combined chapter 2 test 1st year
Grand Test#1 CHEMISTRY 1ST YEAR
Time: 1:30
minutes Chapter :01,02,08,09,10,11 Marks:
44
____________________________________________________________________________
1) Molecularity
of a chemical reaction:
a) cannot be less than
2 b) can have a
fractional value
c) can be zero d) is always
a whole number
2) when a reaction proceeds in a
sequence of steps the overall rate is determined by
a) fastest step b) slowest
step
c) order of different
step d) molecularity
of all step
3) In acidic media, oxygen atoms are
balanced by adding:
a) H2O b) OH-
4) Conversion
of chemical energy into electrical energy is done in:
a) voltaic cell b) galvanic cell c)
electrolytic cell d) both
a and b
5) Oxidation
potential of zinc is:
a) -0.34V b) +0.76V c) +0.34V d) -0.76V
) 6) Elevation of boiling point is directly related with:
a) ppm b) %w/w solution c) molarity d)
molality
7) The number of water molecules attached
to SO4-2 in CuSO4
is:
a) 1 b)
2 c)
3 d) 4
8) Molal
boiling point constant of ethanol for 1molal solution is:
a)
1.75 C0 b)
2.70 C0 c)
0.52 C0 d)
79 C0
9) A substance, which retards the rate of a reaction is called.
a) Inhibitor b) Activator c) Autocatalyst d) None
10) The acid hydrolysis of ethyl acetate in the
presence of mineral acid is
a) zero order
b) first order
c) pseudo first
order
d) second order
11) If the product of a
reaction itself acts as a catalyst as K [H2] [Br2] ½
is
a) homocatalysis b)
autocatalysis c) negative
catalysis d)
heterocatalysis
12) the order of a reaction can be
a) positive
integer b) zero c) in
fraction d) All
…………………………………………………………………………………………………
Q.no2. SHORT QUESTIONS:
(2x10=20)
1) Define zeotropic and azeotropic mixtures with examples
2) Differentiate between positive and negative deviation from Raoult’s law.
3) Differentiate between cryoscopic and ebullioscopic constant.
4) What is the function of salt bridge?
5) Differentiate between electrolytic and voltaic cell.
6) Define electrochemistry.
7) A catalyst is specific in its action. Give
reason
8) The
radioactive decay is always a first order reaction. How?
9) Define
activation energy and activated complex.
10) How does
a catalyst effect the reversible chemical reactions?
Q.no3 EXTENSIVE QUESTIONS:
(4+4+4)
a. Write a
detailed note on Solvent Extraction.
b. Write a note
on Arrhenius equation.
......................................................................................................................
Grand Test#2 CHEMISTRY 1ST YEAR
Time: 1:30
minutes Chapter :03,04,05 Marks: 40
____________________________________________________________________________
Q.no1: MULTIPLE
CHOICE QUESTIONS: (12x1=12)
1.
For which law, temperature and pressure are constant?
a) Boyle’s law b)
Graham’s law c) Charles law d)
both a & b
2.
The sum of mole fraction of all the 10 different components in mixture is:
a) 4 b)
3 c) 10 d) 1
3.
Pressure of water vapors is also called as:
a) Aqueous tension b)
diffusion c)
effusion d) viscosity
4.
The color of NO2 gas is:
a) Yellow b)
colorless c) brown d) red
5. Which of the following is pseudo solid?
a) CaF2 b)
glass c) NaCl
d) all of these
6. Acetone and chloroform are soluble in each other
due to:
a) London
force b)
dipole dipole force
c) Debye
force d)
hydrogen bonding
7. Hydrogen bonding is responsible for:
a) Cleansing action of soap b) tensile strength of fiber
c) Double helix of DNA d) all of these
8.Iodine is solid while chlorine is gas because of:
a) Debye
force b) dipole dipole force c) London force d) all of these
9.In Milikan Oil Droplet method, air inside chamber is ionized by:
a)
X
rays b) alpha rays c) beta rays d) none of these
10. The unit of frequency is:
a) Hertz b) sec-1 c) cycle per second d) all
11. Who suggested the elliptical shape of orbits?
a) bohr b) Rydberg c) Milliken d) Sommerfield
12.
The heaviest particle
among all four given particles is:
a) meson b)
proton c)
neutron d) electron
…………………………………………………………………………………………………….
Q.no2. SHORT QUESTIONS:
(2x10=20)
1. What
are the causes for deviation from non ideality?
2. What
are the characteristics of plasma?
3. Give
two uses of plasma.
4. Water
vapours don’t behave ideally at 273K why?
5. Heat
of sublimation of iodine is very high as compare to other halogens. Why?
6.
Why is lattice energy of LiCl higher than that of
NaCl?
7.
why ionic solids are brittle? Explain.
8.
State Moseley’s law. Give its application
9. How
would you prove that cathode rays are negatively charged?
10. Why
is e/m value of positive rays always less than that of electron?
Q.no3 EXTENSIVE QUESTIONS:
(4+4)
a) Explain Boyle’s law and Avogadro’s law from kinetic molecular equation.
b) Write a comprehensive note on Quantum numbers.
Comments