(Inter Part- I)
SARGODHA BOARD
CHEMISTRY 2013
Chemistry (Objective) (Group-1) (New Scheme Paper (1)
Time Allowed: 20 minutes Maximum marks: - 17
Note:- You have four choices for each objective we question as A, B, C and D. The choice which you think is correct till that circle in front of that question number. Use marker or pen to fill the circles, Cutting or filling two or more, circles with result in zero mark in that question. Attempt as many questions as given in objective type question paper and leave others blank. Write the letter A, B, C or D in the column (write correct option) against each question. If there is a contradiction in the bubble and hand written answers bubble option will be considered correct.

Question#1

• Swedish Chemist J. Brezelius determine:
  
  (A) Al.no
  (B) Al.mass
  (C) Mol.mass
  (D) Ionic mass
  
  
• 27 gm of Al react completely with how much mass of oxygen to produce Al₂O₃.
  
  (A) 8 gm of Oxygen
  (B) 16 gm of Oxygen
  (C) 32 gm of Oxygen
  (D) 24 gm of Oxygen
  
  
• A component having small value of K( (distribution Coefficient) mostly remains in the:
  
  (A) Stationary phase
  (B) Mobilc phase
  (C) Chromatographic Phase
  (D) Solvent
  
  
• the molar volume of CO₂ is maximum at:
  
  
• (A) STP
  (B) 127⁰C and 1 atm
  (C) 0⁰C and 2 atm
  (D) 273⁰C and 2 atm
  
  
• The distillation of Liquid under reduced pressure is called:
  
  (A) Destructive distillation
  (B) Vacuum distillation
  (C) Fractional distillation
  (D) Simple distillation
  
  
• Allotropy the property of:
  
  (A) Compound
  (B) Element
  (C) Atom
  (D) Mixture
  
  
• Lyman series lies Spectral region:
  
  (A) Infra red
  (B) Ultra violet
  (C) Visible
  (D) None of these
  
  
• Which equationcorrectly represent the Heisenbergs uncertainly principle?
  
  (A) ΔX. ΔP=h/4π
  (B) ΔX. ΔP>h 4π
  (C) ΔX. ΔP>=h/4π
  (D) ΔX. ΔP<=h/4π
  
  
• Thc pharmagnetic behavior of Oxygen is well explained on the basis of:
  
  (A) M.O theory
  (B) VSEPR theory
  (C) V.B theory
  (D) C.F theory
  
  
• Which of the Hyrdrogen halides has the highest percentage of ionic character:-
  
  (A) HCI
  (B) HI
  (C) H.Br
  (D) HF
  
  
• For a given proeess, the heat changes at constant pressure(q_o) and constant volume(q_v) are related to each other as:
  
  (A) q_p=q_v
  (B) q_p<q_v
  (C) q_p>q_v
  (D) q_p=q_A
  
  
• By adding NH₄Cl to NH₄OH. The ionization of NH₄OH:
  
  (A) Increase
  (B) Remain same
  (C) Decrease
  (D) Increase 100 times
  
  
• The solubility product of AgCl in 2.0x10^-10 mole² dm^-6 the maximum concentration of Ag1 ions in the solution is (M. mass AgCl 143.5)
  
  (A) 2.0x10^-10 mole dm^-6
  (B) 1.41x10^-5 mole dm^-6
  (C) 1.0x10^-10 mole dm^-6
  (D) 4.0x10^-20 mole dm^-6
  
  
• An aqueous solution of methanol in water has vapour pressure.
  
  (A) Equal to that of water
  (B) Equal to that of methonal
  (C) More than that of water
  (D) Less than that of water 
  
  
• If a strip of Cu is placed in a solution of FeSO₄.
  
  (A) Cu will be precipitated out
  (B) Fe is precipitated out
  (C) Cu and Fe both dissolves
  (D) No reaction take place
  
  
• Oxidation No of C in C₁₂H₂₂O₁₁ is:
  
  (A) Zero
  (B) -6
  (C) +6
  (D) 12
  
  
• The rate of reaction determined at any given time is called
  
  (A) Average rate
  (B) Instantancous rate
  (C) Seprate
  (D) Over all rate

SUBJECTIVE-PART
GROUP-I

2. Answer briefly any Eight parts from the followings:- • (8x2 = 16 )

• Flow limiting reactant is identified
• Calculate the number of Oxygen atoms in 0.1 mole .
• Why no individual neon atom in the sample of the element has a mass of 20.18a.m.u
• Give the salient feature of an ideal solvent?
• Why is the difference between absorption and partition Chromatography?
• why the graph plotted between pressure and volume moves away from pressure axis at higher temperature. 
• Derive the Si units of R (General gas constant)
• Define Diffusion and effusion
• Why electrical conductivity of metals decreases on increasing temperature?
• Why O has higher boiling point than HF
• Why Graphite is a good conductor of electricity?
• Why boiling point of water is different at Murree Hills and at Mount Everest?

