Download Type Of Chemical Reaction

Chemistry Final Exam Review 2015-16
Identify the following types of equations and balance the equations:
1.
Na + Cl2
2NaCl
2.
CH4 + 2O2
3.
2H2O
4.
2NaCl + CaCO3
5.
2Li + 2H2O
Synthesis
CO2 + 2H2O
2H2 +
Combustion
O2
Decomposition
CaCl2 + Na2CO3
2LiOH +
Double replacement
H2
Single replacement
6. The symbol for a gas in a chemical reaction is? Solid? Liquid? Solution?
g, s, l, aq
7. ______ are the substances to the left side of the arrow in a chemical reaction
Reactants
8. _________ are the substances to the right of the arrow in a chemical reaction
Products
9. A skeleton equation is a chemical equation that is not __________.
Balanced
10. ________ is a small number written to the right and slightly lower than the symbol
Subscript
11. _______ is a small number written above and to the right of the symbols
Superscript/oxidation
number
12. Which number is the coefficient in the following: 3H2O? How many atoms of each element are in
the compound?
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3/ 6 H/ 3 O
13. Which law states that the number of each type of atom in the reactants must equal the number of
atoms of each type in the product?
Law of Conservation of
Mass
14. How many atoms of neon are in a mole of Neon?
6.02 x 1023
15. How many formula units of salt are in a mole of NaCl?
6.02 x 1023
16. How many molecules of H2O are in a mole of H2O?
6.02 x 1023
17. How many Twinkies® are in a mole of Twinkies®?
6.02 x 1023
18. What is the molar mass of H3PO4
98 g/mol
19. How many moles are there in 30 grams of H3PO4?
0.3 mol
20. How many grams are in 5.6 moles of C6H6?
437 g
21. How many liters of gas are in a mole of O2 at STP?
22.4 L
22. Given the balanced equation:
2 C2H2 + 5 O2 -----> 4 CO2
+ 2 H2 O
5:2
4:2 or 2:1
What is the molar ratio of Oxygen to Water?
What is the molar ratio of carbon dioxide to C2H2?
23. Identify the diatomic molecule : F2 or MgO
F2
24. Using the balanced equation, 2H2 + O2 --> 2H2O, how many grams of oxygen are required to
produce 8 moles of water?
128 grams O2
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25. Given
P4 +
3O2 -->
2P2O3, balance the equation.
How many moles of phosphorus are required to react with 6 moles of oxygen?
2 moles P4
26. How many grams are there in 2 moles of C6H12O6?
360 g
27. Determine the molar mass of hydrogen gas
2.02 g
28. How many moles of Al are in 2.16 mol of Al2O3?
4.32 mol Al
29. Determine the mass in grams of the following: 1.25 mol Ca3(PO4)2
388g Ca3(PO4)2
30. How many moles of H2 and N2 can be formed by the decomposition of 0.145 mol of NH3?
0.0725mol N2 and
0.218mol H2
31. Given: 3Cu(s) + 8HNO3(aq) --> 3Cu(NO3)2(aq) + 2NO(g) + 4H2O(aq)
30.31g HNO3
How many grams of HNO3 are needed to react with 11.45g of Cu?
32. According to the ______________ theory of ______________, the particles in a gas move rapidly,
the particles in a gas are relatively far apart, the particles in a gas move independently of each other.
Kinetic Theory of Gases
33. At what temperature does the motion of particles theoretically ceases?
0.0 K = – 273 0C
34. What phase of matter has no definite shape nor definite volume?
Gas
35. What device that is used to measure atmospheric pressure?
Barometer
36. The average kinetic energy of particles of a substance is directly proportional to the ____________
of a substance.
37. Water could be made to boil at a temperature higher than 100 °C by:
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Temperature
Increasing the air
pressure above the water
38. The melting point of the substance is the same as the:
Freezing Point
39. As you climb a mountain, atmospheric pressure: (Increases or Decreases)
Decreases
40. Liquids compared to gases have ____(stronger or weaker)____ intermolecular attractions.
Stronger
41. When vapor pressure of a liquid is equal to the external pressure on the liquid, _________ occurs.
Boiling
42. The escape of high energy molecules from the liquid phase below the boiling point is called?
Evaporation
43. During the process of freezing, a liquid
Loses Energy
(Gains or Loses)
energy.
44. What phase transition of matter goes directly from the solid phase to the gas phase without passing
through an intermediate liquid phase? (Hint: Dry Ice)
Sublimation
45. A _______________ diagram gives the conditions of temperature and pressure at which a
substance exists as a solid, liquid & gas.
Phase
46. Name 3 properties of solids.
Definite Shape, High
Density & definite
Volume
47. What causes gas pressure?
Gas particles colliding
over a given area of its
container.
