FINAL TEST QUESTIONS
SUBJECT : CHEMISTRY
CLASS : XI
1.
Multiple
choice
|
Num.
|
Topic
|
Question
|
Answer key
|
Level of Difficulty
|
|
1.
|
Fundamental concepts of chemistry
|
There are three phases or states of matter,
they are..
a.
Pink , black and yellow
b.
Stone, Salt, food
c.
Solids, liquids, gases
d.
Solution, Solutes, Solvents
e.
Gases, black, liquids
|
C
|
Easy
|
|
2
|
Fundamental
concepts of chemistry
|
The Simplest substances and are composed of
a single type of atom are called..
a.
The Chemical elements
b.
The Compound
c.
Molecules
d.
Metals
e.
Non-metals
|
A
|
Easy
|
|
3
|
Fundamental concepts of chemistry
|
The amount
of a substance is called by..
a.
Molar mass
b.
Mass of substance
c.
State of substance
d.
Mole
e.
Avogadro’s constant
|
D
|
Easy
|
|
4.
|
Atomic Structure
|
Atoms are composed of three subatomic
particles, they are…
a.
Protons, electrons, molecules
b.
Electrons. Neutrons, compounds
c.
Protons, neutrons,electrons
d.
Electrons, protons, elements
e.
Molecules, protons, neutron
|
C
|
Easy
|
|
5.
|
Atomic Structure
|
The sub-atomic particles which occupy the
nucleus of atom are…
a.
Protons and electrons
b.
Protons and neutrons
c.
Neutrons and electrons
d.
Alpa and beta
e.
Alpa and neutrons
|
B
|
Easy
|
|
6.
|
The mole concept and Avogadro’s constant
|
How many mol 36 gram of H2 O ( Ar H=1, O=16)..
a.
1 mol
b.
3 mol
c.
2 mol
d.
4 mol
e.
5 mol
|
C
|
Medium
|
|
7
|
Atomic structure
|
The word “atom” derived from the Greek word
“atomos” meaning…….
a.
Uncuttable
b.
Unblockable
c.
Uncloseable
d.
Uncalculate
e.
Unseen
|
|
Easy
|
|
8
|
Atomic structure
|
The atomic number of a netral atom is…
a.
The numbers of neutron
b.
The number of electron
c.
The number of proton
d.
The number of avogadro’s constant
e.
The number of molar mass
|
C
|
Easy
|
|
9
|
Atomic structure
|
An atom of aluminium has mass number 27 and
atomic number 13. Which statement is true..
a.
Proton 13, electron 13, neutron 14
b.
Proton 27, electron 14, neutron 13
c.
Proton 13, electron 27, neutron 14
d.
Proton 14,electron 13, neutron 14
e.
Proton 13, electron 14, neutron14
|
A
|
Medium
|
|
10
|
Atomic structure
|
Which element shows chemical behavior similar to Sodium…..
a.
Boron
b.
Oxygen
c.
Chlorine
d.
Pottasium
e.
Xenon
|
P
|
Medium
|
|
11
|
The empirical and molecular mass
|
The molecular formula of a compound
containing 85% by mass of carbon and 15% by mass of hydrogen. The molar mass of the compound is
28 g/mol.
a.
CH2
b.
C2H2
c.
C2H4
d.
C2H6
e.
C4H8
|
C
|
Medium
|
|
12
|
Concept of mole and avogadro’s constant
|
The molar mass of ammonia gas = Mr g/mol. What is the number molecules
of 10 mol ammonia if Avogadro’s contant is L..
a.
10
b.
10L
c.
L/10Mr
d.
10 Mr L
e.
10L/Mr
|
B
|
Medium
|
|
13
|
Percentage purity
|
Amount
of nitrogen (Ar N= 14) in
ammonium nitrate (Mr= 80) is…
a.
10 %
b.
15 %
c.
20 %
d.
35 %
e.
50 %
|
D
|
Medium
|
|
14
|
The mole concept and Avogadros’s constant
|
The mole of magnesium that can be obtained
from the reaction between 9.6 grams of magnesium and 9.8 gram sulfur. (Ar Mg = 24, S= 32)
a.
0.1 mol
b.
0.2 mol
c.
0.3 mol
d.
0.4 mol
e.
0.5 mol
|
D
|
Medium
|
|
15
|
The ionic equation
|
The Ionic equation of MgSO4 is..
a.
Mg
+ SO4
b.
Mg+ + SO4-
c.
Mg+ + SO42-
d.
Mg2+ + SO42+
e.
Mg2- + SO42+
|
D
|
Medium
|
|
16
|
Chemical equation
|
_C2H6(g) + _O2(g) à _CO2(g) +_ H2O(l)
What is the whole coefficient for the equation above when it
is balanced..
a.
2, 7, 4, 6
b.
2, 2, 6, 4
c.
