good conductivity in solid state
solubility in polar solvents
ww
1
Ionic solids are characterized by
(a)
low melting points
(b)
(c)
high vapour pressure
(d)
2 Amorphous solids.
(a)
have sharp melting points
(c)
have perfect arrangements of atoms
bio
w.i
(b) undergo clean cleavage when cut with knife
(d) can presses small regions of orderly
arrangements of atoms
3
The force of attraction between the atoms of helium is
(a)
hydrogen bonding
(b)
coordinate covalent bond
(c)
covalent bond
(d)
london dispersion force
4 Which of the following is a pseudo-solid
(a)
CaF2
(b)
Glass
(c)
NaCl
(d)All
5 Diamond is a bad conductor because
(a)
It has a tight structure
(b)
It has a high density
(c)
There is no free electron present in the crystal of diamond to conduct electricity
(d)
None of the above
6
The weakest intermolecular for a
(a) dipole–dipole force
(b) electrostatic force between ions
(c) ion–dipole force
(d) dipole–induced dipole force
7
In liquids intermolecular forces are
(a)
very weak
(b) very strong
(c) reasonably strong
(d) ion–dipole force
kaa
8
Values of heat of vaporization for liquids, with strong dipole–dipole forces will be
(a) very high
(b) very low
(c) reasonably high
(d)
negligible
9
Instantaneous dipole–induced dipole force is also called
(a)
dipole force
(b)
london dispersion
(c)
hydrogen bonding
(d)
none of the above
re.c
10 Down the group polarizability generally
(a)
increases
(b)
decreases
(c)
remains constant
(d)
do not follow a regular trend
11 Trend of boiling points of halogens from fluorine to iodine
(a)
decreases
(b) increases (c) remains constant
is that it.
(d) negligible
12 Molecules of hydro carbons with large chain lengths experience
(a)
repulsive forces
(b)
strong attractive force
(c)
weaker attractive forces
(d)
no attractive force
om
13 Hydrocarbons which generally have high molecular masses exist is.
(a)
solid form
(b)
liquid form (c)
vapour form
(d)
gaseous form
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Exceptionally low acidic strength of HF is due to
strong polar bond
(b)
small size of fluorine
strong hydrogen bonding (d)
Vander Waal’s forces
Long chain of amino acids are coiled about one another into spiral by.
covalent bond
(b)
ionic bond
(c) hydrogen bond (d) Vander Waal’s forces
Evaporation of water is possible at
100oC
(b)
0oC
(c) at all temperatures
(d)above 100oC
Boiling point is low for liquid with
high vapour pressure at given temperature
(b)low vapour pressure at a given temperature
very high vapour pressure
(d)
very low vapour pressure
w.i
ww
14
(a)
(c)
15
(a)
16
(a)
17
(a)
(c)
18 At equilibrium rate of evaporation and rate of condensation
(a) become very high
(b) become very low (c) can never be equal
(d)become equal
19 In an open system vapour pressure of water at 100oC at sea level is
(a) 700 mm of Hg
(b) 760 mm of Hg (c) 670 mm of Hg
(d) 1000 mm of Hg
bio
20 Molar heat of vaporization of water is
(a) 140.6 kJ/mol (b) 14.06 kJ/mol (c)18 kJ/mol
(d)40.6 kJ/mol
21 When external pressure is 23.7 torr boiling point of water is
(a)
100oC
(b)
200oC (c)
98oC
(d)
25oC
22
kaa
Distillation under very reduced pressure is called
(a)
fractional distillation
(b)
(c)
vacuum destructive distillation
(d)
23 Water may boil at 120oC when external pressure is
(a) 760 torr
(b) 100 torr
(c)1489 torr
distillation
destructive distillation
(d)
700 torr
form at its melting
re.c
24 Amount of heat absorbed when one mole of solid melts into liquid
point is called
(a)
molar heat of sublimation
(b)
heat of vaporization
(c)
latent heat of fusion
(d)
molar heat of fusion
25 Ethanol is much more soluble in water than ethyl ethanuate which one of the
following statement correctly account for this
(a)
ethanol is polar molecule but ethyl ethanoate is non–polar
(b)
ethanol is non polar molecule but ethyl ethanoate is polar
(c)
a hydrogen bond is formed between H–atom of the OH group in ethanol and O–atom
of water molecule
d)
a hydrogen bond is formed between the H–atom of the OH group in ethanol and
hydogen of the water molecule
om
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33 Isomorphous crystals show
(a)
same chemical properties
(c)
same crystalline form
kaa
bio
w.i
ww
26 The boiling point of a liquid will be
(a)
lower at high altitude
