С.Ж. АСФЕНДИЯРОВ АТЫНДАҒЫ
ҚАЗАҚ ҰЛТТЫҚ МЕДИЦИНА УНИВЕРСИТЕТІ
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KAZAKH NATIONAL MEDICAL
UNIVERSITY BY S.D.ASPHENDIYAROV
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Department of Chemistry
TESTS FOR FORINERS
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" Confirmed "
Vice-rector for educational work
________________K.A.Tulebaeb
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EXAMINATION TESTS
on the Chemistry
for foreigners
on 2014-2015 academic year
1. Which of the following is an example of a physical change?
-
Ice forming after water is placed in a freezer.
-
A certain liquid is added to a solid, and bubbles of gas form.
-
Adding baking powder to vinegar.
-
A bicycle rusting in the rain.
2. Which of the following changes is a chemical change?
-
Water is boiled.
-
Wood is burned.
-
Aluminum foil is crumpled.
-
Glass is shattered.
3. This is the formula for vinegar CH3CO2H. What are all of the elements found in the formula for vinegar?
-
Hydrogen and Oxygen
-
Carbon, Hydrogen, and Oxygen
-
Carbon and Oxygen
-
Chrome, Cobalt, and Hydrogen
4. Name the three states of matter
-
protons, neutrons, and electrons
-
metals, non-metals, and metalloids
-
solid, liquid, and gas
-
freezing, melting, and evaporation
5. A substance consisting of two elements chemically combined is known as
-
mixture
-
solution
-
element
-
compound
6. A positive charge particle found in the nucleus is called
-
neutron
-
proton
-
electron
-
atom
7. A change from liquid to solid is called
-
melting
-
boiling
-
freezing
-
condensation
8. A change from liquid to gas is known as
-
condensation
-
melting
-
sublimation
-
evaporation
9. A change from gas to liquid is called
-
sublimation
-
evaporation
-
freezing
-
condensation
10. A mixture of sand and iron particles can be separated by
-
distillation
-
magnetism
-
decantation
-
filtration
11. Water is an example of
-
compound
-
element
-
atom
-
mixture
12. One molecule of water is composed of
-
two atoms of oxygen and one atom of hydrogen
-
one atom of oxygen and two atoms of hydrogen
-
two atoms of oxygen and two atoms of hydrogen
-
one atom of oxygen and one atoms of hydrogen
13. The symbol of magnesium is
-
Mn
-
M
-
Mo
-
Mg
14. The symbol of copper is
-
Co
-
Cu
-
C
-
Cp
15. What is the name of the element with symbol Sr
-
sodium
-
silicon
-
scandium
-
strontium
16. An example of alkali metal is
-
K
-
Ca
-
P
-
Cl
-
Au
17. An example of a noble gas is
-
N
-
Na
-
Ne
-
No
18. An example of a hallogen is
-
Ca
-
Co
-
Br
-
S
19. How many valence electron are present in an oxygen atom
-
4
-
5
-
6
-
7
-
8
20. Which of the following pair belong in the same group
-
Na and Ca
-
Si and Al
-
C, Ge
-
S, Cl
21. To get the atomic mass, we sum up the numbers of
-
protons and electrons
-
electrons and neutrons
-
protons and neutrons
-
atomic number and number of protons
22. Which of the following elements will most likely not participate in bonding
-
Si
-
Sr
-
Xe
-
K
23. An atom contains 11 protons, 11 electrons, and 12 neutrons. What is the mass number
-
11
-
12
-
23
-
25
24. Which of the following is an example of a chemical change?
-
Sodium and chlorine combining to form NaCl.
-
CO2 in the form of dry ice evaporating into CO2 gas.
-
Glass that is shattered by a baseball.
-
The condensation of steam into liquid water.
25. Which statement relating to compounds is incorrect.
-
Different compounds can contain the same type of elements.
-
Two different compounds cannot have the exact same type of elements.
-
Compounds are formed from the combination of different elements.
-
Elements combine in compounds in whole number ratios.
26. Which of the following represents a compound with four different types of atoms?
-
H2O
-
NO2
-
Ca(C2H3O2)2
-
Fe(NO3)2
27. Which method would best be used to recover sugar from a solution of sugar and water?
-
boiling the solution to remove the water.
