all test 1st year fsc
Subject: Chemistry-I Chapter
# 01 Marks: 40
Roll.No: ……………. Name……….
Q.NO.1: Encircle the correct answer (12)
1.The number
of gram of element present in 100g of a
compound is called
(a) %age of
element (b) Empirical formula (c) Molecular
formula (d) Relative abundance of element
2.The empirical
formula of benzene is …………
a) C6H12O6 b) CH c) C6H6 d) CH2O
3. In combustion analysis the CO2 is absorbed by………..
a) H2O b) 50%KOH c)
Mg(ClO4)2
d) H2 SO4
4. One Mole of Glucose C6H12O6
contain ………… grams of Glucose
a) 342 b) 180 c) 238 d) 106
5. The volume occupied by 28g of N2 at STP is………
a) 2.24dm3 b) 22.414dm3 c) 112Cm3 d)
1.12dm3
6. The reactant which give …………. Amount of product is called
as limiting reactant.
a) less b) large c)
both a & b d)
none
7. The simplest formula which give the small whole number
ratio between the element in a compound is called as ………..
a) Molecular formula
b) Empirical formula c) Chemical
formula d) Structural formula
8. The graph which
gives the relative abundance of isotopes is called as ……….
a) Mass spectrometer
b) Mass spectrum c)
Electrograph d) Spectrograph
9. Electrometer is also called as ………………..
a) Mass spectrum b)
Accelerator c) Separator
d) Ion collector
10. A sample of pure matter is
(a) element (b) compound (c) substance (d) mixture
11. nm stands for
(a) Newton meter (b) Nanometer (c) Newton square meter (d) none of the above
12. The number of moles of CO2 which contains 8.0 gm of oxygen
(a) 0.25 (b) 0.50 (c) 1.0 (d) 1.50
(a) element (b) compound (c) substance (d) mixture
11. nm stands for
(a) Newton meter (b) Nanometer (c) Newton square meter (d) none of the above
12. The number of moles of CO2 which contains 8.0 gm of oxygen
(a) 0.25 (b) 0.50 (c) 1.0 (d) 1.50
Short Question. 10X2=20
- Why 23g of Na and 238g of U have same number of atoms?
- What is Molar Volume? Why different masses of different gases have same molar volume
- What are the steps to determine the empirical formula?
- Why Mg Atom is twice heavier than C atom?
- What are molecular ions. How they are produced?
- Why we can not obtain a clear and accurate image of an atom by using compound microscope?
- What is the Basic Principle of Mass spectrometery?
- What are Mono Isotopic elements? Give example
- What is average atomic mass? How it can be calculated explain with example.
- Why Actual yield is always less than theoretical yield?
Long Question (4x2=8)
- How Combustion analysis can be used to find out the empirical formula of a compound? Explain with example.
- What is Mass spectrometer? Discuss its function with the diagram and mass spectrum
......................................
Name…………………………………….…….. Test no.2 Roll
No:………………..chp03
Section………………. 1st
year Chemistry
Q.No. 1 Encircle the correction option. (12)
1) Number of molecules in one dm3 of
water is close to:
(a)6.02 x 1023 (b) 1x3.01x 1023 (c)5x6.02 x 1023 (d) 55.6 x 6.02 x 1023
2) The deviation of a gas from ideal behaviour
is maximum at,
(a) – 10 oC and 5atm (b) – 10 oC and 2atm (c) 100 oC and 2atm (d) 0 oC and 2atm
3) Which of the following have same no. of molecules at STP
3) Which of the following have same no. of molecules at STP
(a) 1000 cm3 of N2H4
and O2(b) 200 cm3 of CO2 and N2O(c)
50 cm3 each of CO and N2(d) all
4) If absolute temperature is doubled and the pressure is increased 4 times. The volume is
4) If absolute temperature is doubled and the pressure is increased 4 times. The volume is
(a) half
(b) double (c)
four times (d) remains the changed
5) Density of a gas is usually expressed in
5) Density of a gas is usually expressed in
(a) kg m3 (b) kg dm-3 (c) g dm–3 (d) g cm–3
6)Value of gas constant R in SI system is:
6)Value of gas constant R in SI system is:
(a) 0.0821 dm3atm k–1 mol–1 (b) 82.1 cm3atm k–1
(c) 8.31 Nm k–1 mol–1 (d) 1.987 cal k–1
mol–1
7) Concept of distribution of velocities among
the gas molecules was developed by
(a) Claudius
(b) Maxwell (c) Boltzman (d) Vander Waal
8) Deviation a gas from ideal behaviour is maximum at
8) Deviation a gas from ideal behaviour is maximum at
(a) low temperature, low pressure (b) low temperature, high pressure
(c)high temperature, low pressure (d) high temperature high
pressure
9) Most ideal gas at room temperature is:
(a) CO2 (b) NH3 (c) SO2 (d) N2
10)The value of compressibility factor for an ideal gas is equal to:
10)The value of compressibility factor for an ideal gas is equal to:
(a) 1
(b) 1.5 (c) 2 (d) 2.5
11)An ideal gas obeys
11)An ideal gas obeys
(a) Boyle’s law
(b) Charle’s law (c) Avogadro’s law (d)
all above
12)0.1 mole of any gas at STP occupies volume
12)0.1 mole of any gas at STP occupies volume
(a) 2.24 dm3 (b) 22.4 dm3 (c) 44.4 dm3
(d) 48.4 dm3
--------------------------------------------------------------------------------------------------------------------------------------------
Q.No. 2
Write Short answers of the following Questions. 10x2=20
1.