(b)
higher at high altitude
(c)
same at sea level and high altitudes (d)
equal to atmospheric pressure
27 The process in which liquids can be made to boil at low temperature is called
(a)
vacuum distillation
(b)
destructive distillation
(c)
distillation
(d)
vacuum destructive distillation
28 Why is the boiling point of methane greater than that of neon
(a)
a molecule of methane has a greater mass
(b)
a molecule of methane has more electrons than a molecule of neon
(c)
the molecules of methane have stronger intermolecular forces than those of neon
(d)
the molecule of methane is polar but that of neon is not
29 The amount of heat required to vaporize one mole of a liquid at its boiling point is called
(a)
molar heat of vaporization
(b)
molar heat of fusion
(c)
latent heat of fusion
(d)
molar heat of sublimation
30 Which of the elements in its crystalline form will have lowest enthalpy change of vaporization
(a)
chlorine
(b)
argon (c)
phosphorous (d)
silicon
31 Crystals show variation in physical properties depending upon the direction. The property called
(a)
isomorphism
(b)
polymorphism (c)
anisotropy (d)
isotropy
32 Certain melt to a turbid liquid phase with properties of liquids as well as some degree of order like
solid. Such turbid liquids are called
(a)
anorphous solid
(b)
vitreous solid (c)
crystalline solid
(d)
liquid crystal
(b)
(d)
same physical properties
same melting point
Covalent solids are composed of
ions
(b)
different molecules
(c) neutral atoms
(d) any of the above
Carbon atoms of diamond are
sp hybridized
(b) sp2 hybridized (c) sp3 hybridized
(d)
unhybridized
Molecular crystals are generally
hard
(b) soft (c) unstable
(d)stable
Ionic crystals are
hard
(b)
soft (c)
brittle
(d)
amorphous
om
37
(a)
38
(a)
39
(a)
40
(a)
re.c
34 Existence of an element in more than form is known as
(a)
allotropy (b)
isomorphism
(c)
isotropy
(d)
none of these
35 Crystalline forms of the same, substance can coexist in equilibrium with each other at its
(a)
melting point (b) transition temperature (c)boiling point (d) none of these
36 Crystal lattice of substance can be catagorised into
(a)
five types
(b)
seven types (c)
six types
(d)
none of these
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41.
Which statement correctly describes Hess's Law?
a
The enthalpy of all reactants in their standard states is defined as zero.
Enthalpy changes may only be calculated if one or more of the reactants
is an element.
c
The enthalpy change of a reaction is independent of the route taken.
d
e
42.
Which one of the following statements best describes the standard enthalpy of
formation of any element?
a
The value of
H°f(element) depends on temperature.
b
The value of
H°f(element) is zero only for elements in the solid state.
c
The value of
H°f(element) is zero for any element in the standard state.
d
The value of
H°f(element) is zero only at absolute zero temperature.
e
The value of
H°f(element) depends on S° for that element.
Under which circumstances would a reaction be non-spontaneous at all
temperatures?
a
ΔH° negative and ΔS° positive
b
ΔH° negative and ΔS° negative
c
ΔH° positive and ΔS° negative
d
ΔH° positive and ΔS° positive
e
It is impossible to tell without calculating ΔG°.
kaa
In which direction will the following equilibrium shift if a solution of CH3CO2Na
is added?
CH3CO2–(aq) + H+(aq)
CH3COOH(aq)
A
shift to the right (more products)
B
shift to the left (more reactant)
C
no change
D
cannot be predicted
re.c
45.
Exothermic reactions occur quickly, endothermic reactions occur slowly.
bio
44.
The enthalpy change of a reaction may only be calculated at 1 atm
pressure and 25 °C.
w.i
43.
ww
b
In which of the following acid / base titrations, can we NOT determine the
equivalence point in an accurate manner?
strong acid / strong base
b
strong acid / weak base
c
weak acid / strong base
d
weak acid / weak base
om
a
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46. What is the expression for Ka for the following reaction?
CH3CO2–(aq) + H+(aq)
CH3COOH(aq)
A
Ka = [CH3CO2–(aq)][H+(aq)]/[CH3COOH(aq)]
B
D
47.
ww
C
Ka = 2[H+(aq)]/[CH3COOH(aq)]
Ka = [H+(aq)]2/[CH3COOH(aq)]
Ka = [CH3COOH(aq)]/[H+(aq)]2
Rank the following 1 M water solutions in order of decreasing freezing point.