-
filtering the solution with filter paper
-
adding additional sugar to the solution to cause the sugar to precipitate
-
adding alcohol to the solution
28. 50 grams of acetic acid C2H4O2 are dissolved in 200 g of water. Calculate the weight % of the acetic acid in the solution.
-
20%
-
0.069%
-
25%,
-
20%
29. Place the following in the correct order of increasing acidity.
-
HCl< HF< HI< HBr
-
HCl< HBr< HI< HF
-
HI< HBr< HCl< HF
-
HF< HCl< HBr< HI
30. 100 g of ethanol C2H6O is dissolved in 100 g of water. The final solution has a volume of 0.2 L. What is the density of the resulting solution?
-
0.5 g/mL
-
1 g/mL
-
46 g/mL
-
40 g/mL
31. Which particle in the atom has a neutral charge.
-
proton
-
neutron
-
electron
-
nucleus
32. Atoms become ions by losing or gaining which particle?
-
neutron
-
ion
-
electron
-
proton
33. If a neutral atom has 10 protons and 10 electrons, what charge will the resulting ion have if the atom loses 3 electrons?
-
postive
-
negative
-
neutral
-
cannot be determine without the number of neutrons
34. Which term describes a negatively charged ion?
-
positron
-
anion
-
ionic
-
cation
35. The addition of 2 electrons to a neutral atom results in an ion of charge:
-
atoms don’t lose electrons
-
a charge of -2
-
a charge of +2
-
can only be determine by knowing the number of protons in the nucleus
36. Which statement is not true for an ion of sulfur with a charge of -2 (S-2)
-
The number of protons decreased by 2 to form this ion.
-
There are two more electons than protons in this ion.
-
The number of electrons increased by 2 to form this ion.
-
The number of neutrons did not change when this ion was formed.
