Physical Chemistry Grand Test #1
1. The heat
content of a system is called;
a) Internal energy
b) Enthalpy c) Entropy
d) Potential energy
2. Which of the
following contains two significant figures?
(a) 0.04
(b) 0.004
(c) 0.0004 (d) 0.042
3. Apparent charge on atom
in a molecule or ion is known as;
(a) Oxidation number (b)
Valency ( c) Electron (d) Reduction
number
4. Na+ is
isoelectronic with:
(a) Mg2+
( b) Ar
(c)
Na (d) Fe2+
5. The
empirical formula of a compound is CH2O and its molecular mass is
60. It‘s molecular formula is;
a) CH2O b)
C2H4O2
c) C3H6O3
(d) C4H8O4
6. Which of the
following have the same number of molecules at S.T.P?
a) 1dm3 of N2 &
O2 b) 500cm3 of CI2 &
O2
c) 100cm3 of CO2 & O2
d) All of these
7. Which has
minimum bond energy?
a) H – F
b) H – I c) H –
Cl d) H – Br
8. Highest
Hydration Energy is for;
a) Li+ b)
Na+
c) k+ d) Rb+
9. Which
statement correct for H2 + I2 + Heat ⇌ 2HI
a) HR > HP
b) HP > HR
c) HR = HP
d) NONE
10. 3.01 x 1023 molecules
of oxygen gas at STP occupy a volume of;
a) 25.5dm3
b) 22.4dm3
c) 11.2dm3
d) 2.24dm3
11. Orbitals
having same energy are called:
(a) Degenerate
Orbitals (b)
Valence Orbitals
(c) Hybrid Orbitals
(d) Bonding Orbitals
12. Viscosity
is following property;
a)
Extensive b)
Intensive c)
Normal d) Liquid
13. Water in a
glass. The glass is;
a) System
b) Surrounding c)
Boundary d) All of these
14. The formula of Aluminum
phosphate is;
a) AIPO4 b)
AI2(PO4)3 c)
AI3(PO4)3 d)
AI3(PO4)2
15. Isotopes contain the
same number of;
a) Electron
b) Physical properties c) Neutron
d) Proton
16. The
addition of catalyst to the reaction would cause a change, in which of the
following indicates the change of enthalpy of the reaction (∆H);
a) I
b) II
c) III
d) I & II
17. Which is not a state
function?
a)
Pressure b)
Temperature c)
Work d)
Volume
18. The
unit of the rate constant of the reaction; 2NO +O2 ® 2NO2:
a) dm6.mol‒2. Sec-1 b) dm3.mol‒1.sec‒1
c)
mol.dm‒3.sec‒1 d)
Sec‒1
19. The
activation energy of a reaction may be lowered by.
a) Raising
temperature b)
Lowering
temperature c)
Removing temperature d) Adding Catalyst
20. A
rise of 10K rise in temperature approximately ___________the rate of reaction.
a)
Half b)
Double c)
Thrice d)
Four times
21. Order
of reaction of the reaction 2NO + O2 ® 2NO2 is
_____________.
a)
One b)
Two c)
Three d)
Zero
22. Lighter
gasses diffuse ______________ than heavier gasses.
a)
Faster b)
Slower c)
Same
rate d)
None
23. Density
of a gas may be express by.
a)
PM/RT b)
M/V c)
V/M d)
nPM/RT
24. Water
forms _______________meniscus with glass.
a)
Concave b)
Convex c)
No d)
Both a and b
25. Which
one contains less number of molecules?
a) 98g H2SO4 b)
48g O2 c)
32g CH4 d)
10g H2
26. The
volume occupied by 14g of N2 at STP_____________dm3.
a) 22.4 b)
2.24 c)
1.673 d)
11.2
27. Beta
rays are:
(a)
Helium
Nuclei (b)
Electron (c)
Proton (d)
Neutron
28. Very
small Kc value shows;
a) Complete reaction b) Product is much more
c)
Forward reaction with negligible speed d) None
29. Which
of the following orbital has the greatest n+l value?
a)
5s b)
4d c)
4s d)
4f
30. The oxidation state of O in Na2O2 is:
a) – 1 b) – ½ c) 1/2 d) 1
31. For
a sparingly soluble salt the precipitation will occur if the product of ionic
concentration is;
a) Less than Ksp b)
greater than Ksp c)
Equal to Ksp d)
None of the above
32. A
beaker containing 180g of water contains following number of molecules;
a) 6.02 x 1023 b)
6.02 x 1024 c)
10.02 x 1023 d)
12.01 x 1023
33. One debye (D) is equal to:
a) 3.34 x 10‒28cm b) 3.34 x10‒38cm
c) 3.34 x 10‒30cm d) 4.184 x 10‒30cm
a) Evaporation b) Condensation c) Sublimation d) Fusion
35. The reaction proceeds at a rate that is independent of the concentration of that reaction is:
a) Rate of reaction b) 3rd order reaction
c) Zero order reaction d) Chemical reaction
36. Which
one of the following is a pure atomic orbital?
a) sp2 b)
d c)
sp3 d)
sp3d2
37. Which
type of overlaping is found in HF molecule?
a) s – s b) s – sp3 c) s – p d) p – p
38. The
rate of diffusion of Methane at a given temperature is twice that of ‘x’. The
molecular mass of ‘x’ is;
a) 64 (b) 16 (c)4 (d) none
39. The
unit of dipole moment is;
a) Calorie b) Debye c) Poise d) Newton
40. The
mass of 11.2 dm3 oxygen gas at STP;
a) 16g b)
24g c)
32g d)
48g
41. For
reaction 2NH3 ⇌ N2
+ 3H2
a) Kp = Kc b) Kp > Kc c) Kp < Kc d) None
42. Vapour
pressure of water at 100oC is;
a) 55 mm Hg b) 760 mm Hg c) 355mm Hg d) none of above
43. The
shape of diamond crystal is;
a) cubic b) hexagonal c) tetragonal d) orthorhombic
44. The number of orbitals in a shell can be determined by the formula:
(a) (2l+1) (b) n2 (c) 2(2l+1) (d) 2n2
45. Empirical formula for glucose is
(a) CH (b) CH2O (c) CO2 (d) H2O
46. The formula which represents actual number of atoms of each element in a molecule is called:
(a) Molecular Formula (b) Empirical Formula
(c) Atomic Formula (d) Compound Formula
47. Absolute zero is equal to:
(a) -273.15K (b) -273.15oC (c) -273.15K (d) -237.15oC
48. The oxidation number of Sulphur in Na2S2O3 is:
(a) +6 (b) +4 (c) +3 (d) +2
49. Bohr’s atomic
radius for n=1 is:
(a) 0.5 29 oA (b) 5.29 oA (c) 0.05 oA (d) 52.9oA
50. Ice is the example of which crystal:
(a) Atomic (b) Ionic (c) Covalent (d) Molecular
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