NaCl
glucose
CaCl2
CH3COOH
lowest freezing point
w.i
highest freezing point
Na3PO4
a NaCl > glucose > CaCl2 > CH3COOH > Na3PO4
b
glucose > NaCl > CaCl2 > CH3COOH > Na3PO4
c glucose > NaCl > CH3COOH > CaCl2 > Na3PO4
glucose > NaCl > CH3COOH > Na3PO4 > CaCl2
e
glucose > CH3COOH > NaCl > CaCl2 > Na3PO4
bio
48.
d
Arrange the following species from left to right in order of increasing radius.
Na, Mg, F–, Na+, Mg2+
a
F– < Mg2+ < Na+ < Mg < Na
b Na+ < Mg2+ < F– < Mg < Na
kaa
c Na+ < Mg2+ < F– < Na < Mg
d Mg2+ < Na+ < F– < Mg < Na
e Mg2+ < Mg < Na+ < Na < F–
49.
What is the [OH–] of a solution with a pH of 9.0?
a 1 × 10–5 M
c 1 × 10–4 M
d 1 × 10–7 M
e
50.
none of the above
re.c
b 1 × 10–9 M
Which of the following statements regarding the solubility of Mg(OH)2 is correct?
om
a
pH has no effect on the solubility of Mg(OH)2.
b
Mg(OH)2 is less soluble at pH 4 than pH 7.
c
Mg(OH)2 is less soluble in 0.1 M MgCl2 solution than in water.
d
all of the above
e
none of the above
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51.
When cells are placed into an isotonic solution (i.e. the solution and cell fluid have
the same osmotic pressure):
a
no exchange of water across the cell membrane occurs.
b
water enters the cell faster than it leaves the cell.
d
e
52.
water enters the cell at the same rate that it leaves the cell.
ready exchange of solutes, but not water, occurs across the cell membrane.
What is the relationship between Kc and Kp for the following reaction?
A(g) + B(g)
2C(g)
Kp = Kc(RT)2
w.i
a
b
Kc = Kp(RT)2
c
Kc = Kp
d
Kc = √Kp
e
Kc = KpRT
bio
53.
water leaves the cell faster than it enters the cell.
ww
c
Histidine is an amino acid. The fully protonated form has the pKa values indicated
below.
pKa = 5.97
H
N
NH
kaa
CH2
pKa = 1.82
HOOC
C
pKa = 9.17
NH3
H
Which one of the following is the predominant structure at pH 7.6?
H
N
NH
NH
CH2
HOOC
C
H
N
re.c
N
NH
CH2
NH3
O2C
A
C
H
B
H
CH2
NH3
O2C
H
C
NH3
N
N
CH2
CH2
C
H
D
NH3
HOOC
C
H
E
om
NH
NH
HOOC
C
NH2
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54. Arrange the following 1 M solutions in order of increasing pH.
a
HCl
KOH
CaCl2 CH3COOH
KOH < CaCl2 < Na3PO4 < CH3COOH < HCl
Na3PO4
b HCl < CaCl2 < CH3COOH < KOH < Na3PO4
d
e
ww
c CH3COOH < HCl < CaCl2 < KOH < Na3PO4
HCl < CH3COOH < Na3PO4 < CaCl2 < KOH
HCl < CH3COOH < CaCl2 < Na3PO4 < KOH
In answering questions 15-19, consider the following titration curve.
12
w.i
10
8
pH
6
2
bio
4
10
20
30
40
50
Amount of solution added (mL)
kaa
55.
Which one of the following combinations does the titration curve represent?
a
b
c
Addition of a strong base to a weak acid
Addition of a weak base to a strong acid
Addition of a strong acid to a weak base
d Addition of a weak acid to a strong base
re.c
e Addition of a strong acid to a strong base
56.
What is the value of the pKa that can be obtained from this titration curve?
a 11.3
57.
c 9.3
d 5.3
e 1.8
What is the pH of the solution at the point of maximum buffering?
b 10.0
c 9.3
d 5.3
e 1.8
om
a 11.3
58.
b 10.0
What is the pH of the solution at the equivalence point?
a 11.3
b 10.0
c 9.3
d 5.3
e 1.8
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59.