3, 4 , 6, 7
d.
7, 2 , 4, 5
e.
2, 7, 5, 6
|
A
|
Medium
|
|
17
|
Chemical equation
|
When sodium (Na) reacts with sulfate(SO4) to form a formula.
The formula is…..
a.
NaSO4
b.
Na(SO4)2
c.
Na2SO4
d.
Na2(SO4)2
e.
Na2(SO4)3
|
C
|
Medium
|
|
18
|
Percentage purity
|
The Combustion of 60 gram ethane produces
water and carbondioxide. What is the percentage purity of carbon in
carbondioxide ? ( molar mass of C = 12, H= 1, O =16)
a.
27.3 %
b.
20.3 %
c.
15.3 %
d.
9.3 %
e.
4.3 %
|
A
|
Difficult
|
|
19
|
The ideal gas equation
|
What is the volume of 4 gram hydrogen gas at 270C temperature and 1 atm pressure.
a.
44,1 L
b.
45,2 L
c.
46,3 L
d.
48,2 L
e.
49,2 L
|
E
|
Difficult
|
|
20
|
Molar volume of gas
|
What is the volume of carbondioxide in STP
condition that is produced from the
combustion of 5,6 gram C2H4
a.
1,96 L
b.
10,96 L
c.
36,96 L
d.
8, 96 L
e.
3, 96 L
|
D
|
Difficult
|
|
21
|
Concept mole and Avogadro’s constant
|
What is the number particles of 22 gram CO2
( molar mass CO2 is 44).? ( Avogadro’s Constant is 6.02 x 1023
a.
9.03 x 1023
b.
12.03 x 1023
c.
15. 03 x 1023
d.
20.03 x 1023
e.
28. 03 x 1023
|
A
|
Medium
|
|
22
|
Empirical and molecular formula
|
A Compound containing 46,2 % by mass of
carbon, and 53,8% by mass of Nitrogen in STP condition. If the volume of this
gas is 5,6 Litre and its mass is 13 gram, what is the formula of the compound.?
( Ar C = 12, N = 14)
a.
CN
b.
CN2
c.
C2N
d.
C2N2
e.
C2N4
|
D
|
Difficult
|
|
23
|
Solutions
|
Sodium chloride solution is the mixture of
water and sodium chloride solid. Water as…
a.
Solutes
b.
Solvent
c.
Index
d.
Density
e.
Solution
|
B
|
Easy
|
|
24
|
Solutions
|
What is the concentration of 0.98 gram H2SO4 ( molar
mass =98) in 500 ml water.
a.
0.08 mol/L
b.
0.06 mol/L
c.
0.04 mol/L
d.
0.02 mol/L
e.
0.012 mol/L
|
D
|
Medium
|
|
25
|
Atomic structure
|
The number of proton, electron, and neutron
in calcium ion (4020Ca2+) are..
a.
20, 30, 40
b.
20, 20, 18
c.
20, 18, 30
d.
20, 30, 18
e.
20, 20, 30
|
B
|
Medium
|
|
26
|
The Periodic Table
|
A horizontal row of elements in the periodic
table is called..
a.
Group
b.
Metal
c.
Period
d.
Halogens
e.
Noble gases
|
C
|
Easy
|
|
27
|
The periodic table
|
The elements ingroup 7 known as..
a.
Metals
b.
Non-metals
c.
Alkali-metals
d.
Halogens
e.
Noble gas
|
D
|
Medium
|
|
28
|
Physical properties of elements
|
The minimum energy required to remove one
mole of electron from one mole of gases atoms is called…
a.
The first ionization energy
b.
The electronegativity
c.
The melting point
d.
The density
e.
The alkali metals
|
A
|
Easy
|
|
29
|
Physical properties of element
|
Which element has the highest of melting point among the elements below…
a.
Caesium
b.
Rubidium
c.
Pottasium
d.
Sodium
e.
Lithium
|
E
|
Medium
|
|
30
|
The chemistry properties of elements
|
What gas is produced when sodium placed in
water…
a.
Chlorine
b.
Oxygen
c.
Hydrogen
d.
Iodine
e.
Nitrogen
|
C
|
Medium
|
|
31
|
Ionic
bonding
|
Which one of the following compounds is classified to ionic compound..
a.
HCl
b.
NaCl
c.
CO2
d.
N2
e.
CH4
|
B
|
Difficult
|
|
32
|
Ionic bonding
|
The ionic compound formed from the reactions
between 19K and 16S is..
a.
KS
b.
K2S
c.
K2S2
d.
KS2
e.
K2S3
|
B
|
Difficult
|
|
33
|
Atomic Structure
|
The scientist who discover electron is..
a.
Dalton
b.
Niels Bohr
c.
Rutherford
d.
Thomson
e.