37. Which of the following elements occurs as a diatomic element.
-
Argon
-
Krypton
-
Fluorine
-
Carbon
38. What is the charge of an ion that has 6 protons, 9 neutrons, and 7 electrons?
-
+1
-
-1
-
+2
-
-2
39. What is the correct maximum number of electrons contained in the s-orbital.
-
2
-
6
-
10
-
14
40. Which of the following electon configurations is correct for the potassium atom?
-
1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d1
-
1s2, 2s2, 2p6, 3s2, 3p6, 3d11
-
1s2, 2s2, 2p6, 3s2, 3p6, 4s2
-
1s2, 2s2, 2p6, 3s2, 3p6, 4s1
41. Which of the following electon configurations is correct for the chlorine atom ?
-
1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p6
-
1s2, 2s2, 2p6, 3s2, 3p5
-
1s2, 2s2, 2p6
-
1s2, 2s2, 2p6, 3s2, 3p6
42. Which electron configuration correctly represents a nonmetal element on the periodic chart?
-
1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p5
-
1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d9
-
1s2, 2s2, 2p6, 3s2, 3p6, 4s1
-
1s2, 2s2, 2p6, 3s2, 3d6
43. Which electron configuration most likely represents an element in the last column of the periodic chart?
-
1s2, 2s2, 2p6, 3s2, 3p6
-
1s2, 2s2, 2p6, 3s2, 3p6, 4s1
-
1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10
-
1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p3
44. Which of the following elements has the most electrons in the outer p-orbital?
-
oxygen
-
Fluorine
-
Sodium
-
Magnesium
45. Which element does not occur as a diatomic molecule?
-
helium
-
fluorine
-
nitrogen
-
bromine
46. Choose the correct formula for the compound: Magnesium Bromide
-
MgBr
-
MgBr2
-
Mg2Br
-
Mg2Br2
47. Choose the correct formula for the compound: Magnesium Sulfide
-
Mg2S2
-
Mg2S
-
MgS2
-
MgS
48. Choose the correct formula for the compound: Lithium Sulfide
-
Li2S2
-
LiS
-
Li2S
-
LiS2
49. Choose the correct formula for the compound: Aluminum Sulfide
-
AlS2
-
Al3S2
-
Al2S3
-
AlS
50. Choose the correct formula for the compound: Barium Hydroxide
-
BaH2
-
BaOH
-
BaOH2
-
Ba(OH)2
51. Choose the correct formula for the compound: Ammonium Carbonate
-
NH4CO3
-
(NH4)2CO3
-
NH4(CO3)2
-
NH3CO3
52. Choose the correct formula for the compound: Barium Phosphate
-
Ba3(PO4)2
-
BaPO4
-
Ba3PO4
-
Ba2(PO4)3
53. Choose the correct formula for the compound: Sulphuric acid
-
H2SO3
-
H3SO3
-
H3SO4
-
H2SO4
54. Choose the correct formula for the compound: Copper (II) Bromide
-
Cu2Br2
-
CuBr2
-
CuBr
-
Cu2Br
55. Choose the correct formula for the compound: Chromium (III) Iodide
-
Cr3I
-
CrI
-
CrI3
-
Cr3I3
56. Choose the correct formula for the compound: Lead (II) Sulfide
-
PbS
-
Pb2S
-
Pb2S2
-
PbS2
57. Choose the correct formula for the compound: Mercury (I) Sulfide
-
HgS
-
Hg2S2
-
HgS2
-
Hg2S
58. Choose the correct formula for the compound: Sulfur Trioxide
-
SO3
-
SO
-
S2O
-
SO2
59. Choose the correct formula for the compound: Silicon Dioxide
-
Si2O2
-
SiO2
-
Si2O
-
SiO
60. Choose the correct name for the compound: BaI2
-
Barium Iodate
-
Barium Diiodide
-
Barium (II) Iodide
-
Barium Iodide
61. Choose the correct name for the compound: AlCl3
-
Aluminum (III) Chloride
-
Aluminum Chloride
-
Aluminum Trichloride
-
Aluminum Tetrachloride
62. Choose the correct name for the compound: CaS
-
Calcium sulfide
-
Calcium Monosulfide
-
Calcium (II) sulfide
-
Calcium (I) sulfide
63. Choose the correct name for the compound: K2SO3
-
Potassium Sulfide
-
diPotassium Sulfite
-
Potassium (II) Sulfite
-
Potassium Sulfite
64. Choose the correct name for the compound: (NH4)3PO4
-
Aluminum Phosphate
-
Ammonium Phosphate
-
Nitrogen TriHydrate Phosphate
-
Triammonium Phosphate
65. Choose the correct name for the compound: NH4Br
-
Nitrous Tetrahydrogen
-
Ammonium Bromide
-
MonobromideAmmonium Bromide
-
Nitrogen Hydrogen Bromine
66. Choose the correct name for the compound: Al2(CO3)3
-
Aluminum Tricarbonate
-
Aluminum Carbonate
-
Aluminum Carbide
-
Ammonium Tricarbide
67. Choose the correct name for the compound: Fe(NO3)2
-
Iron (II) Nitrite
-
Iron (II) Nitrate
-
Iron Nitrite
-
Iron Dinitrite
68. Choose the correct name for the acid: H2SO4
-
Hydro Sulfuric Acid
-
Sulfuric Acid
-
Sulfurous Acid
-
Hydro Sulfurous Acid
69. The type of reaction illustrated by the equation below would best be described as:
2Al(OH)3 → Al2O3 + 3H2O
-
double replacement
-
decomposition
-
combination
-
combustion
70. The type of reaction illustrated by the equation below would best be described as:
2C2H6 + 5 O2 → 2CO2 + 6H2O
-
double replacement
-
decomposition
-
combination
-
combustion
71. For the indicated reaction, choose the products that are most likely to be formed.
K2CO3 →
-
K2C + O2
-
KO + CO2
-
KO2 + CO2
-
K2O + CO2
72. For the indicated reaction, choose the products that are most likely to be formed.
Ag + S →
-
AgS
-
SAg
-
Ag2S
-
S2Ag
73. For the indicated reaction, choose the products that are most likely to be formed.
Fe + Cl2 (assume Fe .. Fe+2) →
-
FeCl2
-
FeCl + Cl
-
FeCl3
-
FeCl
74. For the indicated reaction, choose the products that are most likely to be formed.
Al + Pb(NO3)2 →
-
Al(NO3)3 + Pb
-
Al(NO3)2 + Pb
-
AlPb + NO3
-
PbAl + NO3-
75. For the indicated reaction, choose the products that are most likely to be formed.
K + H2O →
-
K2O + H2
-
KOH + H2
-
KO + H2
-
K2O + H2O
76. For the indicated reaction, choose the products that are most likely to be formed.
K2CrO4 + Pb(NO3)2 →
-
KPb + NO3CrO4
-
K2Pb + NO3CrO4
-
KNO3 + PbCrO4
-
K2(NO3)2 + PbCrO4
77. For the indicated reaction, choose the products that are most likely to be formed.
F2 + BaCl2 →
-
BaF + Cl
-
BaF2 + Cl2
-
Ba + FCl
-
Ba + ClF
78. For the indicated reaction, choose the products that are most likely to be formed.
Na + H2O →
-
NaH + O2
-
NaH2 + O2
-
Na2O + H2
-
NaOH + H2
79. For the indicated reaction, choose the products that are most likely to be formed.
C2H6 + O2 →
-
CH2O
-
CO2 + H2O
-
C6H12O6
-
C6H6 + H2O
80. The molar mass of 1 mole of carbon is:
-
6.0 g
-
12.0 g
-
18.0 g
-
24.0 g
81. The molar mass of one mole of nitrogen gas is:
-
7.0 g
-
14.0 g
-
21.0 g
-
28.0 g
82. The molar mass of HCl is:
-
36.46 g
-
18.00 g
-
72.90 g
-
35.45 g
83. The molar mass of H3PO4 is:
-
8.00 g
-
47.98 g
-
82.00 g
-
98.00 g
84. Equation: Zn + 2HCl → ZnCl2 + H2↑
From the indicated equation, if 5.0 moles of zinc are used with excess HCl, how many moles of the product ZnCl2 would be formed.
-
1.0
-
2.5
-
5.0
-
10.0
85. Equation: Zn + 2HCl → ZnCl2 + H2↑
From the indicated equation, if 5.0 moles of HCl are used with excess Zn, how many moles of the product ZnCl2 would be formed.
-
1.0
-
2.5
-
5.0
-
10.0
86. Equation: Zn + 2HCl → ZnCl2 + H2↑
From the indicated equation, if 5.0 moles of HCl are used with 5.0 moles of Zn, how many moles of the product ZnCl2 would be formed.
-
1.0
-
2.5
-
5.0
-
10.0
87. Equation: Zn + 2HCl → ZnCl2 + H2↑
From the indicated equation, if 5.0 moles of HCl are used with 2.0 moles of Zn, how many moles of the product ZnCl2 would be formed.
-
1.0
-
2.0
-
2.5
-
5.0
88. When a catalyst is added to a system at equilibrium, a decrease occurs in the
-
activation energy
-
heat of reaction
-
potential energy of the reactants
-
potential energy of the products
89. In a chemical reaction, a catalyst changes the
-
potential energy of the products
-
potential energy of the reactants
-
heat of reaction
-
activation energy
90. Which is a property of a reaction that has reached equilibrium?
-
The amount of products is greater than the amount of reactants.
-
The amount of products is equal to the amount of reactants.
-
The rate of the forward reaction is greater than the rate of the reverse reaction.
-
The rate of the forward reaction is equal to than the rate of the reverse reaction.
91. Which procedure will increases the solubility of KCl in water?
-
stirring the solute and solvent mixture
-
increasing the surface area of the solute
-
raising the temperature of the solvent
-
increasing the pressure on the surface of the solvent
92. Given the reaction at equilibrium: 2CO(g) + O2(g) <-> 2CO2(g) When the reaction is subjected to stress, a change will occur in the concentration of
-
reactants, only
-
products, only
-
both reactants and products
-
neither reactants nor products
93. In which reaction will the point of equilibrium shift to the left when the pressure on the system is increased?
-
C(s) + O2(g) ↔ CO2(g)
-
CaCO3(s) ↔ CaO(s) + CO2(g)
-
2Mg(s) + O2(g) ↔ 2MgO(s)
-
2H2(g) + O2(g) ↔ 2H2O(g)
94. Given the reaction at equilibrium: 2 SO2(g) + O2(g) ↔ 2 SO3(g) + heat
Which change will shift the equilibrium to the right?
-
adding a catalyst
-
adding more O2(g)
-
decreasing the pressure
-
increasing the temperature
95. Given the unbalanced equation: Al + O2 = Al2O3. When this equation is completely balanced using the smallest whole numbers, what is the sum of the coefficients?