Which one of the following indicators would be most suitable for this titration?
a
any acid/base indicator is suitable
b
phenolphthalein (pKa = 9.6)
c
cresol red (pKa = 8.3)
e
60.
ww
d
methyl yellow (pKa = 3.1)
How many stereoisomers are possible for the complex [NiCl2(en)2]?
en = ethylenediamine = NH2CH2CH2NH2
a
c 3
d 4
e6
1
w.i
b2
How many stereoisomers are possible for the complex [Ni(en)3]2+?
en = ethylenediamine = NH2CH2CH2NH2
a1
b2
c 3
e6
62.
What is the solubility constant expression for Zn3(PO4)2?
A
Ksp = [Zn2+][PO43–]
B
Ksp = [Zn2+][2PO43–]
C
Ksp = [Zn2+]3[PO43–]2
D
Ksp = [3Zn2+]3[2PO43–]2
E
Ksp = [Zn3+]2[PO42–]3
re.c
63.
kaa
d 4
bio
61.
methyl red (pKa = 5.1)
What is the solubility product constant expression for Ag3PO4?
Ksp = [Ag+][PO43–]
B
Ksp = [Ag+][PO43–]3
C
Ksp = [Ag+]3[PO43–]
D
Ksp = [3Ag+]3[PO43–]
E
Ksp = 3[Ag+][PO43–]
om
A
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64. How would the concentration of Pb2+(aq) ions in equilibrium with PbI2(s) be
affected if the concentration of I–(aq) ions were doubled?
a
no change
b
increased by a factor of 2
ww
c decreased by a factor of 2
d decreased by a factor of 4
e decreased by a factor of 16
65.
Which one of the following is a coordination isomer of the complex salt,
trans-[CrCl2(OH2)4]Br?
B
trans-[CrBrCl(OH2)4]Cl
C
trans-[Cr Br2 (OH2)4]Cl
D
trans-[CrBr2(OH2)4]Cl
E
trans-[Cr(OH2)4Cl2]Br
bio
66.
cis-[CrCl2(OH2)4]Br
w.i
A
Which one of the following equations describes the enthalpy of combustion
of glucose.
C6H12O6(s) → 6C(s) + 6H2O(l)
b
C6H12O6(s) → 2C2H5OH(l) + 2CO2(g)
c
C6H12O6(s) → 6C(s) + 3O2(g) + 6H2(g)
d
C6H12O6(s) + 3O2(g) → 6CO2(g) + 6H2(g)
kaa
a
e C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(g)
Questions 67 - 70 refer to the voltaic cell shown below.
Voltmeter
1.0 M Ni2+
re.c
Ni
Salt Bridge
Cu
1.0 M Cu2+
om
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67.
What is the overall reaction occurring in this cell?
a
There will be no spontaneous reaction.
b
Ni2+(aq) + Cu(s) → Ni(s) + Cu2+(aq)
c
Cu2+(aq) + Ni(s) → Cu(s) + Ni2+(aq)
ww
d
Cu2+(aq) + Ni2+(aq) + 4e– → Cu(s) + Ni(s)
e Cu(s) + Ni(s) → Cu2+(aq) + Ni2+(aq) + 4e–
68.
What would be the value of Ecell at equilibrium?
a
0.34 V
c 0.24 V
d 0.10 V
e 0.00 V
69.
What is the reading on the voltmeter when the half cells are first connected?
0.58 V
b
0.34 V
c
0.24 V
d
0.10 V
e
0.00 V
kaa
a
bio
70.
w.i
b
0.58 V
Which electrode is the anode and to which electrode do the electrons flow?
a
The Ni electrode is the anode; electrons flow to the cathode.
b The Cu electrode is the anode; electrons flow to the cathode.
c The Ni electrode is the anode; electrons flow to the anode.
d
re.c
71.
The Cu electrode is the anode; electrons flow to the anode
Rank the following series of atoms in order of INCREASING electronegativity.
N O F P As
a N < O < F < P < As
b F < O < N < P < As
c As < P < N < O < F
e F < N < O < As < P
om
d As < P < N < F < O
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72.
A reaction has an activation energy of 40 kJ mol–1 and an overall energy change
of –100 kJ mol–1. In each of the potential energy diagrams shown below, the
horizontal axis is the reaction coordinate and the vertical axis is potential energy
in kJ mol–1. Which potential energy diagram best describes this reaction?
ww
40
a
100
reactants
40
b
products
40
100
reactants
products
c
100
reactants
products
40
d
100
products
reactants
products
1
0
b
0
1
c
0
−1
d
0
−1
e
0
1
n
α
α
β
β
137
56
Ba + ?
kaa
a
Cs →
bio
What isotope is produced by the α-decay of
A
222
85
At
B
218
84
Po
C
218
88
Rn
D
222
87
Fr
E
221
85
At
222
86
Rn ?
re.c
75.