3. Answer Briefly any eight Parts from the following

• Which particles arc formed by the decay of free Neutrons?
• What is Zeeman effect
• What is the function of principal quantum number?
• State Moseley’s law. Give its mathematical expression.
• Ionization energy is index to the metallic character. Why?
• What is Co-ordinate Covalent bond? Give one example.
• Why Sigma bond is stronger than Pi bond. 
• Define Dipole moment. Give its S.I unit.
• Differentiate between endothermic and exothermic reaction. Give one example
• What is standard enthalpy of solution? Give one example. 
• How ammonia is synthesized by Hyber’s process. Also give the optimum conditions of reaction.
• A mixture of NS and NCL give basic buffer. Justify it.

4. Answer briefly any six parts from the following (6x2=12).

• Buffers are important in many areas of chemistry. Justify.
• NS.10O shows discontinuous solubility curve. Give example
• Give two applications of colligative properties.
• What is the molality of solution prepared by dissolving5g of Glucose in 250g of Water.
• Balance the equation by oxidation number method Br₂+ NaOH →NaBr+NABrO₃+ H₂O
• Lead accumulator is a chargeable battery. Justify it.
• What is Electro Chemical series? Give its once application
• Define Heterogeneous Catalysis with example.
• What is rate of reaction also give name of four physical methods used to determine the rate of reaction.

Section – II

Note: Attempt any three questions.
Question#5
(a) Write note on the factors affecting the strength of London forces.
(b) N can be produced by heating together two solids NH₄Cl and Ca(OH)₂. If a mixture containing 800g of each solid is heated then how many grams of Nis produced

2NH₄Cl +Ca(OH)₂→CaCl₂+2NH₃+2H₂O  at mass of Ca-40

Question#6
(a) What is an Orbital hybridization? Explain Sp³ hybridization with two example.
(b) Define Lattice energy and Born- Haber Cycle. How Lattice energy is measured by Born Haber Cycle. write equation of different enthalpy changes in the formation of NaCl from its elements.

Question#7
(a) What is Kinetic molecular theory of gases. Give its postulates
(b) Discuss
(i) Azimuthal Quantum number and
(ii) Magnetic quantum number

Question#8
(a) Describe the electrolysis of molten sodium chloride and a concentrated solution of sodium Chloride.
(b)The solubility of PbF₂ at 25°C ;is is 0.64gdm^-3. Calculate K_ep of PbF₂ mol. Mass of PbF₂245.2gmole^-1

Question#9
(a) Define Non ideal solution and explain positive deviation with the help of a graph.
(b) What is catalysis? Write down its types and explain any one of the them briefly.

Section – III

10. Note:Attempt ant three parts

(A) Write down standard solution, chemical equation with mole ration , indicator with end point procedure and supposed reading with calculations for A, B, C and D.
(B) Write down material required Diagram and procedure for part D and E.
(C) The given solution contains 8g NaOH dissolved per dm³ . Determine percentage purity of NaOH volumetrically. (Molecular mass of NaOH=40)
(D) The Given solution contains 30 g of FeSO₄.7H₂O m 500 cm³ solution volumetrically (Molar mass of FeSO₄.7H₂O=278)
(E) Determine the percentage of Iodine in the Given sample solution . The Sample solution contains10g Iodine dissolved per of solution (Molecular mass of Iodine =254)
(F) You are provided mixture of various inks. Separate them by paper chromatography.
(G) Prepare the Crystals of Benzoic acid from water as solvent by crystallization method.

Inter part - I
Chemistry
(Objective Type)
Group – II
(New Scheme)
Time: 20 Minutes
Marks: 17
Note: Write answers to the questions on the objective answer sheet provided. Four possible answers A, B, C and D to each question are given. Which answer you consider correct, fill the corresponding circle A, B, C and D given in front of each question with Marker or pen ink on the answer sheet provided.

Question#1

• The volume occupied by 1.4g of N₂ at S.T.P is
  
  (A) 24 dm⁴
  (B) 22.4 dm³
  (C) 1.2 dm³
  (D) 11.2 dm⁴
  
  
• The largest number of molecules are present in
  
  (A) 6 g of H₂O
  (B) 4.8 g of C₂H₃OH
  (C) 2.8 g of CO
  (D) 5.4 g of N₂O₃
  
  
• During the process of crystallization the hot saturated solution.
  