Why temperature is measured in Kelvin scale in order to apply
charle’s law on gases.
2.
How the density of the gas can be Calculated from general gas
equation.
3.
Justify that 1 Cm3 of O2 and 1 Cm3
of N2 have same no of molecules at STP.
4.
What is Aqueous Tension?
5.
Why do Pilots feel uncomfortable in breathing at higher altitude.
6.
Why lighter gases effuse and diffuse rapidly as compare to heavier
gases.
7.
Derive boyle’slaw from kinetic molecular theory of gases.
8.
What is Mean Squar Velocity? Why we use this term. Explain with
formula.
9.
Do you think that some of the postulates of kinetic molecular
theory of gases are faulty? Point out these postulates.
10.
What are the characteristics of plasma?
Extensive
Questions:- 4x2=8
1)One mole of methane gas is maintained at 300K. Its volume is 250 cm3.
Calculate the pressured exerted by the gas under the following conditions.
i)When the gas is
ideal. ii)when the gas is non-ideal.a
= 2.253 atm dm6 mol-2b
= 0.0428 dm3 mol-1
2) Working at a
vaccum line, a chemist isolated a gas in a weighing bulb with a volume of 255cm3
at a temperature of 25 C0 and under the pressure of 10.0torr. The gas weighed 12.1mg. What is the
molecular mass of this gas?
Grand Test#04 CHEMISTRY 1ST YEAR
Time: 1:30
minutes Chapter :03 Marks: 40
____________________________________________________________________________
Q.no1: MULTIPLE
CHOICE QUESTIONS: (12x1=12)
1.
For
which law, temperature and pressure are constant?
a.
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.
a)
4 b)
3 c) 10 d) 1
3.
Pressure
of water vapors is also called as:
a.
a)
Aqueous tension b) diffusion
c) effusion d) viscosity
4.
The
color of NO2 gas is:
a.
a)
Yellow b) colorless c) brown d) red
5.
Root
mean square velocity is directly proportional to:
a.
a)
molar mass b) temperature c) density d)
all of these
6.
So
far the minimum temperature attained is:
a.
a)
10-6 K b) 10-5
K c) 0K d) none of these
7. One atm is equal — psi
a) 14.8 b) 13.7 c) 12.7 d)
none
8.
Who
presented the kinetic molecular equation?
a.
a)
Boltzmann b) Maxwell c) Bernoulli d) Clausius
9.
Incompressible
volume of 1mole of hydrogen is:
a.
a)
0.0266 b) 0.0564 c) 0.0371 d) 0.0318
10.
Plasma
was discovered by:
a.
a)
Van der Wall b) William Crooks c) Linde d) Graham
11.
Which
is the 1.5 million kilometer ball of plasma?
a.
a)
moon b) earth
c) sun d)
Mars
12.
Minimum
temperature of natural plasma is:
a.
a)
20000C0 b)
2000C0 c) 2000C0 d) 200000C0
…………………………………………………………………………………………………….
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.
Why
polar gasses compressed easily?
6.
Why
is the idea of mean square velocity required?
7.
Differentiate
between diffusion and effusion.
8.
How
is cooling produced when a compressed gas is allowed to expand?
9.