40
What is the missing particle for the following nuclear decay process?
137
55
74.
100
w.i
reactants
73.
e
Which one of the following statements about reaction rate is false?
Reaction rate is the speed at which the reaction proceeds.
b
Reaction rate is governed by the energy barrier between reactants and
products.
c
Enzymes can accelerate the rate of a reaction.
d Reaction rates are not sensitive to temperature.
om
a
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76. What isotope is produced by the α-decay of
None -
B
99
42
Mo
C
95
41
Nb
99
44
Ru
D
E
77.
103
45
Rh
What is the oxidation state of Rh in the complex K3[Rh(CN)6]?
A
+I
B
+III
C
+VI
D
0
E
–III
What is the oxidation state of Tc in K2[TcO(ox)2]? ox is the oxalate anion, C2O42–.
+II
B
+III
C
+IV
D
+V
E
+VI
kaa
A
A solid pharmaceutical dispersed in a carrier gas is an example of which one of the
following?
a gel
b
a foam
c
an emulsion
re.c
a
d an aerosol
80.
bio
79.
Tc undergoes β– decay
99
43
w.i
78.
Tc ?
43
ww
A
99
How many isomers are possible for the square planar complex [PtI2(NH3)2]?
1
2
3
4
5
om
a
b
c
d
e
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ww
81. Which of the following statements is false?
a. Condensed states have much higher densities than gases.
b. Molecules are very far apart in gases and closer together in liquids and solids.
c. Gases completely fill any container they occupy and are easily compressed.
d. Vapor refers to a gas formed by evaporation of a liquid or sublimation of a solid.
e. Solid water (ice), unlike most substances, is denser than its liquid form (water).
w.i
82. Which physical state/ property is incorrectly matched?
a. liquids and solids - rigid shape b. gases - easily compressed
c. gases and liquids - flow
d. solids - higher density than gases
e. liquids - incompressible
bio
83. An open-tube manometer is used to measure the pressure in flask. The atmospheric pressure is 756 torr
and the Hg column is 10.5 cm higher on the open end. What is the pressure in the flask?
a. 766.5 mmHg
b. 861 cm Hg
c. 861 torr
d. 649 torr
e. 745.5 mm Hg
kaa
84. The volume of a sample of a gas is 405 mL at 10.0 atm and 467 K. What volume will it occupy at 4.29
atm and the same temperature?
a. 17.4 L
b. 189 mL
c. 174 mL
d. 1047 mL
e. 944 mL
re.c
85. Absolute zero is the temperature at which
a. a graph of V versus 1/P intersects the 1/P-axis.
b. gaseous helium liquefies.
c. the straight line graph of V versus T intersects the T-axis.
d. a graph of P versus 1/V intersects the 1/V-axis.
e. none of the above
om
86. A sample of nitrogen occupies 5.50 liters under a pressure of 900. torr at 25.0 C. At what temperature will it
occupy 10.0 liters at the same pressure?
a. 32 C
b. -109 C
c. 154 C
d. 269 C
e. 370 C
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ww
87. Snoopy is inflated for the Macy's Thanksgiving parade with 50,000 L of He at 25 C and 1.2 atm. What is the
percent decrease in Snoopy's volume if the temperature drops to 4 C before the parade? Assume constant
pressure.
a. 7.58 %
b. 10.1 %
c. 7.1 %
d. 21 %
e. 1.2 %
w.i
88. A gas sample occupies 1.00 L at 120. C and 1.00 atm. What volume will it occupy at STP?
a. 1.14 L
b. 1.44 L
c. 0.846 L
d. 0.782 L
e. 0.695 L
bio
89. A sample of propane, C3H8, occupies 1.73 mL when the pressure is 320 torr at 30 C. What is the volume
at STP?
a. 656 mL
b. 499 mL
c. 5.09 L
d. 3.70 L
e. 808 mL
kaa
90. What volume will 12.40 grams of CO2 occupy at STP, if it behaves ideally?
a. 6.31 L
b. 8.46 L
c. 4.42 L
d. 11.7 L
e. 9.68 L
91. Ten (10.0) moles of a gas are contained in a 10.0 L container at 273 K. Calculate the pressure of the gas.
a. 2.24 atm
b. 4.48 atm
c. 11.2 atm
d. 15.7 atm
e. 22.4 atm
re.c
92. A gaseous compound is 30.4% nitrogen and 69.6% oxygen by mass. A 5.25-gram sample of the gas occupies
a volume of 1.00 liter and exerts a pressure of 1.26 atmospheres at - 4.0 C. What is its molecular formula?
a. NO
b. NO2
c. N3O6
d. N2O4
e. N2O5
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93. A 10.0-L flask contains 0.400 mole of H2, 0.300 mole of He and 0.500 mole of Ne at 35.0 C. What is the total
pressure in the flask?
a. 2.53 atm
b. 4.05 atm
c. 3.03 atm
d. 1.01 atm
e. 0.345 atm
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94. A mixture of gas consists of 5.0 g CH4, 5.0 g C2H2, and 5.0 g C2H4. What are the mole fractions of each?
