Inter (Part-I) Gujranwala Board 2012
Chemistry Paper: I
Time : 20 Minutes Marks: 17
OBJECTIVE
Note: you have four choices for each objective type question as A, B, C, and D. The choice which you think is correct, fill that circle in front of that question number with market or pen on the answer book provided. Cutting or filling two or more circles will result in zero mark in that question. Attempt as many question as given in objective type question paper and leave other blank. Write the letter A, B, C, and D in the column (write correct option) against each question. If there is a contradiction in the bubble and hand written answer , bubble option will be considered correct.

• The number of moles of CO₂ which contains 16 gm of oxygen is:
  
  (A) 0.25
  (B) 0.50
  (C) 1.0
  (D) 1.50
  
  
• The mass of one mole of electron is:
  
  (A) 1.008mg
  (B) 0.55 mg
  (C) 1.84 gm
  (D) 1.673 mg
  
  
• The comparative rates at which the solutes move in paper chromatography depend on :
  
  (A) the size of the paper
  (B) Rf values of solutes
  (C) temperature of the experiment
  (D) size of the chromatographic tank used

•  Number of molecules in one dm3 of water is close to :
  
  (A) 6.02 x 10²³  
  (B) 12.04 x 10²³
  C) (18 /22.4) x 10²³
  (D) 55.6 x 6.02 x 10²³ 
  
  
• Equal masses of methane and oxygen are mixed in an empty container at 25o C. The fraction of total pressure exerted by oxygen is:
  
  (A) 1/3
  (B) 8/9
  (C) 1/9
  (D) 16/17
  
  
• When water freezes at 0o its density decreases due to :
  
  (A) cubic structure of ice
  (B) change of bond length
  (C) empty spaces present in the structure of ice
  (D) change of bond angle
  
  
• Ionic solids are characterized by:
  
  (A) low melting points
  (B) good conductivity in solid state
  (C) have perfect arrangement of atoms
  (D) can possess small regions of orderly arrangement of atoms
  
  
• The wave number o light emitted by a certain source is 2 x 107 m the wavelength of this light will be.
  (A) 500 nm
  (B) 500 m
  (C) 200 nm
  (D) 5x10⁷ m
  
  
• When 6d orbital is complete, the entering electron goes into:
  (A) 7f
  (B) 7s
  (C) 7p
  (D) 7d
  
  
• Which of the hydrogen halides has the highest percentage of ionic character?
  (A) HCℓ
  (B) HF
  (C) HBr
  (D) HI
  
  
• Octet rule is not followed in the formation of :
  
  (A) NF₃
  (B) CF₄
  (C) CCℓ₄
  (D) PCℓ₅
  
  
• If an endothermic reaction is allowed to take place very rapidly in the air the temperature of the surrounding air.
  
  (A) remains constant
  (B) increases
  (C) decreases
  (D) remains unchanged
  
  
• An excess of aqueous sliver nitrate is added to aqueous barium chloride and precipitate is removed by filtration. What are the main ions in the filtrate:
  
  (A) Ag⁺ and NO₃ only
  (B) Ag⁺ and Ba₂+ and NO_3-
  (C) Ba₂+ and NO₃ only
  (D) Ba₂⁺ and NO₃ and CI^-
  
  
• 18 gm glucose is dissolved in 90 gm of water. The relative lowering of vapour pressure is equal:
  
  (A) 1/5
  (B) 5.1
  (C) 1/51
  (D) 6
   
• The eathodic reaction in the electrolysis of dil. H₂SO₄ with Pt electrode is:
  
  (A) reduction
  (B) oxidation
  (C) both oxidation and reduction
  (D) neither oxidation nor reduction
  
  
• Galvanic cells which cannot be recharged are called:
  
  (A) diffused cells
  (B) secondary cells
  (C) tertiary cells
  (D) primary cells
  
  
• The unit of rate constant is the same as that of the rate of reaction in”
  
  (A) first order reaction
  (B) second order reaction
  (C) zero order reaction
  (D) third order reaction

Inter (Part-I)
Gujranwala Board 2012
Chemistry Paper: I
Time : 2:40 Hours
Marks: 68

SUBJECTIVE

2. Write short answers to any EIGHT question: (2x8=16)

• Why the actual yield is always less than the theoretical yield:
• 180g of gucose and 342 g of sucrose have the same number of molecules but different number of atoms present in them Explain.
• N₂ and CO have the same number of electrons, porotons, and neutrons, Give reason.
• What is partition law:
• Give the main characteristics of the solvent used for crystallization.
• What is JouleThomson Effect: Write application.
• Write four application of plasma.
• Explain two applications of Dalton’s law of partial pressure.
• Differentiate between critical temperature and critical pressure.
• Cleavage of the crystal is itself anisotropic behavior.
• Earthenware vessels keep water cool. Why?
• Explain why heat of sublimation of iodine is very high.

3. Write short answers to any EIGHT question :

• Why is it necessary to decrease the pressure in discharge tube to get cathode rays?
• e/m value of cathode ray is just equal to that of electrons Justify.
• The positive rays are also called canal rays. Explain.
• π bonds are more diffused than o bonds. Give reason.
• Bond distance is the compromise distance between two atoms. Give reason.
• Differentiate between spontaneous and non-spontaneous reactions.
• Spontaneous reactions always proceed in the forward direction. Give reason
• Why is exothermic reactions, heat is released from the system:
• Freezing points are depressed due to presence of solutes. Justify
• Relative lowering of vapour pressure is independent of the temperature. Explain.
• A salt bridge maintain electrical neutrality in the cell. Give reason.
• The radioactive decay is always a first order reaction.