Prove
mathematically that absolute temperature is directly related to average
translational kinetic energy.
10.
What
will be the molar mass of a gas which can diffuse 4 times rapidly than methane
gas?
Q.no3 EXTENSIVE QUESTIONS:
(4+4)
a)
Explain
Boyle’s law and Avogadro’s law from kinetic molecular equation.
b)
How
was the Ideal Gas Equation corrected for real gases?
Grand Test#5 CHEMISTRY 1ST YEAR
Time: 1:30
minutes Chapter :04 Marks: 40
____________________________________________________________________________
Q.no1: MULTIPLE
CHOICE QUESTIONS: (12x1=12)
1.Ionic bond is:
a) Intermolecular force of attraction b) Intramolecular force of attraction
c) Repulsive force d)
Adhesive force
2.Iodine is solid while chlorine is gas
because of:
a) Debye force b) dipole dipole force c) London force d) all of these
3.Ice occupies how much more space as
compared to liquid water?
a) 36% b) 27% c) 18% d) 9%
4.Hydrogen bonding is responsible for:
a) Cleansing action of soap b) tensile strength of fiber
c) Double helix of DNA d) all of these
5.Acetone and chloroform are soluble in
each other due to:
a) London force b) dipole dipole
force
c) Debye force d) hydrogen bonding
6.CO2 and SO2 are
both triatomic gases but possess different heats of vaporization because:
a) greater electronegative character
of sulphur b) greater
size of sulphur
c) CO2 is non polar &
SO2 is polar d)
SO2 is more acidic
7.What will be the melting temperature
of cholestryl benzoate?
a) 246K b) 145C0 c)
179C0 d)
-20C0
8.Vapour pressure of liquid is measured
when liquid and vapours are in equilibrium. It means
that:
a) both have same kinetic energy b)
both have same heat content c) rate of evaporation is equal to rate of
condensation d) all of these
9.In order to mention the boiling point
of water at 110C0, the external pressure should be:
a) between 760 and 1200 torr b) between
200 and 760 torr
c) 765 torr d)
any value of pressure
10.Ionic solids are characterized by:
a) low melting points b) conductivity in solid state
c) high vapour pressure d) solubility in polar
solvents
11.Which of the following is pseudo
solid?
a)
CaF2 b) glass c) NaCl
d) all of these
12.Which pair of species is isomorphic?
a) SO4-2 &
CrO4-2 b)
SO4-2 & NO3-1 c) SO4-2 & Cr2O7-2 d) all
…………………………………………………………………………………………………….
Q.no2. SHORT QUESTIONS:
(2x10=20)
1. why ionic solids are brittle? Explain.
2. What is anisotropy? Give example.
3. Why is unit of ionic solid not called
as molecule?
4. Differentiate between polymorphism and
isomorphism with one example each.
5. What is metallic luster?
6.
Why
is electrical conductivity decreased with increase in temperature in case of
metals?
7.
Why
is lattice energy of LiCl higher than that of NaCl?
8.
Evaporation
takes place at all temperatures. Explain why?
9.
Earthenware
vessels keep the water cool. Justify.
10. Heat of sublimation of iodine is very
high as compare to other halogens. Why?
Q.no3 EXTENSIVE QUESTIONS:
(4+4)
a) Define liquid crystals? What are their
properties resembling liquids and solids. Describe their uses.
b) Define instantaneous dipole induced
dipole forces of attraction. Also discuss the factors affecting these
attractive forces.
.........................................................................................................................................................................
Grand Test#6 CHEMISTRY 1ST YEAR
Time: 1:30
minutes Chapter :05 Marks: 40
____________________________________________________________________________
Q.no1: MULTIPLE
CHOICE QUESTIONS: (12x1=12)
1. The nature of positive rays depend
on the nature of:
a) Cathode rays b) discharge tube c) residual gas d)
all of these
2. The heaviest particle among all four
given particles is:
a) meson b) proton c)
neutron d) electron
3. ) A proton is identical to:
a) ionized H2 b) alpha particle c) Ionized H d) hydronium ion
4. The mass of neutron lies in the
range of:
a) 1.6750 x 10-23Kg b) 1.6750 x 10-24Kg c) 1.6750 x 10-27Kg d) 1.6750 x 10-26Kg
5. In Milikan Oil Droplet method, air
inside chamber is ionized by:
a) X rays b)
alpha rays c) beta
rays d) none of these
6) The energy of fast neutrons is more
than:
a) 2MeV b) 5.2 MeV c) 1.2 MeV d) none of these
7. Unit of wave number is:
a) cm- b) m- c) nm- d) all of these
8. Radius of 2nd orbit of
alpha particles is:
a) 0.529Ao
b) 2.11Ao
c) 4.75Ao d)
none of these
9. Electron revolving in 3rd
orbit of hydrogen atom will have energy:
a) -52.53 KJ/mole b) -82.08 KJ/mole
c) -145.92 KJ/mole d)-328.32 KJ/mole
10 The wavelength of blue light is
higher than that of:
a) violet b) green c)
yellow d) red
11. The unit of frequency is:
a) Hertz b) sec-1 c) cycle per second d) all
12. Who suggested the elliptical shape
of orbits?
