Academy for Excellence
chung Lahore
Chemistry-1st 09-10 Ch# 1 Paper:
Complete
Without Prob of Exercise Total Marks: 20
Name:
______________________________________________________Sec: ______________Roll:
_________________
A. Choose the correct
answer
1. Atoms of which gas can exist independently
a. O2 b. CO2 c. Ar d. N2
2. Atomicity of glucose (C6H12O6)
is
a.6 b.
24 c. 12 d. 18
3. There are many examples of anions having group of atoms
like
a. PO4 b. Cl c. P d. S
4. Which of the following is a charged particle
a. Element b.
Ion c. atom d. Molecule
5. Carbon is used as standard reference for relative atomic
mass due to
a. unstability of carbon b. stability of
carbon
c. abundance of carbon compounds
d. both b + c
6. Which of the following is not a property of Isotopes
a. Isotopes
have same chemical properties
b. Isotopes
have same atomic Number
c. Isotopes
have same physical properties
d. Isotopes
have same position in periodic table
7. Which of the following statement is true for mass
spectrometer
a. It uses
liquid molecules in magnetic field
b. Magnetic
field supply the voltage to vapours
c. It
separates Ions according to their mass only
d. All
Statements are wrong
8. A potential difference of 500 – 2000 volts is applied to
accelerate the positive Ions by
a. electric field b. magnetic field
c.
Ionization chamber d. electrometer
9. By combustion analysis, only those organic compounds can
be analyzed which simply contain
a. C , S , N b. C , H , O c. C , H , N d.
S , H , O
10. In elements and compounds, the Avogadro’s No correlates the
Number and masses of
a. Atoms b.
Ions c. Molecules d. All
11. Which statement about molar volume is true?
a. it is
denoted by Vm b. It is applicable only to an ideal gas
c.
normally in gases, one molecule is about 300 times at a greater distance
than its own diameter
d. All are
true
12. Theoretical yield is also called
a. expected
yield b. calculated yield c. both a + b d. none
13. The mass of one mole of electrons is
a. 1.008 mg b. 0.55 mg c. 0.184 mg d. 1.673 mg
14. 27 g of Al will react completely with
how much mass of O2 to produce Al2O3
a. 8g of
oxygen b. 16g of oxygen
c. 32g of
oxygen d. 24g of oxygen
15. The number of moles of CO2,
which contain 8.0 g of oxygen
a. 0.25 b. 0.50 c. 1.0 d.
1.50
16. The largest numbers of molecules are
present in
a. 3.6 g of
H2O b. 4.8g of C2H5OH
c. 2.8 g of
CO d. 5.4 g of N2O5
17. One mole of SO2 contains
a. 6.02 x 1023
atoms of oxygen b. 18.1 x 1023molecules
of SO2
c.
2 x 6.0223 atoms of sulphur d.
2 x 6.0223 atoms of oxygen
18. The volume occupied by 1.4g of N2
at S.T.P is
a. 2.24 dm3 b. 22.4 dm3 c. 1.12 dm3 d. 112 cm3
19. One atom mass unit is equal to
a. 1.66 x 10–27 kg b. 1.66 x 10–27 g c. 1.66 x 10–24 g d. Both a + c
20. Which of the following has eleven isotopes
a. Ni b.
S c.
Cd d. Sn
Give Short Questions
a). Why we use
limiting reactant deliberately
b). What is
gram molecule. Give two example
c). What is
Gram molecule. Give two examples
d). How
empirical formula is determined.
Q#2. Explain in detail mass spectrometry
-----------------------------------------------------------------------------------------------------------------------------------------
Give Short Questions
a). Why we use
limiting reactant deliberately
b). What is
gram molecule. Give two example
c). What is
Gram molecule. Give two examples
d). How
empirical formula is determined.
Q#2. Explain in detail mass spectrometry
-----------------------------------------------------------------------------------------------------------------------------------------
Give Short Questions
a). Why we use
limiting reactant deliberately
b). What is
gram molecule. Give two example
c). What is
Gram molecule. Give two examples
d). How
empirical formula is determined.
Q#2. Explain in detail mass spectrometry
-----------------------------------------------------------------------------------------------------------------------------------------
Give Short Questions
a). Why we use
limiting reactant deliberately
b). What is
gram molecule. Give two example
c). What is
Gram molecule. Give two examples
d). How
empirical formula is determined.
Q#2. Explain in detail mass spectrometry
-----------------------------------------------------------------------------------------------------------------------------------------
Give Short Questions
a). Why we use
limiting reactant deliberately
b). What is
gram molecule. Give two example
c). What is
Gram molecule. Give two examples
d). How
empirical formula is determined.
Q#2. Explain in detail mass spectrometry
-----------------------------------------------------------------------------------------------------------------------------------------
Give Short Questions
a). Why we use
limiting reactant deliberately
b). What is
gram molecule. Give two example
c). What is
Gram molecule. Give two examples
d). How
empirical formula is determined.
Q#2. Explain in detail mass spectrometry
-----------------------------------------------------------------------------------------------------------------------------------------
Give Short Questions
a). Why we use
limiting reactant deliberately
b). What is
gram molecule. Give two example
c). What is
Gram molecule. Give two examples
d). How
empirical formula is determined.
Q#2. Explain in detail mass spectrometry
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