Transcript Slide 1

Revision to 110 Chapter 1-4
Dr. Ali Bumajdad
1-
Which one is not a pure substance?
A) Chlorine
B) Sulfur
C) Water
D) Oxygen
E) Air
Not Pure Substance= Mixture
2- The normal temperature of a human body is 37.00C.
equivalent to _____ 0F.
A) 19.0
B) 94.8
C) 310
D) 98.6
E) 97.8
3- Which of the following is a metalloid?
A) Ge
B) Xe
C) F
D) H
E) Li
This value is
TC = (TF – 32)  5
9
TF = (TC  9 ) + 32
5
Slide 1
4- Of the three types of radioactivity characterized by Rutherford, which is
(are) not electrically charged?
A) Alfa rays
B) Alfa rays, beta rays and gamma rays
C) Gamma rays
D) Alfa rays and beta rays
E) Alfa rays and gamma rays
Alpha,  = particles with +2 charge
Beta, 
= high speed eGamma,  = high energy light (no charge)
Dr. Ali Bumajdad
5- A molecule of water contains hydrogen and oxygen in a 1:8 ratio by
mass. This is a statement of:
A) The law of multiple proportions.
B) The law of constant composition.
C) The law of conservation of mass.
D) The law of conservation of energy.
E) None of these.
Law of constant composition =1
Law of Multiple Proportion =2
6- Which of the following is a pair of isotopes of the same element?
A)
116
92
2
119
92
B)
116
92
2
122
89
C)
96
48
D)
120
89
M,
E)
116
92
2
M ,
M ,
M,
M
2
M
Isotopes have same number of protons
116
92
M
120
92
M ,
M
122
89
2
M
7- What is the empirical formula of a compound that contains 49.4% K,
20.3% S and 30.3% O by mass?
n=
m
M.m.
A) KSO2
B) KSO3
C) K2SO4
D) K2SO3
E) KSO4
Empirical Formula = I need no. of moles
1)
Find the moles elements
(for %mass assume you have 100 g)
Divide by the smallest mole value
2)
8- In an experiment, 200 g of Al and 700 g of Fe 3O4 are mixed and allowed
to react according to the following equation:
3Fe3O4 + 8Al