Millikan
|
D
|
Medium
|
|
34
|
Atomic structure
|
How much is the amount of proton, elekctron,
and neutron in 1123Na+….
a.
Proton 11, electron 10 , neutron 12
b.
Proton 23, electron 12, neutron 10
c.
Proton 11, electron 12, neutron 10
d.
Proton 12, electron 11, neutron 12
e.
Proton 11, electron 23, neutron 12
|
A
|
Difficult
|
|
35
|
The periodic table
|
Element which doesnot belong to earth
alkaline group, is..
a.
Mg
b.
K
c.
Ba
d.
Sr
e.
Ca
|
B
|
Medium
|
|
36
|
The periodic table
|
Elements within metalloid group are..
a.
Sodium, magnesium, and aluminium
b.
Boron, silicon, and tellurium
c.
Barium, arsenic, and helium
d.
Argon, chlorine, and sodium
e.
Antimony, silicon, neon
|
A
|
Difficult
|
|
37
|
Covalent bonding
|
The groups of compounds below which are
having a covalent bond are..
a.
KCl, HBr, Cl2
b.
I2 , HBr, KCl
c.
CO2, CH4 ,NaCl
d.
NaH, KBr, LiCl
e.
NH3, H2O , HCl
|
E
|
medium
|
|
38
|
Calculation
of Enthalpy changes
|
The reaction of CO2 gas formation
occurs in two steps, those are ;
C(s) +
 O2(g)
à CO(g) ∆H = -110 kJ
CO(g) +
O2(g)
à CO2(g) ∆H =
-284 kJ
What is the change in enthalpy for reaction
of CO2 gas formation.
a.
-694 kJ
b.
-594 kJ
c.
-394 kJ
d.
-294 kJ
e.
-194 kJ
|
C
|
Difficult
|
|
39
|
Calculation of Enthalpy changes
|
How much energy is required to increase the
temperature of 40 gram of water (specific heat capacity 4.18 J/g 0C)
from 100C to 300C.?
a.
3344 J
b.
3444 J
c.
3334 J
d.
3244 J
e.
3144 J
|
A
|
Medium
|
|
40
|
Calculation of enthalpy changes
|
Given that:
∆Hf C2H5OH
= -266 kJ
∆Hf CO2 = -394 kJ
∆Hf h2O = -286 kJ
Based on the data of the change in standard
enthalpy of formation for the substances above. What is the change in enthalpy for the following reaction.
C2H5OH + 3O2 à 2CO2 + 3H2O
a.
-1341 kJ
b.
-1340 kJ
c.
-1360 kJ
d.
-1370 kJ
e.
-1380 kJ
|
E
|
Difficult
|
|
|
|
|
|
|
2.
Fill
in the blanks
|
Num.
|
Topic
|
Question
|
Answer
Key
|
Level
of Difficulty
|
|
1
|
Atomic Structure
|
In 1932, a british scientist had found the neutron particle by…..
|
James Chadwick
|
Medium
|
|
2
|
Atomic structure
|
Each chemical element is
composed of particles called…..
|
Atoms
|
Easy
|
|
3
|
Reacting Volumes of gases
|
The combustion of one mol propane will produce………..( in mol)
|
3 mol CO2 and 2 mol
H2O
|
Medium
|
|
4
|
Concepts mol and Avogadro’s Constant
|
If Avogadro’s contant is 6.02 x 1023. The number of H2S
molecules in 0.4 mol of H2S is…
|
The number of H2S molecules = mol x 6.02 x 1023
= 2.4 x 1023
|
Medium
|
|
5
|
The ideal gas equation
|
If at STP condition, a gas has 4.25 gram of mass and 2.8 L of volume
, then the molar mass of gas is…
|
Volume gas in STP = mol x 22.4 L
-
Mol = mass/molar mass
Thus, molar mass of gas is 34
g/mol
|
Difficult
|
|
6
|
The empirical formula
|
An analysis on ionic compound shows that the compound contains 2.82
gram of sodium , 4.35 gram of chlorine, and 7.83 gram oxygen. The empirical
of the compound is….
|
Define the mass of element
Na : Cl : O
2.82/23 4.35/35.5 7.83/16
0.123 0.123 0.489
1 1 4
So. Its empirical formula is NaClO4
|
Difficult
|
|
7
|
Ionic Bonding
|
A chemical bond occurs in KBr is…
|
Ionic bond
|
Easy
|
|
8
|
Bonding
|
The atomic number of X is 13, and the atomic number of Y is 9. A
possible compound formed from X and Y is ..
|
X2Y3
|
Difficult
|
|
9
|
Exothermic and endothermic reaction
|
The majority of chemical reactions releases heat energy to their
surroundings.The type of the reaction is known as an……
|
Exothermic reaction
|
Easy
|
|
10
|
Calculation of enthalpy changes
|
80 gram of water (the specific heat capacity water is 4.18 J/g0C ) has the heat capacity….