a) bohr b)
Rydberg c) Milliken d) Sommerfield
…………………………………………………………………………………………………
Q.no2. SHORT QUESTIONS:
(2x10=20)
1. State Moseley’s law. Give its
application
2. Differentiate between atomic
absorption and emission spectrum..
3. Differentiate between wave number and
wave length
4. What are the uses of slow and fast
neutrons?
5. How would you prove that cathode rays
are negatively charged?
6. What are the defects of Rutherford
atomic model?
7. How would you calculate the mass of
electron from its e/m value?
8. Why is e/m value of positive rays
always less than that of electron?
9. Write the electronic configuration of
.. i) Ar ii) K
10. Differentiate between orbit and orbital
Q.no3 EXTENSIVE QUESTIONS:
(4+4)
a) Discuss in detail Millikan Oil Droplet
Method to find out the charge of electron.
b) Write a comprehensive note on Quantum
numbers.
....................................................................................................................................
Grand Test#7 CHEMISTRY 1ST YEAR
Time: 1:30
minutes Chapter :06 Marks: 40
____________________________________________________________________________
Q.no1: MULTIPLE
CHOICE QUESTIONS: (12x1=12)
1 The compromise distance of C-Cl bond
is:
a) 75.4 pm b) 77.3 pm c) 176.7 pm d) none of these
2. The bond energy of H2
molecule is:
a) 436 KJ/mole b)
486 KJ/mole c) 400 KJ/mole d)
none of these
3. ) -
Atomic radii can be measured by:
a) X- rays b) Cosmic rays c) spectroscopy d) both a & c
4. The mass of neutron lies in the
range of:
a) 1.6750 x 10-23Kg b) 1.6750 x 10-24Kg c) 1.6750 x 10-27Kg d) 1.6750 x 10-26Kg
5 The size of Al+3 is
smaller than:
a) Na+ b) Ca+2 c) Ga+3 d) all of these
6) The size of F- is smaller
than that of:
a) Br- b) O-2
c) N-3 d) all of these
7. Third ionization energy of magnesium
is:
a) 738KJ/Mole b) 1450KJ/Mole c)
7730KJ/Mole d) 9500 KJ/Mole
8. In BF3 molecule, for
bonding purposes, boron atom makes use of
a) 2s orbital b) 2p orbital
c) 3s orbital d)
sp2 orbital
9. -
If we want to change O2 to O2-1, the electron
is to be placed in:
a) δ2pz b) π2py c)
π*2py d)
π2px
10 Molecular orbitals are filled with
electrons according to:
a) Auf bau principle b) Hund’s rule c)
Pauli Exclusion Principle d) all
of these
11 Number of sigma bonds between two
carbon atoms in C2H2 is:
a) four b)
three c) two d) one
12. The carbon atom in CO2
is:
a) sp3 hybridized b) sp2 hybridized c) sp hybridized d) not hybridized
…………………………………………………………………………………………………
Q.no2. SHORT QUESTIONS:
(2x10=20)
1.
How
is the structure of ethyne explained by sp hybridization?
2.
Why
is MOT superior to VBT?
3.
Why
are 2nd and 3rd ionization energies higher than that of 1st
ionization energy?
4.
What
is screening effect and its effect on the ionization energy value?
5.
Why
do atoms combine chemically?
6.
How
would you calculate the bond order of helium?
7.
What
is the sequence of molecular orbitals of N2 with respect to energy
value?
8.
Why
is electron affinity of fluorine less than that of chlorine although fluorine
is more electronegative?
9.
How
is the molecule of BF3 triangular planar?