4Al 2O3
+ 9Fe
How many grams of Fe can be formed?
A) 506
B) 581
C) 412
D) 519
E) 466
2 masses = may be limiting reactant
Fe3O4 M.w. = 231.55 g mol
Al M.w.
= 27 g/mol
Fe M.w.
= 55.85 g/mol
Slide 1
Dr. Ali Bumajdad
9-
How many mL of water should be added to 25.0 mL of 6.0 M HCl to
make 2.50 M HCl?
A)
B)
C)
D)
E)
Dilution = one substance + water
60.0 mL
35.0 mL
10.4 mL
300 mL
275 mL
Mi Vi =Mf Vf
10- An example of oxidation is:
A)
B)
C)
D)
E)
11-
Ice melting in a soft drink.
Table salt dissolving in water.
Oxidation: Loss
Rusting of iron.
The reaction of NaCl with Pb(NO3)2.
All of the above are oxidation-reduction reactions.
A temperature of 400. K is the same as _____
A) 260
B) 286
C) 88
D) 103
E) 127
TC = TK – 273.15
(0.002843)(12.80184)
= ______
0.00032
12A)
B)
C)
D)
E)
113.73635
113.736
113.74
113.7
1.1 x 102
0
of electrons
F:
TF = (TC  9 ) + 32
5
113.7634725
Slide 1
13- Which pair of substances could be used to illustrate the law of multiple
proportions?
a.
b.
c.
d.
e.
SO2, H2SO4
SO, SO2
H2O, O2
CH4, C6H12O6
NaCl, KCl
Law of Multiple Proportion = 2 compound
from the same elements
Dr. Ali Bumajdad
14-______ -rays consist of fast-moving electrons?
a.
b.
c.
d.
e.
Alpha, 
alpha
beta
Beta, 
gamma
Gamma,
X
none of these
= particles with +2 charge
= high speed e = high energy light (no charge)
15- Naturally occurring bromine is 50.69% 79Br which has an atomic mass
of 79.618 amu and 49.31% 81Br which has an atomic mass of 80.196 amu.
The average atomic mass of bromine is:
a.
b.
c.
d.
e.
79.903
78.910
81.000
79.920
79.548
16 - Calcium is a
A)
B)
C)
D)
E)
amu
amu
amu
amu
amu
____
Slide 1
and silver is a ______ :
nonmetal, metal
metal, metal
metalloid, metal
metal, metalloid
nonmetal, metalloid
Slide 1
17- There are _____ electrons, _____ protons, and _____ neutrons in the
ion
77
35
3
X
?
a.
b.
c.
d.
e.
38,
77,
32,
77,
35,
35,
32,
80,
77,
35,
42
77
35
35
42
Mass Number
A
Atomic Number
Z
X
Element Symbol
Dr. Ali Bumajdad
18- The number of carbon atoms in 0.500 g of carbon dioxide, CO 2 is:
a.
b.
c.
d.
e.
6.84
1.14
6.86
6.84
3.01
x
x
x
x
x
1022
1021
1023
1021
1023
No. of Objects = I need n and NA
n=
m
M.m.
n=
N
NA
19- Maleic acid contains 41.4% carbon, 3.47% hydrogen and 55.1%
oxygen by weight. A 0.050 mole sample of this compound weighs 5.80 g.
What is the molecular formula of maleic acid?
a.
b.
c.
d.
e.
CHO
C2H2O2
C 3H 3O
C4H4O4
C6H6O6
C 3.45 H 3.44 O 3.44
Molecular Formula = I need no. of moles and
Molar mass
1)
2)
Find the moles elements
(for %mass assume you have 100 g)
Divide by the smallest mole value
3)
M.F. = E.F. ×
M.m. M.F.
M.m. E.F.
20- The spectator ion(s) in the reaction between aqueous solutions of a
weak acid, hydrofluoric acid(HF) and sodium hydroxide (NaOH) are:
a.
b.
c.
d.
e.
HF, Na+

H+/F
Na+

F
all are spectator ions
Spectator ions disappear in the
net ionic equation
Dr. Ali Bumajdad
21- What is the oxidation number of P in H 3PO2 ?
a.
b.
c.
d.
e.
-3
0
+1
+3
+7
Slide 1
22- What is the molarity of an aqueous solution of potassium hydroxide,
KOH if 21.34 mL is exactly neutralized by 20.71 mL of 0.058 M H 2SO4?
a.
b.
c.
d.
e.
0.226 M
1.130 M
2.14 M
0.113 M
0.0565 M
nH M aicd V acid = nOHM base V base
23- The reaction of 2.50 g of aluminum with 2.50 g of oxygen produced
3.50 g of aluminum oxide. The yield of aluminum oxide is ___ %.
4Al(s)
a.
b.
c.
d.
e.
+
74.2
37.2
47.2
66.5
26.7
3O2(g)

2Al 2O3(s)
2 masses = may be limiting reactant
O2 M.w. = 32.0 g mol
Al M.w.
= 27.0 g/mol
Al2O3 M.w. = 55.85 g/mol
Slide 1
24- Which of the following is/are decomposition reaction(s)?
1234-
CH4(g) +
CaO(s) +
Mg(s) +
PbCO3(s)
a.
b.
c.
d.
e.
O2(g)  CO2(g) + H2O(ℓ)
CO2(g)  CaCO3(s)
O2(g)  MgO(s)
 PbO(s) + CO2(g)
1, 2 and 3
2 and 3
1, 2, 3 and 4
4 only
2, 3, and 4
Slide 1
Dr. Ali Bumajdad
25- Which pair of symbols below represents isotopes?
A) 16O, 16N
B) H , He
C) He , He+
D) 16O, 17O
E) 13C, 14N
Isotopes have same number of protons
but different number of neutrons
26- Use the law of definite proportion to find the mass of O atoms in H 2O2
(if the mass of H atoms is 8 g):
A)
B)
C)
D)
E)
27-
6
8
128
64
32
Law of constant composition =1
2.016
=
32
C2H4
+
3O2
8
X
2CO2 + 2H2O