48. Name three units for pressure.
Pa, atm., Torr, mm Hg
49. _____ is the empty space with no particles and no pressure.
Vacuum
50. Temperature at which the vapor pressure of the liquid is just equal to the external pressure on the
liquid is
Boiling point
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51. For a fixed volume of gas, if the temperature increases the pressure will
increase
52. The reduction in volume of matter under pressure is a physical property called ______________.
compressibility
53. Pressure and volume are _________ proportional.
inversely
54. Temperature and volume are ______________ proportional
directly
55. Temperature and pressure are ______________ proportional
directly
56. The total pressure exerted by a mixture of gases is equal to __________
the sum of the partial
pressures of the
component gases?
57. How can you increase the pressure of a gas in a closed container?
Add more gas, increases
the temperature, decrease
the volume
58. The ideal gas law is the only gas law that lets you calculate ________.
The amount (moles) of
gas.
59. What is the equation to convert °C to Kelvin?
K = °C +273
60. What does STP stand for?
Standard Temperature
and Pressure (0 °C and 1
atm)
61. A given mass of oxygen occupies 280 ml when the pressure is 400 Pa. If the temperature is kept
constant, the volume that the gas will occupy when the pressure changes to 350 Pa is?
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320 mL
62. Why does water have high surface tension?
Hydrogen bonding
between water molecules
63. A compound that does conduct an electric current in aqueous solution or when molten is called a(n)
electrolyte
64. Why is the density of ice less than the density of water?
Hydrogen bonding in the sol’n
results in a honey comb
structure which has a lot of
empty space so density solid is
less than liquid
65. _________ is the inward force or pull that tends to minimize the surface area of a liquid.
Surface tension
66. The scattering of visible light in all directions by colloids or suspensions is called the ____.
Tyndall Effect
67. Which substance will conduct electricity solid NaCl or a solution of NaCl?
Solution of NaCl
68. Does water have a low vapor pressure? Explain.
Yes, because of hydrogen
bonding
69. Which of the following do not exhibit the Tyndall effect? (solutions, colloids, or suspensions)
solutions
70. Two liquids that a mutually soluble in each other are ______________
miscible
71. As the pressure increases, the solubility of ___________ in liquids increases.
gases
72. A(n) ___ solution contains the maximum amount of solute for a given quantity of solvent at a
constant temperature and pressure
Saturated solution
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73. A(n)______ solution is a solution that contains less solute that a saturated solution at a given
temperature and pressure
Unsaturated solution
74. A(n) ________ solution contains more solute that it can theoretically hold at a given temperature
supersaturated
75. What three things can you do to a solute to dissolve faster in a solvent?
Increase temperature, stir
solution, increase surface
area (crush substance
into a powder)
76. _____ is the characteristic ion for all bases
OH-
77. _____ is the characteristic ion for all acids
H+ or H3O+
78. Bases taste_______
bitter
79. Acids taste __________
sour
80. A __________ is slippery to the touch.
base
81. Fruits are considered (acidic or basic)
acidic
82. What is the formula for hydrobromic acid?
HBr
83. What is the formula for Hydrochloric acid?
HCl
84. What is the name of the following acid HNO2
Nitrous acid
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85. What is the name of HNO3
Nitric acid
86. An acid/base reaction will always yield what two products?
Water + salt
87. The pH range for acids is
0 to < 7
88. In a neutral solution, what two ions are equal in concentration? What is the pH?
H+ and OH- pH=7
89. The pH range of bases is
> 7 14
90. _____ are substances that may change color in the presence of an acid or base
indicators
91. Si, Ge and B are classified in what general group on the periodic table.
Metalloids
92. A substance has luster, conducts electricity and forms positive ions. Is it a metal or a non metal?
metal
93. Copper melting is an example of what type of change?
Physical
94. What types of sublevels are in the 4th energy level?
S, p, d, f
95. Any chemical reaction that releases energy is called
Exothermic
96. Give some examples of a chemical change
Souring milk, rusting
iron, burning paper,
baking a cake, eating
food
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97. Color, boiling point, solubility and hardness are what type of properties
Physical
98. What does the law for conservation of mass say?
States that mass cannot
be created or destroyed,
just changes form
99. Draw a graph that illustrates a direct relationship
100. Define density.
Mass per unit of
volume
101. If you have 10 grams of a substance and it occupies 20 ml, what is its density?
10 grams/ 20 ml. = .5
g/ml
102. Changing the number of _____ in an atom will change its identity.
Protons
103. Iron rusting is an example of which type of change (Chemical or physical)?
Chemical
104. A boron atom has 5 protons, 6 neutrons and 5 electrons. What is the mass number of boron?
11 amu
105. As the atomic number of the elements increase, what happens to the number of electrons in a
neutral atom?
