for copper(I) sulfate?
a)
CuSO3
b)
CuSO4
c)
Cu2SO3
d)
Cu2SO4
100.
The chemical formula for an ionic compound of potassium and oxygen is
a)
KO.
b)
K2O.
c)
K2O2.
d)
KO2.
101.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

102.

What is the name of the compound Na2(SO4)?

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

103.

Name the ionic compound SnSe2

a)

Tin diselenide

b)

Tin (IV) Selenide

c)

Tin selenide

d)

Tin (II) triselenide

104.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
105.
What is the chemical formula for Tetrasulfur pentoxide?
a)
SO
b)
S4O
c)
S4O5
d)
S5O4
106.
What is the name of C3Cl8 ?
a)
Carbon octachloride
b)
Tricarbon octachloride
c)
Carbon trichloride
d)
Octacarbon trichloride
107.
What is the chemical formula for Nitrogen triiodide?
a)
NI
b)
N3I
c)
NI3
d)
None of these
108.
What is the name of Br6F10 ?
a)
Bromium fluoride
b)
Hexabromine fluoride
c)
Bromium decafluoride
d)
none of the above
109.
What is the name of CO
a)
Carbon oxide
b)
Carbon dioxide
c)
Carbon monoxide
d)
Carbon II oxide
110.
phosphorus trichloride
a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
111.
The chemical formula of sulfur hexabromide is
a)
SBr₆
b)
S₆Br
c)
S(VI)Br
d)
S6Br
112.
Which of the following shows the correct way to balance the chemical equation?
Fe + O2 -> Fe2O3
a)
4Fe + 3O2 -> 2Fe2O3
b)
2 Fe + 3O2 -> Fe2O6
c)
4 Fe + O6 -> 2Fe2O3
d)
None of the options are correctly balanced.
113.
Balance this equation-
__P4 + __O2 --> __P2O3
a)
it is already balanced
b)
2, 1, 3
c)
1, 2, 3
d)
1, 3, 2
114.
Balance this equation
_Al +_HCl --> _H2 +_AlCl3
a)
2, 6, 3, 2
b)
it is already balanced
c)
4, 12, 3, 4
d)
2, 1, 4, 5
115.
Balance this equation.
_CH4 + _O2 --> _CO2 + _H2O
a)
1,2,1,1
b)
2,1,2,1
c)
1,2,1,2
d)
0,2,0,2
116.
What is the type of reaction shown at the top?
a)
Combination
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
117.
KOH + H3PO4 --> K3PO4 + H2O
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
118.
Si + S8 --> Si2S4
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
119.
The following reaction is an example of what reaction type? 
CoCO3 → CoO + CO2
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
120.
What is the left part of a chemical equation called?
H2 + O → H2O
a)
Reactants
b)
Products 
c)
Yields 
d)
Chemical Equation 
121.
What is the right part of a chemical equation called?
H2 + O → H2O
a)
Reactants
b)
Products 
c)
Yields 
d)
Chemical Equation 
122.

Which type of reaction is:

3 Pb + 2 H3PO4 → 3 H2 + Pb3(PO4)2

a)
Synthesis
b)
Single Displacement
c)
Double Displacement
d)
Combustion
123.

Fill in the blank. (Copper has a charge of 2+)

Cu+ AgNO3 → Ag + _____

a)

Cu(NO3)2

b)

CuNO3

c)

CuAg

d)

Cu

124.

Predict the products of this synthesis reaction: H2 + Cl2 →

a)

HCl

b)

H2Cl2

c)

H2Cl

d)

HCl2

125.

Predict the products for the this Single Replacement reaction:

K + HCl →

a)

KCl + H2

b)

KHCl

c)

KH + Cl2

d)

HCl + K2

126.

Predict the products for the this Double Replacement reaction:

AgNO3 + KCl →

a)

AgCl + KNO3

b)

AgK + ClNO3

c)

KAg + NO3Cl

d)

AgCl + 3 KNO

127.

Predict the product of this synthesis reaction:

Al + S₈ →

a)

AlS

b)

AlS8

c)

Al2S

d)

Al2S3

128.

Predict the products for the decomposition of aluminum oxide, Al2O3 →

a)

Al + O2

b)

O + Al2

c)

Al2 + O3

d)

Al + O

129.

What are the products of this reaction:

C2H4 + O2 →

a)

C2O2 + H4

b)

CO2 + H2 + O2

c)

CO + H

d)

CO2 + H2O

130.
In an exothermic reaction, heat is ...
a)
taken in
b)
given out
131.

In an endothermic reaction, heat is ...

a)

taken in

b)

given out

132.
If a chemical reaction is EXOTHERMIC, the temperature would....
a)
Stay the same
b)
Increase
c)
Decrease
133.
The diagram represents which type of reaction
a)
endothermic
b)
exothermic
134.

What type of reaction is this?

a)

Endothermic and Exothermic

b)

Endothermic

c)

Exothermic

d)

Neither Endothermic or Exothermic

135.