How many grams of CO2 will be formed when a mixture
containing 2.70 g C2H4 and 5.80 g O2 is burned?
A)
B)
C)
D)
E)
3.00
1.68
9.15
5.32
7.23
g
g
g
g
g
2 masses = may be limiting reactant
C2H4 M.w. = 26.036 g/mol
O2 M.w. = 32.0 g/mol
CO2 M.w. = 44.0 g/mol
Slide 1
28- After balancing the equation below, the coefficient of O 2 will be:
C7H16
A)
B)
C)
D)
E)
+
O2

CO2 +
H 2O
9
7
8
4
11
Start by balancing those elements that appear in only
one reactant and one product.
Dr. Ali Bumajdad
29- The mass in gram of 1.0 x 103 atoms of sulfur (S) is:
a.
b.
c.
d.
e.
5.3
5.0
7.3
5.3
4.0
x
g
x
x
x
1020 g
1023 g
1023 g
1020 g
m of 1 atom in g
=
m of 1 mol in g
NA
30- The number of moles of hydrogen atoms (H) in 9.01 x 10 20 molecules
of methane (CH4) is:
a.
b.
c.
d.
e.
1.50
2.01
2.99
3.32
5.98
x 103 mol
mol
x 103 mol
x 1023 mol
x 103 mol
N
NA
n=
Slide 1
31- A compound with an empirical formula of NPCl 2 and its molar mass is
347.64 g/mol. What is the molecular formula?
a.
b.
c.
d.
e.
M.m. M.F.
M.F. = E.F. ×
M.m. E.F.
N2P2Cl4
N3P3Cl6
NPCl6
N3P3Cl2
NPCl2
NPCl2 M.w. = 115.87 g/mol
32- Which of the following aqueous solution contains the greatest
number of ions?
a.
b.
c.
d.
e.
0.10
0.10
0.10
0.10
0.10
M
M
M
M
M
NaCl
CaCl 2
FeCl 3
Glucose (C6H12O6)
Al 2(SO4)3
2 moles
3 moles
4 moles
No
5 moles
33- What is the molarity of an aqueous solution contains 22.5 g
sucrose (C12H22O11) in 35.5 ml of solution?
A)
B)
C)
D)
E)
0.0657 M
1.85 x 103 M
1.85 M
3.52 M
0.104 M
M=
n
VLsolution
C12H22O11 M.w. = 342 g/mol
Dr. Ali Bumajdad
34- What is/are spectator ion(s) for the reaction between aqueous
solution of CoBr2 and AgNO3?
a.
b.
c.
d.
e.
NO3
Br
Co2+ and Ag+
NO3 and Br
Co2+ and NO3
Spectator ions disappear in the
net ionic equation
Slide 1
35- If matter is uniform throughout and cannot be separated into
other substances by physical means, it is _______
A)
B)
C)
D)
E)
a compound only
either an element or a compound
a homogeneous mixture
a heterogeneous mixture
an element only
Slide 1
36- Nitrogen may form two gases NO and NO2 with oxygen. The
amount of oxygen combining with one nitrogen in NO 2 is double that
in NO. This can be a statement from:
Law of Multiple Proportion = 2 compound
from the same elements
A)
B)
C)
D)
E)
The law of conservation of mass
The law of multiple proportion
The law of constant composition
The law of conservation of energy
None of these
37- A temperature of 400 K is the same as _______ 0F.
A)
B)
C)
D)
E)
261
286
88
103
127
Dr. Ali Bumajdad
38- In the answer to the following computation:
(31.2-22.0) (1.78x105)/ (1.39)
The number of significant figure(s) is:
A) 1
A) 2
B) 3
C) 4
D) 5
Slide 1
39- Accuracy refers to ______ :
A) How close a measured number is to zero
A) How close a measured number is to the calculated value
B) How close a measured number is to other measured
numbers
C) How close a measured number is to the true value
D) How close a measured number is to infinity
40- The number of protons, electrons and neutrons in the ion
are:
A)
B)
C)
D)
E)
28, 31 and 73