10. Why do atoms combine
chemically?
11. Why can we not
measure the exact atomic radius?
Q.no3 EXTENSIVE QUESTIONS:
(4+4)
a.
Explain
in detail the term electron affinity. Also discuss its trend in periodic table.
b.
Draw
molecular orbital diagram of oxygen. Also explain its paramagnetic character.
Grand Test#8 CHEMISTRY 1ST YEAR
Time: 1:30
minutes Chapter :07 Marks: 40
____________________________________________________________________________
Q.no1: MULTIPLE
CHOICE QUESTIONS: (12x1=12)
1 If exothermic reaction is allowed to
take place in air, temperature of surrounding will:
a) remains constant b) increases c)
decreases d) unchanged
2 The study of heat changes in a
chemical reaction is called as:
a) organic chemistry b) physical chemistry c) thermo chemistry d) inorganic chemistry
3. Most of the reactions which give stable
products are :
a) exothermic b) endothermic c) isobaric d) isothermal
4. The sign of w is positive when work
is done:
a) on surrounding b) by system c) by surrounding d) none
5 The relationship between internal
energy change, enthalpy and work done is:
a) ∆E - ∆H - W=0 b) ∆H=∆E+W
c) ∆E=W+∆H d)
∆H=∆E-W
6) At constant pressure, qv
is equal to:
a) ∆H b) ∆E c)
P∆V d) V∆P
7. -
Enthalpy of combustion of graphite, in magnitude, is:
a) 280KJ/mol b) 393KJ/mol c) 285KJ/mol d) none
8. For a given reaction, heat change at
constant pressure and constant volume are related as:
a) qp=qv
b) qp<qv c) qp>qv d) qp=qv/2
9. Bond dissociation energy of chlorine
molecule is:
a) 108 KJ/mol b) 496 KJ/mol
c) 121 KJ/mol d) 436
KJ/mol
10 The pressure of oxygen in bomb calorimeter
is:
a) 10 atm b) 20 atm c) 1 atm d) 15 atm
11 16.2 KJ/mol is enthalpy of solution
of:
a)
NH4Cl b) Na2CO3 c) C2H5OH d) MgO
12. Structure, bonding and properties of
ionic compounds are explained by:
a) enthalpy b) lattice energy c) internal energy d)
free energy
…………………………………………………………………………………………………
Q.no2. SHORT QUESTIONS:
(2x10=20)
1.
How
would you differentiate between heat and work?
2.
Is
spontaneous reaction always exothermic? Support your answer with example
3.
Define state and state function.
4.
Why does heat change occur during a chemical
reaction?
5.
Differentiate between spontaneous and non
spontaneous process.
6.
Why
can we not measure the enthalpy of formation of CCl4 directly?
7.
What is the structure of Bomb calorimeter?
8.
What
do you mean by the term enthalpy of neutralization?
9.
Why
is it necessary to mention the physical states of reactants and products in
thermo dynamical properties?
10. How would you calculate the enthalpy of
formation of CO?
Q.no3 EXTENSIVE QUESTIONS:
(4+4)
1) How would you calculate the lattice
energy of NaCl using Born Haber cycle at constant pressure?
2) State first law of thermodynamics.
Explain it when heat is supplied to the system at
constant pressure
Grand Test#9 CHEMISTRY 1ST YEAR
Time: 1:30
minutes Chapter :08 Marks: 40
____________________________________________________________________________
Q.no1: MULTIPLE
CHOICE QUESTIONS: (12x1=12)
A chemical reaction which proceeds
only in one direction is called:
a) addition reaction b)
decomposition reaction
c) reversible reaction d)
irreversible reaction
2 -
In a chemical reaction, equilibrium is said to have established when:
a) temperature of opposing reaction is same
b) velocities of opposite reactions become
equal
c) opposing reactions cease
d) concentration of reactants and
products are equal
3. The units of equilibrium constant Kc
for H2 + I2 ------------------ 2HI :
a) mol-1dm3 b)
mol-2dm3 c) moldm-1 d)
none
4. The Law of Mass Action was given by:
a) Guldberg & Waage b) Vant Hoff c)
Dalton d)
Lechatelier
5 -
For reaction 2A + B ----------- C,at equilibrium, [A]=0.2, [B]=0.45,
[C]=0.15 moles. What is Kc?