Magnesium can be burned in oxygen to produce solid magnesium oxide.

a)

Mg + O2→ MgO

b)

Mg+ O→ MgO

c)

Mg + CO2 → MgO + C

d)

Mg + O2→ Mg2O2

136.

Sodium reacts with chlorine gas to produce sodium chloride.

a)

NaCl→ Cl + Na

b)

Na+ CO2 → NaCO2

c)

Na + Cl2→ NaCl

d)

Na + Cl → NaCl

137.

Iron reacts with solid sulfur to produce iron(II) sulfide powder.

a)

Fe + S → Fe2S

b)

Fe + S → FeS

c)

Fe2 + S→ Fe2S2

d)

Fe + S2 → Fe2S

138.

When the temperature of a substance is lowered, its particles

a)

vibrate more quickly

b)

stop vibrating completely

c)

escape the attractive forces of the other particles

d)

vibrate more slowly

139.
__________ have a definite volume and tend to take the shape of their container. 
a)
solids
b)
liquids
c)
gases
140.

A green powder is heated & a gas is given off while it turns to a black solid. This describes

a)

Physical Change

b)

Chemical Change

c)

Change in State

d)

Change in Temperature

141.

Which of the following could indicate that a chemical change took place?

a)

Change in color

b)

Production of Energy

c)

Formation of Gas

d)

All are correct

142.

The formation of a solid when two liquids combine is called?

a)

Solidification

b)

Freezing

c)

Precipitate

d)

Solubility

143.

Identify what type of change happening in the picture below...

a)

Chemical Change

b)

Physical Change

c)

Endothermic Reaction

d)

Exothermic Reaction

144.

Identify what type of change happening in the picture below...

a)

Chemical Change

b)

Physical Change

c)

Endothermic Reaction

d)

Exothermic Reaction

145.

Identify what type of change happening in the picture below...

a)

Chemical Reaction

b)

Physical Change

c)

Change in State

d)

Change in appearance only

146.

If the chemical properties of a substance remain unchanged & the appearance or shape of an substance changes it is a...

a)

Chemical Change

b)

Physical Change

c)

Both a physical and chemical change.

d)

Neither a physical or chemical change.

147.
What is the Law of Conservation of mass?
a)
Mass is created in a chemical reaction
b)
Mass is created in a physical change
c)
New chemicals formed from a chemical reaction have a larger overall mass than the original reactants
d)
Mass is never created or destroyed
148.

A student mixes 125 grams of sugar, 250 grams of water and 5 grams of flavoring. The solution weighs...

a)

250 grams

b)

375 grams

c)

380 grams

d)

400 grams

149.
A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?
a)
Mg4N3
b)
MgN2
c)
Mg3N2 
d)
MgN
150.
You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.
a)
SO
b)
SO2
c)
SO3
d)
SO4
151.
What is the molecular formula if the empirical formula is CH2O and the molecular molar mass is 180.18?
a)
CH2O
b)
C2H4O2
c)
C4H8O4
d)
C6H12O6
152.
What is the molecular formula for a compound with the empirical formula: K2SO4 and a molecular mass of 696g.
a)
K2SO4 
b)
K8SO16
c)
K8S4O8 
d)
K8S4O16 
153.
Which conversion factor should be used for the following question " How many molecules are there in 4.00 moles of glucose, C6H12O6? 
a)
1 mole = 78.12 g
b)
1 mole = 22.4 L 
c)
1 mol = 6.02x 1023 particles 
d)
more than one
154.
Which conversion factor should be used to solve the following, "How many moles in 28 grams of CO2?"
a)
1 mol = 22.4 L 
b)
1 mol = 44.01 g
c)
1 mol = 6.02x1023 atoms
d)
more than one
155.
Which of the following dimensional analysis setups will correctly convert 27.76g of Li to atoms of Li?
a)
A
b)
B
c)
C
d)
D
156.
How many moles are in 3.01 x 1022 atoms of magnesium?
a)
0.050 moles
b)
1.81 x 1046 moles
c)
5.00 x 1021 moles
d)
5.00 moles
157.
2H2  +   O2  →  2H2O
How many moles of oxygen are consumed if 8 moles H2 are used?
a)
2
b)
4
c)
6
d)
8
158.
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
159.
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
160.
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
161.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
162.
4NH3 + 5O2 --> 4NO + 6H2O
How many grams of NO are formed if 6.30g of ammonia react with 1.80g of oxygen? 
a)
0.37g
b)
0.045g
c)
1.35g
d)
11.1g
163.
Which factors increase the rate of a reaction.
a)
increasing temperature
b)
increasing concentration
c)
increasing surface area
d)
all of these
164.
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 
165.
To slow down a chemical reaction you will do one of the following:
a)
Place the reactants in hot water
b)
Place the products in ice bath
c)
Place the reactants in a ice bath
d)
Keep stirring the reactants with a stirring rod
166.

How could we make this reaction happen more quickly?

a)

Decrease the concentration of the acid

b)

crush the chalk to increase the surface area

c)

Put the test tube in an ice bath

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