It also increases
106. What is the mass of one mole of sodium hydroxide?
NaOH
Na= 23 ; O=16; H=1=
40AMU
107. How many moles are there in 500g of HCl?
13.7 moles
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108. You have 0.5 moles of MgCO3. How many grams do you have?
42g
109. How many molecules are there in 2 moles of N2 gas?
1.24 X 1024 molecules
110. An atom is identified by its _____________________.
Atomic number
111. Isotopes of the same element have different _______________.
Numbers of neutrons
112. What is the formula for calcium hydroxide?
Ca(OH)2
113. Name the compound As2O5.
Diarsenic pentaoxide
114. Name the compound AgCl?
Silver chloride
115. Name the compound K NO3
Potassium nitrate
116. Write the formula for Iron (II) chloride.
FeCl2
117. What is the formula for diphosphorous pentasulfide?
P2S5
118.Significant figures are all the numbers that are known with certainty and one that is _________
Uncertain
119. How many significant figures are there in the following : 7001g, .009ml, 7.07 Km?
4, 1, 3
120. How many electrons can the p sublevel hold?
6
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Chemistry Review Part 2
1. Phase Change Diagram of water
E
100°C
T
E
M
P
E
R
A
T
U
R
E
D
C
0°C
B
A
Heat Energy
Answer the following questions by looking at the graph (1 point each)
a.
What happens to the temperature at section B?__remains constant_________
b.
What is happening to the water at section D?___boiling__________
c.
For what section(s) does the temperature increase as energy is added?_____A, C, and E__ ____
2. Moles
a. Is nitrogen a diatomic molecule? (Yes or No)
Yes
b. What is the molar mass of nitrogen? 28 g/mol
c. What mass of nitrogen gas would you need to have 10 moles of nitrogen gas? 280 grams
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3. Balance each of the following chemical equations and write the name of the type of chemical reaction on the line provided.
(combustion, synthesis, decomposition, single replacement, double replacement)
Type Of Chemical Reaction
a.
C2H4
+
3 O2 
2CO2 +
2H2O
a. Combustion
b.
Cu(ClO3)2 → CuCl2
c.
FeCl3
d.
FeS +
2HCl →
e.
AlBr3 +
3K  3KBr + Al
f.
N2
+
3H2 →
2NH3
f. Synthesis
g.
P4 +
5O2 
P4O10
g. Synthesis
h.
Al2(SO4)3 + 3Cu →
i.
CH4
j.
Al2(SO4)3
+ 3KOH 
+ 2O2 →
3O2
+
b. Decomposition
Fe(OH)3
H2S
CO2
+ 3Ca(OH)2
+
+
c. Double Replacement
FeCl2
d. Double Replacement
e. Single Replacement
3CuSO4 +
+
3KCl
2Al
h. Single Replacement
2H2O
i. Combustion
 3CaSO4 + 2Al(OH)3
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j. Double Replacement
4. Gas Laws
Calculations: Please list all information give, the equation used, number plugged into equation and the answer with units!
P1V1 = P2V2
T1V2 = T2V1
a. When the temperature of a gas is held steady and the pressure is 10 Pa for 520 ml, what will be the pressure for 260 ml?
2 ml
𝑷 𝟏 𝑽𝟏 = 𝑷 𝟐 𝑽 𝟐
𝑷𝟏 = 𝟏𝟎 𝑷𝒂
𝑽𝟏 = 𝟓𝟐𝟎 𝒎𝑳
𝑷𝟐 =?
𝑽𝟐 = 𝟐𝟔𝟎 𝒎𝑳
𝑷𝟏 𝑽𝟏 (𝟏𝟎𝑷𝒂 )(𝟓𝟐𝟎𝒎𝑳)
𝑷𝟐 =
=
= 𝟐𝟎𝑷𝒂
𝑽𝟐
𝟐𝟔𝟎 𝒎𝑳
b. The volume of a gas at 50 K is 25 ml. What will be the temperature of the gas at 50 ml?
100 K
𝑻𝟐 𝑽𝟏 = 𝑻𝟏 𝑽𝟐
𝑻𝟏 𝑽𝟐 (𝟓𝟎𝑲)(𝟓𝟎𝒎𝑳)
𝑻𝟏 = 𝟓𝟎𝑲
𝑻𝟐 =
=
= 𝟏𝟎𝟎𝑲
𝑽𝟏
𝟐𝟓 𝒎𝑳
𝑽𝟏 = 𝟐𝟓 𝒎𝑳
𝑻𝟐 =?
𝑽𝟐 = 𝟓𝟎 𝒎𝑳
c. If you have 3L of a gas at 300K and 4 atm, how many moles do you have?