|
Heat capacity = 4.18 x 80
=
334.4 J/0C
|
Medium
|
|
11
|
Atomic structure
|
Proton is discovered by….
|
Ernest Rutherford
|
Medium
|
|
12
|
Atomic structure
|
 memiliki jumlah neutron sebanyak… |
6
|
easy
|
|
13
|
Fundamental concepts of chemistry
|
Pure substances can be devided into….
|
The chemical elements and chemical compounds
|
easy
|
|
14
|
Calculating quantities
|
What is the mol of 22 gram propane (molar mass of propane = 44)…..
|
0.50 mol
|
medium
|
|
15
|
Ionic equation
|
the ionic equation of BaSO4 is…….
|
BaSO4 à
Ba2+ + SO42-
|
Medium
|
|
16
|
Solutions
|
The mixture of solvent and solute is termed a…
|
Solution
|
|
|
17
|
Mass number, atomic number, isotops
|
The total number of protons and neutrons is called….
|
The mass number
|
medium
|
|
18
|
Mass number, atomic number, isotops
|
Atoms of the same element that
have different mass number are called…
|
Isotopes
|
Medium
|
|
19
|
Physicals properties of element
|
The ability or power of an atom in a covalent bond to attract shared
pairs of electrons to itself kinown
as…
|
The electronegativity
|
Medium
|
|
20
|
Enthalpy changes
|
This potential energy stored in the chemical bonds known as…
|
Enthalpy
|
Medium
|
3.
Essay
|
Num.
|
Topic
|
Question
|
Answer
Key
|
Level
of Difficult
|
||||||
|
1
|
The ideal gas equation
|
How much is the volume of 8 gram of SO3 gas, at 1 atm
pressure and 270C temperature ( known Ar S = 32, O= 16 , and R = 0.082 L atm/mol K)
|
Mol SO3 = mass/Mr
= 8 / 80= 0.1 mol
Volume = nRT/P
V =
= 2.46 L
|
Medium
|
||||||
|
2.
|
Molecular formula
|
Vitamin C is a compound consisted of C, H and O. The compound has
molar mass = 176 g/mol. When 1 gram of
vitamin C sample is burnt using
combustion analysis instrument, it result the data :
Define the molecular formula of vitamin C
|
Define the mass of C and H using the chemical formula;
The element mass= compound mass x
Mass C = 0.409 g ,
Mass of H = 0.046 g
And O = 0.545 g
Devide the mass of each element with its Ar,
C = 0.0341
H = 0.0.46
O = 0.0341
So, the empirical formula is
C3H4O3
The molecular formula ;
(C3H4O3)n = Mr (176)
n = 2
So the empirical formula is (C3H4O3)2 = C6H8O6
|
Difficult
|
||||||
|
3
|
Atom structure
|
How much is the amount of proton, electron, and neutron in ion of S-2
that has 16 atomic number and 32 mass
number….
|
Atomic number = proton
So, proton = 16
Mass number = 32 = proton + neutron
So, neutron = 32-16 = 16
Electron = 16 – (-2) = 18
|
Easy
|
||||||
|
4
|
Bonding
|
The atomic number of P, Q, R and S are 6, 9, 11, and 18. Which pairs
of atoms will from ionic bonds?
|
Ionic bond are formed and between metallic and non-metallic ions. So,
the elements that can form an ionic bonds are:
a. R
and Q
b. R
and P
|
Medium
|
||||||
|
5
|
Energetics
|
What is exothermic and endothermic reaction, and example reaction for
each reaction?
|
Exothermic reaction is the majority of chemical reactions release
heat energy to their surroundings
Example :
CH4 + O2 à
CO2 + H2O ∆H
= - X kJ
Endothermic reactions are a few chemical reactions absorb heat energy
from their surroundings
Example
CaCO3 à
CaO + CO2 ∆H = + X kJ
|
Medium
|
||||||
|
6
|
Atomic structure
|
What are positive ions and negative ions ?
|
Positive ions are formed when atoms lose electrons
Positive ions are formed when atoms gains electrons
|
Medium
|
||||||
|
7
|
The periodic table
|
What is the members of group 1 in the periodic table…
|
Hydrogen, Lithium, Sodium, Pottassium, Rubidium, Caesium, fransium.
|
Medium
|
||||||
|
8
|
Ionic compound
|
Write side,, five the examples of ionic compounds
|
NaCl. KCl, LiCl, MgCl2,CaCl2
|
difficult
|
||||||
|
9
|
Covalent compound
|
Write side, five the examples of covalent compounds?
|
CO2, H2O, HCl, N2, O2
|
difficult
|
||||||
|
10
|
Fundamental concept of chemistry
|
What is decomposition?
|
The splitting of a chemical compound into its constituent elements
|
Medium
|
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