XCH4
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a.
b.
c.
d.
e.
XC2H2
0.321
0.333
0.217
0.567
0.457
0.192
0.333
0.375
0.137
0.281
XC2H4
0.177
0.333
0.408
0.326
0.262
w.i
95. A 5.00 L container contains CH4, H2, and Xe at 35 C with a total pressure of 1.81 atm. If there are equal
moles of each gas, what is the partial pressure of H2?
a. 0.603 atm
b. 0.034 atm c. 1.81 atm
d. 3.05 atm
e. 0.362 atm
96. A 10.0-L flask contains 0.400 mole of H2, 0.300 mole of He and 0.500 mole of Ne at 35.0 C. What is the
partial pressure of the Ne?
a. 1.26 atm
b. 3.03 atm
c. 1.05 atm
d. 1.69 atm
e. 0.144 atm
bio
97. What is the pressure exerted by a mixture of 1.0 g H2 and 5.0 g He when confined to a volume of 5.0 liters at
20. C?
a. 12.6 atm
b. 8.4 atm
c. 3.61 atm
d. 10.4 atm
e. 6.5 atm
98. What is the mole fraction of O2 in a mixture of 2.00 g He, 12.0 g O2, and 17.0 g N2?
a. 0.608 b. 0.253
c. 0.410
d. 0.200
e. 0.267
99. A mixture of 16.0 g of He, 21.0 g of N2, and 16.0 g of O2 at 25 C is in a 75.0-L container. What are the mole
fractions of each of these three gases?
XN
0.158
0.167
0.150
0.143
0.762
kaa
XHe
0.842
a.
b. 0.889
c. 0.800
d. 0.762
e. 0.952
XO
0.105
0.111
0.100
0.0952
0.143
100. Which one of the statements below about the following reaction is false?
CO2(g) + 2H2O(g)
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CH4(g) + 2O2(g)
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a. Every methane molecule that reacts produces two water molecules.
b. If 16.0 g of methane react with 32.0 g of oxygen, the maximum amount of CO2 produced
will be 22.0 g.
c. If 11.2 liters of methane react with an excess of oxygen, the volume of CO2 produced at
STP is (44/16)(11.2) liters.
d. If 16.0 g of methane react with 64.0 g of oxygen, the combined masses of the products
will be 80.0 g.
e. If 22.4 liters of methane at STP react with 64.0 g of oxygen, 22.4 L (STP) of CO2 can be
produced.
AIIMS,CBSE,AIPMT, AFMC,Bio.Tech & PMT, Contact :- 9438559863, Mail at :- [email protected],www.ibiokaare.com,compiled by AKB
2
d
7
c
12
b
17
c
22
c
27
a
32
d
37
c
3
d
8
c
13
a
18
d
23
c
28
c
33
c
38
c
4
b
9
b
14
c
19
b
24
d
29
a
34
a
39
b
5
c
10
a
15
c
20
d
25
c
30
b
35
b
40
a
bio
w.i
ww
1
d
6
d
11
b
16
a
21
d
26
a
31
c
36
b
42
C
52
43
C
53
D
C
C
61
B
62
C
63
C
64
D
73
74
D
B
72
71
C
E 82.
93.
45
D
55
46
A
56
47
E
57
48
D
58
49
A
59
50
C
60
E
C
C
C
D
D
C
65
B
66
E
67
C
68
E
69
A
70
A
75
76
77
78
79
80
D
A
B
C
D
B
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81.
A
44
B
54
kaa
41
C
51
A 83. C 84. E 85. C 86. D 87. C 88. E 89. A 90.
C 94.
E 95.
A 96. A 97. B 98.
A 91. E 92. D
B 99. D 100. C
om
AIIMS,CBSE,AIPMT, AFMC,Bio.Tech & PMT, Contact :- 9438559863, Mail at :- [email protected],www.ibiokaare.com,compiled by AKB