-
9
-
7
-
5
-
4
96. Which is the correct formula for nitrogen (I) oxide?
-
NO
-
N2O
-
NO2
-
N2O3
97. What is the total number of atoms represented in the formula CuSO4 . 5H2O?
-
8
-
13
-
21
-
27
98. What is the total number of atoms contained in 2.00 moles of nickel?
-
58.9
-
118
-
6.02 x 1023
-
1.2 x 1024
99. What is the percent by mass of oxygen in magnesium oxide, MgO?
-
20%
-
40%
-
50%
-
60%
100. Which solution is the most concentrated?
-
1 mole of solute dissolved in 1 liter of solution?
-
2 moles of solute dissolved in 3 liters of solution?
-
6 moles of solute dissolved in 4 liters of solution?
-
4 moles of solute dissolved in 8 liters of solution?
101. What is the total number of moles of hydrogen gas contained in 9.03 x 1023
-
1.5 moles
-
2.00 moles
-
6.02 moles
-
9.03 moles
102. What is the total number of moles of H2SO4 needed to prepare 5.0 liters of a 2.0 M solution of H2SO4?
-
2.5
-
5.0
-
10
-
20
103. What is the mass in grams of 3.0 x 1023 molecules of CO2?
-
22 g
-
44 g
-
66 g
-
88 g
104. At STP, 32.0 liters of O2 contain the same number of molecules as
-
22.4 L Ar
-
28.0 L of N2
-
32. 0 L of H2
-
44.8 L of He
105. What is the molarity of a KF (aq) solution containing 116 grams of KF in 1.00 liter of solution?
-
1.00 M
-
2.00 M
-
3.00 M
-
4.00 M
106. Given the reaction CH4 + 2O2 → CO2 + 2H2O,
What amount of oxygen is needed to completely react with 1 mole of CH4?
-
2 moles
-
2 atoms
-
2 grams
-
2 molecules
107. What is the total number of moles of hydrogen atoms contained in one mole of (NH4)2C2O2?
-
6
-
2
-
8
-
8
-
4
108. Given the balanced equation: Mg(s) + 2HCL(aq) → MgCl2(aq) + H2(g)
At STP, what is the total number of liters of hydrogen gas produced when 3.00 moles of hydrochloric acid solution is completely consumed?
-
11.2 L
-
22.4 L
-
33.6 L
-
44.8 L
109. What is the oxidation number of chlorine in HClO4?
-
+1
-
+5
-
+3
-
+7
110. Which compound is a salt?
-
Na3PO4
-
H3PO4
-
CH3COOH
-
Ca(OH)2
111. Which compound will conduct an electric current when dissolved in water?
-
NaOH
-
C2H5OH
-
C6H12O6
-
C12H22O11
112. Which statement best describes compounds containing ionic bonds?
-
These compounds generally contain two non-metals.
-
These compounds generally contain a metal and a non-metal.
-
These compounds generally contain two metals.
-
These compounds generally contain two semi-metals.
113. The molecule F2 is best described by which statement?
-
This is a slightly polar covalent molecule.
-
This is a very polar covalent molecule.
-
This is a very polar ionic molecule.
-
This is a non-polar covalent molecule.
114. The molecule H2O is best described as:
-
Ionic molecule
-
Nonpolar covalent molecule
-
Polar covalent molecule
-
Nonpolar Ionic molecule
115. What is the expected shape of the molecule CH4?
-
triangular
-
angular
-
triganol pyramidal
-
tetrahedral
116. The molar volume of any gases at STP is defined as:
-
100.0 liters
-
22.4 mL
-
22.4 liters
-
1.00 liters
117. Which type of reaction is occurring when a metal undergoes corrosion?
-
oxidation-reduction
-
neutralization
-
polymerization
-
saponification
118. What is the oxidation number of carbon in NaHCO3?
-
+6
-
+2
-
-4
-
+4
119. Which formula represents a salt?
-
KOH
-
KCl
-
CH3OH
-
CH3COOH
120. Which element is present in all organic compounds?
-
carbon
-
nitrogen
-
oxygen
-
phosphorous
121. Which compounds are isomers?
-
1-propanol and 2-propanol
-
methanoic acid and ethanoic acid
-
methanol and methanal
-
ethane and ethanol
122. Which statement explains why the element carbon forms so many compounds?
-
Carbon atoms combine readily with oxygen.
-
Carbon atoms have very high electronegativity.
-
Carbon readily forms ionic bonds with other carbon atoms.
-
Carbon readily forms covalent bonds with other carbon atoms.