34, 31 and 70
31, 31 and 39
31, 34 and 39
31, 28 and 39
70
31
Slide 1
X 3
Slide 1
41- Which one of the following should be the most similar to sulfur (S)
in physical and chemical properties:
A) Se
B) P
C) As
D) Cl
E) F
Slide 1
42- The charge on an electron was determined in the:
A) Cathode ray tube by J.J. Thompson
B) Rutherford gold foil experiment
C) Millikan oil drop experiment
D) Dalton atomic theory
E) Atomic theory of matter
Slide 1
Dr. Ali Bumajdad
43-
________ and _________ are isotopes of the same element.
A)
116
92
X 2 ,
119
92
X
B)
116
92
X 2 ,
122
89
X 2
C)
96
45
D)
233
99
E)
22
11
X ,
X 2 ,
X ,
116
92
116
92
79
38
X
X 4
X 2
44- Assume that element X has three naturally occurring isotopes. The
isotopic masses (amu) and abundances are: 52.62 (19.61%), 56.29
(53.91%) and 58.31 (26.48%). The average atomic weight (amu) of
element X is:
A)
B)
C)
D)
E)
56.33
55.74
56.11
57.23
56.29
Slide 1
45- The number of g of hydrogen atoms in 23 g of CH4O are:
A)
B)
C)
D)
E)
2.9
1.5
2.8
0.36
184
Slide 1
46- A nitrogen oxide contains 63.65% nitrogen by mass.
formula could be:
a.
b.
c.
d.
e.
The molecular
Molecular Formula = I need no. of moles and
NO
Molar mass
NO2
N2O
1)
Find the moles elements
N2O4
(for %mass assume you have
Both NO2 and N2O4
Dr. Ali Bumajdad
2)
100 g)
Divide by the smallest mole value
3)
M.F. = E.F. ×
M.m. M.F.
M.m. E.F.
CH2F2 M.w. = 52.0 g /mol
48- A sample of 19 g of CH 2F2 contains _____ atoms of F.
a.
b.
c.
d.
e.
2.2
6.0
3.3
4.4
4.4
x
x
x
x
x
1024
1023
1024
1023
1024
No. of Objects = I need n and NA
n=
m
M.m.
n=
N
NA
49- The combustion of 3.42 g of a compound known to contain only
nitrogen and hydrogen gave 9.82 g of NO2 and 3.85 g of water. The
empirical formula of this compound is:
a.
b.
c.
d.
e.
1)
NH
NH2
N2H
NH3
N2H6
2)
Find the moles elements
(for %mass assume you have 100 g)
Divide by the smallest mole value
NO2 M.w. = 52.0 g /mol
H2O M.w. = 18.0 g/mol
50- Calcium carbide (CaC2) reacts with water, producing acetylene (C 2H2):
CaC2 + 2H2O  Ca(OH)2 + C2H2
Production of 13 g of C2H2 requires ______ g of H2O.
a.
b.
c.
d.
e.
4.5
9.0
18
4.8 x 102
4.8 x 102
Slide 1
51- The reaction of 2.5 g of aluminium with 2.5 g of oxygen produced 3.5
g of aluminium oxide.
4Al (s) + 3O2(g)

2Al2O3(s)
The % yield of aluminium oxide is:
a.
b.
c.
d.
e.
47
37
74
35
26
Dr. Ali Bumajdad
52- Combining the aqueous solution of BaI2 and K2SO4 yields a participate
of BaSO4.
BaI2 (aq) +
K2SO4 (aq)

Ba SO4 (s)
+
KI(aq)
Which ion(s) is/are spectator(s) in the reaction?
A)
B)
C)
D)
E)
Ba2+
K+
Ba2+ and K+
K+ and ISO4 2- and I-
53- How many moles of chloride ions are present in 0.500L of a 0.400 M
solution of AlCl 3?
A) 0.400
B) 0.600
C) 0.200
D) 0.300
E) 0.150
M=
n
VLsolution
54- A 36.3 mL of 0.0529 M H2SO4(aq) is to be titrated against 0.0411 M
NaOH (aq). The volume (mL) of the base required to reach the equivalence
point is:
A) 93.4
B)
C)
D)
E)
46.7
23.4
211
9.34
nH M aicd V acid = nOHM base V base
________
Dr. Ali Bumajdad
Kuc02.kuniv.edu.kw/~bumajdad/