a) 0.83 b) 0.93 c)
83 d)
93
6) -
The factor of volume is in denominator in equilibrium constant expression for
the reaction:
a) synthesis of NH3 b) formation of ester c)
dissociation of PCl5 d)
any of these
7. Which is the part of catalyst for
ammonia production?
a) magnesia b) alumina c)
silica d)
all of these
8. The solubility of lithium salts
normally increases, when temperature:
a) decreases b) increases c) no change d) cant be predicted
9. By decreasing the concentration of
any of products, the value of Kc:
a) decreases b) increases c) no change d) cant be predicted
10 Almost forward reaction is complete
when Kc value is:
a) very large b) very small c)
moderate value d) cant’ be
predicted
11 “C” represents the concentration in:
a) moles b) mole/dm3 c) dm3
d) all of these
12. How much of total ammonia in world
is used to prepare fertilizers?
a) 50% b)
60% c) 70% d) 80%
…………………………………………………………………………………………………
Q.no2. SHORT QUESTIONS:
(2x10=20)
1.
What
is the relationship between Kp & Kc?
2.
How
equilibrium constant can help in determining the direction of reaction?
3.
How
can we find out the extent of reaction from Kc value?
4.
What
happens to the reaction at equilibrium if more reactants are added?
5.
What
is the effect of catalyst on equilibrium constant
6.
What
do mean by state of dynamic chemical equilibrium?
7.
Calculate
the units of equilibrium reaction for N2 + 3H2
------------- 2NH3.
8.
Derive
an expression for equilibrium constant for 2HF---------------- H2 +
F2.
9.
Calculate
the equilibrium constant expression for formation of ester.
10. Differentiate between reversible and
irreversible reactions.
Q.no3 EXTENSIVE QUESTIONS: (4+4)
1) State Le chatelier principle. Explain
in detail the effect of change in pressure or volume on equilibrium position.
2) State and explain Law of Mass Action.
Time: 1:30
minutes Chapter :09 Marks: 40
____________________________________________________________________________
Q.no1: MULTIPLE
CHOICE QUESTIONS: (12x1=12)
- Which one is not a colligative
property?
a) lowering of vapor pressure b) elevation of boiling
point
c) depression of freezing point d) boiling point
2-
Solubility of cesium sulphate does not decrease after:
a) 100 C0 b) 20 C0 c) 40 C0 d) 30 C0
3-
Maximum increase in solubility with increase in temperature is for:
a) KNO3 b)
KBr c)
KCl d) KI
4-
Solubility of copper sulphate in water at 100 C0 is:
a) 14.3g/100g b)
75.4g/100g c) 37.5g/100g d) 10g/100g
5-
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
6-
Which must be the
condition for the colligative properties?
a) solution should be dilute b) solute
should be non volatile c) solute should be non electrolyte d) all
7-
Beckmann thermometer can read up to:
a) 0.1K b) 0.001K c)
0.01K d)
1K
8- Elevation of boiling point is directly related with:
a) ppm b) %w/w solution c) molarity d)
molality
9-
When 6g urea is dissolved in 500g water, elevation of boiling point will be:
a) 10 C0 b) 0.1 C0 c)
0.52 C0 d)
none
10-
Relative lowering of vapor pressure is equal to:
a) mole fraction of solute b) mole fraction of
solvent
c) total mole fraction of solution d) all
11 The number of water molecules
attached to SO4-2 in CuSO4 is:
a) 1 b)
2 c)
3 d) 4
1215g urea is dissolved in 180cm3
solution of water. The relative lowering of vapor pressure is:
a) 0.024 b) 25.024
c) 2.5
d) none
…………………………………………………………………………………………………
Q.no2. SHORT QUESTIONS:
(2x10=20)
1) How are colligative properties
helpful in daily life?
2) Why is hydration energy decreased
from top to bottom in halogens?
3) Pure benzene (C6H6)
has vapor pressure 122 torr at 32C0.When 20g of solute is
dissolved in 300g of benzene, a vapor pressure
of 120 torr was observed. Calculate
molecular mass of solute.
4) Derive equation for the molecular
mass of solute from relative lowering of vapor
pressure
5) Differentiate between ideal and non
ideal solution.
6) Define zeotropic and azeotropic
mixtures with examples.
7) Differentiate between positive and
negative deviation from Raoult’s law.
8)Why does lowering of vapor pressure
take place when solution is formed?
9) Derive equation for the molecular mass
of solute from relative lowering of vapor
pressure.