123. Which polymers occur naturally?
-
starch and nylon
-
starch and cellulose
-
protein and nylon
-
protein and plastic
124. What products are obtained with CH4(g) burns completely in an excess of oxygen?
-
CO and H2O
-
CO and C
-
CO2 and H2O
-
CO2 and CO
125. Which formula represents butane?
-
CH3CH3
-
CH3CH2CH3
-
CH3CH2CH2CH3
-
CH3CH2CH2CH2CH3
126. A hydrocarbon molecule is considered to be saturated if the molecule contains
-
Single covalent bonds, only
-
A double covalent bond, only
-
A triple covalent bond
-
Single and double covalent bonds
127. What is the name of the compound that has the molecular formula C6H6?
-
butane
-
butene
-
benzene
-
butyne
128. In which pair of hydrocarbons does each compound contain only one double bond per molecule?
-
C2H2 and C2H6
-
C2H2 and C3H6
-
C4H8 and C2H4
-
C6H6 andC7H8
129. The reaction CH2CH2 + H2 → CH3CH3 is an example of
-
substitution
-
addition
-
esterification
-
fermentation
130. Which compound is a saturated hydrocarbon?
-
ethane
-
ethene
-
ethyne
-
ethanol
131. What type of reaction is CH3CH3 + Cl2 → CH3CH2Cl + HCl?
-
an addition reaction
-
a substitution reaction
-
a saponification reaction
-
an esterification reaction
132. What is the maximum number of covalent bonds than an atom of carbon can form?
-
1
-
2
-
3
-
4
133. Which class of organic compounds can be represented as R-OH?
-
acids
-
alcohols
-
esters
-
ethers
134. Which molecule contains a total of three carbon atoms?
-
2-methylpropane
-
2-methylbutane
-
propane
-
butane
135. What substance is made up of monomers joined together in long chains?
-
ketone
-
protein
-
ester
-
acid
136. Which compound is an organic acid?
-
CH3OH
-
CH3OCH3
-
CH3COOH
-
CH3COOCH3
137. Which organic compound is classified as a primary alcohol?
-
Ethylene glycol
-
Ethanol
-
Glycerol
-
2-butanol
138. For ethyne: C2H2
What is the total number of electrons shared between the carbon atoms?
-
6
-
2
-
3
-
4
139. Which set contains one natural polymer and one synthetic polymer?
-
Cellulose and Starch
-
Polyethylene and Nylon
-
Protein and Starch
-
Protein and Nylon
140. Aldehydes can be synthesized by the oxidation of
-
Primary alcohols
-
Secondary alcohols
-
Organic acids
-
Inorganic acids
141. Given the reaction: C2H2 + 2H2 → C2H6
This reaction represents:
-
Substitution
-
Addition
-
Esterification
-
Saponification
142. Which pair of names refers to the same compound?
-
Ethyne and Acetylene
-
Ethyne and Ethene
-
Ethane and Acetylene
-
Ethane and Ethene
143. A condensation polymerization reaction is best described as the
-
Joining of monomers by the removal of oxygen
-
Joining of monomers by the removal of water
-
Oxidation of a hydrocarbon by oxygen
-
Oxidation of a hydrocarbon by water
144. Which formula represents a ketone?
-
CH3COOH
-
C2H5OH
-
CH3COCH3
-
CH3COOCH3
145. The bond between hydrogen and oxygen in a water molecule is classified as
-
Ionic and Nonpolar
-
Ionic and Polar
-
Covalent and Nonpolar
-
Covalent and Polar
146. What is the total number of hydrogen atoms required to form 1 molecule of C3H5(OH)3?
-
1
-
5
-
3
-
8
147. A compound that can act as an acid or a base is referred to as
-
A neutral substance
-
An amphoteric substance
-
A monomer
-
An isomer
148. Which compound is an electrolyte?
-
CH3OH
-
CH3COOH
-
C3H5(OH)3
-
C12H22O11
149. Which organic compound is classified as an acid?
-
CH3CH2COOH
-
CH3CH2OH
-
C12H22O11
-
C6H12O6
150. During fractional distillation, hydrocarbons are separated according to their
-
Boiling points
-
Melting points
-
Triple points
-
Saturation points
Discussed and confirmed at a meeting of the Department of Chemistry,
16.06.14 Protocol № 11
Head. Department of Сhemistry,
professor N.U.Aliev
Developers:
Nechepurenko E.V.
(in.tel.7219)
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