V=3L
n=PV/RT = [(4atm)(3L)]/[(0.0821)(300K)]
T=300K
n=0.487 moles
P=4atm
R=0.0821
n=?
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5. Phase diagrams
a. What is the pressure and temperature of carbon dioxide at the critical
point?
Pressure = ___72.9 atm_______
Temperature = ____31°C_______
b.
At 1 atmosphere and room temperature (25C), would you expect solid
carbon dioxide to melt to the liquid phase, or sublime to the gas
phase? _______sublime to gas _____________________
c.
Some industrial processes require carbon dioxide. The carbon dioxide is
stored on-site in large tanks as liquid carbon dioxide. Assuming you have
carbon dioxide at STP, what could you do to liquefy it? Increase the pressure
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6.
Formula
Lewis dot
Lewis stick structure
CH4
H2O
CH3Br
Br
SO3
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7. Solubility Curve: Use the following curve to answer questions
a. Which of the curves in this figure represents a gas? NH3
b. Which substance is the most soluble at 50 °C? KI
c. How many grams of KNO3 are needed in order to make a saturated solution of KNO3 in
100 g of H2O at 50 °C? 80 g
d. A solution of 90 grams of NaNO3 in 100 g of H2O at 90 °C can be considered?
unsaturated
e. If the solution in problem d was cooled to 10 °C, what would this solution be?
supersaturated
f. If 20 grams of KClO3 was added to 100 grams of H2O at 50 °C, this solution would be
considered?
saturated
g. You start with a saturated solution of NH3 in 100 grams of water at 10 °C. How many
grams of NH3 gas would bubble out of the solution if you raise the temperature to 90 °C? approx 60 grams
70g-10g=60g
h. What is the independent variable on this graph? Temperature
i. What is the dependent variable on this graph? Solubility
j. Which substance is the most soluble at all temperatures? KI
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8. KOH reacts with enough HCl to form KCl and H2O
a. Write and balance the above reaction
KOH + HCl → KCl + H2O
b. If you start with 50.0g of KOH and enough HCl calculate the amount of KCl that theoretically should be produced
50.0g KOH x
1𝑚𝑜𝑙 𝐾𝑂𝐻
56.11𝑔
1 𝑚𝑜𝑙 𝐾𝐶𝑙
74.55𝑔
× 1 𝑚𝑜𝑙 𝐾𝑂𝐻 × 1𝑚𝑜𝑙 𝐾𝐶𝑙 = 66.4𝑔𝐾𝐶𝑙
c. If 60.0g of KCl is actually produced what is the percent yield of this reaction?
T=66.4g
A=60g
%Y=A/T x 100
60g/66.4 x 100 = 90.4%
9. Acids \ Bases
Name 5 characteristics of an Acid:
Taste sour
Produce H+ ions in water
React with metals to form H2
Electrolytes
React with hydroxides to form water and salt
Name 5 characteristics of a Base:
Bitter
Slippery
React with acids to form water and salt
Can be electrolytes
Produce OHPage 17 of 20
The number range of the pH scale is: ____0____ to ___14_____.
A strong acid is typically a pH of what number? _____0_____
A strong base is typically a pH of what number? _____14_____
The ion that accounts for Acidity is: _____H+_or H3O+____
The ion that accounts for Basic is: ____OH-____
A neutral pH is what number: ______7______
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10. Graph the data correctly, tell the type of relationship that
exists and then answer questions based on the data provided.
Mass (g)
56.5
169.5
271.2
587.6
723.2
Mass vs. Volume
Volume (mL)
5
15
24
52
64
750
720
690
660
630
600
570
540
510
Mass 480
a. Calculate the slope of this graph.
(g) 450
420
723.2  56.5  666.7  11.3g / ml
Slope 
390
64  5
59
360
b. What is the equation for density and how does it relate to the 330
300
slope of this graph?
270
240
Density = mass/volume
210
180
150
c. Using the data table below identify which substance was involved
120
in this experiment?
90
60
30
Substance
Density (g/mL)
Copper
8.92
Lead
11.3
Gold
19.3
5 10 15 20 25 30 35 40 45 50 55 60 65
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Volume
(mL)
11.
Diphosphorus pentachloride
Copper (I) carbonate
Carbonic acid
Aluminum hydroxide
phosphorus trioxide
Barium chloride
P2Cl5
Cu2CO3
H2CO3(aq)
Al(OH)3
PO3
BaCl2
12.
H2O
KBr
(NH4)3PO4
CO2
CF4
HClO3(aq)
Dihydrogen monoxide
Potassium Bromide
Ammonium phosphate
Carbon dioxide
Carbon tetrafluoride
Chloric acid
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