Bahawalpur 2014
Chemistry
Inter Part-I
(Objective)
Note: Write answers to the questions on the answer sheet provided. four possible answers A, B, C and D to each questions are given which answer is correct, fill the relevant circle with pen ink to each question on the answer sheet provided:

Question#1

• The mass of one mole of Electrons:
  
  a) 1.008 mg
  b) 0.55 mg
  c) 0.184 mg
  d) 1.673 mg
  
  
• The comparative rate at which the solutes move in paper chromatography depend on:
  
  a) The size of paper
  b) Rf values of solutes
  c) Temperature of the experiment
  d) the size of chromatography tank used
  
  
• Solvent Extraction is an equilibrium process and it is controlled by:
  
  a) Law mass action
  b) The amount of solvent used
  c) Distribution law
  d) The amount of solute
  
  
• 27g of Al will react with how much mass of O₂ to produce AI₂O₃:
  
  a) 8 g of oxygen
  b) 16 g of oxygen
  c) 32 g of oxygen
  d) 24 g of oxygen
  
  
• Pressure remaining constant, at which temperature the volume of gas becomes twice of that it is at O°C:
  
  a) 546°C
  b) 200°C
  c) 546K
  d) 273K
  
  
• When water freeze its volume increases:
  
  a) 10%
  b) 9%
  c) 15%
  d) 18%
  
  
• Acetone and chloroform are soluble each other due to:
  
  a) Intermolecular hydrogen bonding
  b) Ion dipole interaction
  b) Instantaneous Dipole
  d) All these
  
  
• Number of molecules in one dm³ of water is close to
  
  a) 6.02/22.4 *10²³
  b) 12.04/22.4*10²³
  c)18/22.4*10²³
  d) 55.6*6.02*10²³
  
  
• Splitting of spectral lines when atoms are subjected to strong electric field is called:
  
  a) Zeeman effect
  b) Stark effect
  c) Photoelectric effect
  d) Compton Effect
  
  
• The bond angle in NH₃ Molecule is:
  
  a) 109.5 °
  b) 107.5°
  c) 104.5°
  d) 108°
  
  
• Which of the following molecule has zero dipole moment:
  
  a) NH₃
  b) CHCI₃
  c) H₂O
  d) BF₃
  
  
• Quantum number values for 2p orbitals are:
  
  a) n=2, l=1
  b) n=1, l=2
  c) n=1, l=0
  d) n=2, l=0
  
  
• One calorie is equivalent to:
  
  a) 0.4184 j
  b) 41.84j
  c) 4.184 j
  d) 418.4 j
  
  
• Stronger the oxidization agent, greater is the:
  
  a) Oxidation potential
  b) Reduction potential
  c) Redox potential
  d) E.M.F of cell
  
  
• In zero order reaction, the rate is independent of:
  
  a) Temperature of reaction
  b) concentration reactants 
  c) Concentration of products
  d) None of these
  
  
• The ph of 10^-3 moles dm^-3 of an aqueous solution of H₂SO₄ is:
  
  a) 3.0
  b) 2.7
  c) 2.0
  d) 1.5
  
  
• Molarity of pure water is:
  
  a) 1
  b) 18
  c) 55.5
  d) 6 

Subjective type
Note: It is compulsory to attempt 8 parts each from Q.no.2 and Q.No.3 while attempt 6 parts from Q.no.4 and attempt any 3 questions from part II. Write same q.no and its part no as given in the question paper:

Question#2

• Many chemical reactions taking place in our surroundings involve the limiting reactants. Explain with example.
• N₂ and CO have the same number of electrons, protons and neutrons. Explain
• Why actual yield is less than theoretical yield?
• Define distribution law.
• Differentiate between diffusion and effusion.
• Explain Evaporation causes cooling?
•  Differentiate between Partition and adsorption chromatography.
• Derive an expression to find out the partial pressure of a gas?
• Vacuum Distillation can be used to avoid decomposition of sensitive liquid.
• Cleavage of crystals is itself anisotropic behavior explain.

Question#3

• Give two properties of neutrons.
• What is the Mosley’s law? Also give is impotence.
• Define Hun’s Rule with one example .
• Prove ∆E= q_v
• How Davission and Gerner proved dual nature of matter?
• Define Ionization energy. Also discuss it along the period with periodic table.
• Why σ bond is more stronger than π bond?
• The dipole moment of CO2 is zero but that of SO2 is not zero. Why?
• π- bonds are more diffused than σ bond why?
• define with example: i- System ii- State function
• What is ph and POH? How are they related with PKw?
• Define Buffer solution and solubility.

Question#4

• What is the effect of change in pressure on 2SO₂ +O₂(irreversible sign) 2SO₃ Reaction.
• Why hydration energy of Na⁺ ion is les than li⁺ ion?
• One model solution of urea is more dilute than one molar solution why?
• SHE acts as an anode when connected with copper electrode but as cathode with zinc electrode why?
• Rate of reaction decreases with the passage of time. explain
• What is the meant by poisoning of a catalyst?
• Calculate the oxidation number of Mn in KMnO₄.
• What is colligative properties?
• Give two functions of Salt Bridge.

Part -II

Question#5

(a) Write down the combustion analysis for the determination of Empirical formula of a compound.
(b) Define liquid Crystals and write their uses.

Question#6
(a) Define Hybridization of Atomic Orbitals. Discuss Sp³ Hybridization in detail . draw the structure of Methane.
(b) What is the first law of Thermodynamics? Prove that ∆ E=q_p

Question#7
(a) Calculate mass of 1 dm₃ of NH₃ gas at 30° C and 1000mm Hg Pressure considering that NH₃ is behaving ideally.
(b) Calculate the radius of Bohr’s atom using Bohr’s atomic Model.

Question#8
(a) What is galvanic cell? Give its construction.
(b) The following reactions was allowed to reach the state of equilibrium
2A(aq) + B(aq) irreversible sign C(aq)
The initial amounts of the reactants in one dm3 of solution were 0.50 mole of A and 0.60 mole of B. At equilibrium, the amounts were 0.20 moles of A and 0.45 mole of B and 0.15 mole of (c) Calculate the equilibrium constant Kc.

Question#9
(a) Describe one method to record the depression of freezing point of solution.
(b) Describe how the rate of a reaction can be measured by a chemical method?

Part –III
Write down the standard solution, chemical equation with mole ratio, indicator with end point, procedure and supposed readings with calculation for A,B&C.
Write down the material required, diagram and procedure for part D and E.

Question#10

(A) The given solution contains 8.4g per dm³ of MHCO₃. Find out the Atomic weight of M. (Molecular mass of MHCO₃= M+61)
(B) The given solution contains 40g mixture of Fe₃SO₄.7H₂O and (NH₄)₂SO₄ dissolved per dm³. Find out the percentage composition of the mixture (Molecular mass of FeSO₄.7H₂O=246)
(C) The given solution contains 30g Na₂S₂O₃.₅H₂O dissolved per dm3. Find out the percentage purity of the sample (Molecular mass of Na₂S₂O₃.₅H₂O =246 )
(D) Separate the mixture of inks by the paper chromatography. Also calculate its R_f value.
(E) Purify the given sample of impure benzoic acid by Cyrstallization.