  (A) Is cooled very slowly to get large sized crystals
  (B) Is cooled at moderate rate to get maximum sized crystals
  (C) Is evaporated to get the crystals of the product
  (D) Is mixed with an immiscible liquid, to get the pure crystals of the product
  
  
• If absolute temperature of the gas is doubled and the pressure is reduced in one half, the volume of the gas will
  
  (A) Remains unchanged
  (B) Increase four times
  (C) Reduce to 1/4
  (D) Be doubled
  
  
• In order to mention the boiling point of water at 110^oC the external pressure should be
  
  (A) Between 760 torr and 1200 torr
  (B) Between 200 torr and 760 torr
  (C) 765 torr
  (D) Any value of pressure
  
  
• Ionic solids are characterized by
  
  (A) Low meltig points
  (B) Good conductivity in solid state
  (C) High vapor pressure
  (D) Solubility in vapor solvents.
  
  
• When 6d orbital is complete, the entering electron goes into
  
  (A) 7f
  (B) 7s
  (C) 7p
  (D) 7d
  
  
• Bohr model of atom is contracted by
  
  (A) Planck’s quantum theory
  (B) Dual nature of matter
  (C) Heisenberg’s uncertainty principle
  (D) All of the above
  
  
• The bond order of N₂ molecule is What are the main ions in the filtrate?
  
  (A) 1
  (B) 2
  (C) 3
  (D) 4
  
  
• The tendency of an atom to attract a shared pair of electron towards itself is called its
  
  (A) Ionization Energy
  (B) Electron Affinity
  (C) Elecrtomegnativity
  (D) Dipole moment
  
  
• Calorie is equivalent to
  
  (A) 1484 Jq
  (B) 41.84 J
  (C) 4.184 J
  (D) 418.4 J
  
  
• Which statement about the following equilibrium is correct 2SO₂(g) + O₂(g) ↔ 2SO₃(g) D H = – 188.3 kJ mol^-1
  
  (A) the value of Kp falls with a rise in temp
  (B) the value of Kp falls with increasing pressure
  (C) adding V2O5 catalyst increase the equilibrium yield of sulphur trioxide
  (D) the value of Kp is equal to Kc
  
  
• The solubility product of AgCl is 2.0 x 10^-10 mole² dm^-6. The max concentration of Ag+ ions in the solution is
  
  (A) 2.0 x 10^–10 mol dm^–3
  (B) 1.41 x 10^–5 mol dm^–3
  (C) 1.0 x 10^–10 mol dm^–3
  (D) 4.0 x 10^–20 mol dm^–3
  
  
• Molarity of pure water is
  
  (A) 1
  (B) 18
  (C) 5
  (D) 6
  
  
• If a strip of Cu metal is placed in a solution of FeSO₄.
  
  (A) Cu will be precipitated out
  (B) Fe is precipitated out
  (C) Cu and Fe both dissolve
  (D) No reaction takes place
  
  
• The Oxidation number of O-atom is OF₂
  
  (A) -2
  (B) +2
  (C) -1
  (D) 1
  
  
• In zero order reaction the rate is independent of
  
  (A) temperature of reaction
  (B) concentration of reactions
  (C) concentration of products
  (D) none of these

Chemistry
(Essay Type)
Group - II
Time: 3:10 Hours
Marks: 83
Section - I

2. Answer briefly any Eight parts from the following. 2x8=16

• Calculate the moles of Oxygen atoms in 9.0 gm of mg (NO₃).
• What is Stoichiometry? Give two assumptions.
• What is molecular Ion? How it is formed.
• How the crystals are dried in a desicator?
• Define Distribution Law. How it is helpful in solvent extraction?
• Calculate value of R in SI units.
• Give any four uses of Plasma
• Explain the process of respiration obey’s Dalton’s Law of Partial Pressure.
• Metallic crystals are lustrous in nature why?
• Give two uses of liquid crystal.
• Differentiate between Isomorphism and Polymorphism.
• Define lattice energy. Give example. 

3. Answer briefly any Eight parts from the following. 2x8=16

• Why the electron moves faster in an orbit of smaller radius?
• Why the potential energy of an electron is negative in an orbit of atom?
• Why 4s subshell is filled first and 3d afterward?
• Give the electronic configuration of an element atomic number 24.
• Why the one pair of electrons occupies more space over the central atom than bond pair?
• Why molecular orbital theory is superior to that of VSEPR and VB theory?
• Why He₂ molecule does not exist under normal conditions?
• Define dipole moment and give its mathematical expression
• Define enthalpy of neutralization with an example
• Differentiate system and surroundings.
• Why HCl is added before passing H₂S gas in qualitative analysis of 2^nd group basic radicals?
• Define pH with mathematical expression

 4. Answer briefly any Six parts from the following. 2x6=12

• How does a catalyst affect a reversible reaction?
• How will you prepare 5% W/V urea solution in water?
• What is critical solution temperature? Give one example
• NaCl and KNO₃ are used to lower the melting point of ice. Justify it.
• What are the electro chemical series?
• Describe relax reactions which occur during discharging of lead accumulator battery.
• Calculate the oxidation number of Mn in KMnO₄ and MnO₂
• Differentiate between average and instantancous rate of reaction Describe two characteristics of a catalyst.