10) Differentiate between cryoscopic and
ebullioscopic constant.
Q.no3 EXTENSIVE QUESTIONS:
(4+4)
1) Define solubility. Discuss the
solubility curves.
2)Mention
different statements of Raoult’s Law. Calculate the equation when both the
components are volatile.
...........................................................................................................
.....Grand Test #11 CHEMISTRY 1ST YEAR
Time: 1:30
minutes Chapter :10 Marks: 40
____________________________________________________________________________
Q.no1: MULTIPLE
CHOICE QUESTIONS: (12x1=12)
1-Conversion of electrical energy into
chemical energy is done in:
a) voltaic cell b) galvanic cell c)
electrolytic cell d) both
a and b
2-
The oxidation number of oxygen is +2 in:
a) Na2O2 b) KO2 c) OF2 d) CaO
3-
- Oxidation number of Mn in KMnO4
is:
a) +7 b) +6 c)
+5 d)
zero
4-
The algebric sum of oxidation number of all elements in a molecule is:
a) positive b)
negative c) zero d) any of
these
5 In acidic media, oxygen atoms are
balanced by adding:
a) H2O b) OH-
6- The oxidation state of carbon in C2O4-2
is:
a) +3 b)
+4 c) -4 d) -3
7- Conversion
of chemical energy into electrical energy is done in:
a) voltaic cell b) galvanic cell c)
electrolytic cell d) both
a and b
8- Redox equation is split up into two half reactions in:
a) ion electron method b) oxidation
number method
c) inspection method d) hit and
trial method
9- SHE is made up of:
a) hydrogen b) HCl
c)
Platinum d) zinc
10-
Oxidation potential of zinc is:
a) -0.34V b) +0.76V c) +0.34V d) -0.76V
11 caustic soda is obtained by
electrolysis in:
a) Castner Kellner cell b)
Hg cell c)
Nelson cell d) all of these
12 Salt bridge contains the aqueous
solution of:
a) KNO3 b) KCl c) KBr d) all of these
…………………………………………………………………………………………………
Q.no2. SHORT QUESTIONS:
(2x10=20)
1) Define electrochemistry.
2) What is the rule for oxidation number
of hydrogen and oxygen?
3) Differentiate between electrolytic and
voltaic cell.
4) What is the oxidation state of
chromium in Cr2(SO4)3.
5) Calculate oxidation number of
phosphorus in Na3PO4.
6) What is the function of salt bridge?
7) What is electrical double layer?
8) How is aluminium prepared from Hall
Beroult process?
9) How can you purify the copper?
10) What is the construction of standard
hydrogen electrode?
Q.no3 EXTENSIVE QUESTIONS:
(4+4)
1) Balance the following equation by ion
electron method.
Cr2O7-2 + Fe+2 Cr+3 + Fe+3 (acidic
medium)
2) How is electrode potential of copper
and zinc measured?
.
........................................................................................
Grand Test#12 CHEMISTRY 1ST YEAR
Time: 1:30
minutes Chapter :11 Marks: 40
____________________________________________________________________________
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)Velocity constant is the rate
of reaction when the concentrations of reactants are
c) Zero b) unity c) two d) three
4) Hydrolysis of Tertiary butyl bromide has order of reaction
. a) First order c) Pseudo
first order
c) third order d) Second
order
5) The rate of reaction has the dimensions of
a) moles dm-3 b) mole dm-3 s-1 c) mole dm-3 s-1 d) mole dm-6 s-1
) 6)The units of rate constant is same
as that of the rate of reaction is
a) frits order
reaction
b) second order reaction
c) zero order
reaction
d) third order reaction
7) the true representation for the units of rate constant K for the
firest order reaction is
a) sec-1 b) mol dm3 s-1 c) mol dm-3 s-1 d) mol -1 dm-3 s
8) According to collision theory, the rate of reaction is equal to
a) number of
collisions
b) concentration of reaction
c) concentration of
reaction
d) All
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)
Difference between average and instantaneous rate of reaction? 14
2)
Difference between rate and rate constant of a reaction?
3) When the
reaction becomes zero order? What is a zero order reaction?
4) Define
activation energy and activated complex.
5) What is a
promoter or activator? Explain Activation of catalyst.
6) What is
meant by rate determining step?
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)
a. Write a
detailed note on order of reaction?
b. Write a note
on Arrhenius equation. .
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