4. Write short answers to any SIX questions.

• Write the order of repulsion between electron pairs according to VSEPR- Theory.
• Deviation in bond angle in water (H₂O) molecule is more than in ammonia (NH₃) molecule although both have tetrahedral structure .
  What will be nature of solution when:
• pH is more than 7 (b) pH is smaller than 7:
• Give two application of common ion effect.
• What are Kc and Kp and how these are related:
• Why we need Buffer solution ?
• Write two application of electro-chemical series.
• What are redox reactions? Give example .Write rate equation for the following reactions.
• Write rate equation for the following reactions.
  (a) NO + O₃ NO₂ + O₂
  (b) CHCℓ₃ + Cℓ₂CCℓ₄+ HCℓ

(Section – II)

5.  a) What is mass spectrometer? How is it used to determine the relative atomic masses of isotopes? 4
     b) How does hydrogen bonding explain the formation of ice and its lesser density than liquid water? 4
6.  a) Define covalent bond. Discuss its type with suitable example. 4
     b) Neutralization of 100 cm3 of 0.5 M NaOH at 25oC with 100 cm3 of 0.5 M HCℓ at 25oC raised the temperature of reaction mixture to 28.5o C. Find the enthalpy of neutralization. Specific heat of water =4.2 JK⁺¹ g^-1. 4
7.   a) Describe Millikan’s oil drop method for determination of charge of electron.
      b) One mole of methane is maintained at 300 K. its volume is 250 cm3. Calculate the pressure exerted by the gas when it is considered as an ideal gas. 4
8.   a) Define common ion effect. Give its two application 4
      b) Describe the construction and working of standard hydrogen electrode (SHE). 4
9.   a) How can you measure elevation of boiling point Landsberger’s method? 4
      b) Write note on catalysis. Give its types. 4

Inter (Part-I) Gujranwala Board 2013
Chemistry Paper: I
Time : 20 Minutes Marks: 17

OBJECTIVE

Note: you have four choices for each objective type question as A, B, C, and D. The choice which is correct, fill that circle in front of that question number with market or pen on the answer book provided. Cutting or filling two or more circles will result in zero mark in that question. Attempt as many question as given in objective type question paper and leave other blank.

• The mass of one mole of electron is:

            (A) 1.008 mg
            (B) 0.55 mg
            (C) 0.184 mg
            (D) 1.673 mg

• One mole of SO₂ consists of :

             (A) 6.02 x 1023 atoms of oxygen
             (B) 18.1 x 1023 molecules of SO₂
             (C) 6.02 x 1023 atoms of sulphur
             (D) 4 gram atoms of SO₂

• Solvent extraction method is particularly useful technique for separation when the product to be separated:
  (A) non –volatile or thermally unstable
  (B) volatile or thermally stable
  (C) non-volatile or thermally stable
  (D) volatile or thermally unstable
  
  
• Pressure remaining constant at which temperature the volume of a gas will become twice of what it is at 0C^o?
  
  (A) 546C^o
  (B) 200C^o
  (C) 546 K
  (D) 273 K
  
  
• When water freezes at 0C^o, its density decreases due to?
  
  (A) empty spaces present in the structure of ice
  (B) cubic structure of ice
  (C) change of bond lengths
  (D) change of bond angles
  
  
• Diamond is a bad conductor of electricity because:
  
  (A) it has a tight structure
  (B) it has a high density
  (C) there is no free electron present in the crystal of diamond to conduct electricity
  (D) it is transparent to light
  
  
• Splitting electric field is called L
  
  (A) Zeeman effect
  (B) Stark effect
  (C) Photoelectric effect
  (D) Compton effect
  
  
• In ground state of an atom the electron, is present:
  
  (A) in the nucleus
  (B) in the second shell
  (C) nearest to the nucleus
  (D) farthest from the nucleus
  
  
• Which molecule has zero dipole moment?
  
  (A) NH₃
  (B) CHCℓ₃
  (C) H₂O
  (D) BF₃
  
  
• Which species has unpaired electrons in antibonding molecular
  
  (A) Oֻ ₂⁺
  (B) Oֻ ₂⁺
  (C) B₂
  (D) F₂
  
  
• The change in heat energy of a chemical reaction at constant temperature and pressure is called?
  
  (A) enthalpy change
  (B) heat of sublimation
  (C) bond energy
  (D) internal energy change
  
  
• An excess of aqueous sliver nitrate is added to aqueous barium chloride and precipitate is removed by filtration. What are the main ions in the filtrate?
  (A) Ag+ and Ba₂+ and NO₃-
  (B) Ag+ and NO₃- only
  (C) Ba₂+ and NO₃- only
  (D) Ba₂+ and NO₃- and Cℓ-
  
  
• For which system does the equilibrium constant Kc has unit of (concentration)-1
  
  (A) N₂ + 3H₂2NH₃
  (B) H₂ + 12  2H1
  (C) 2NO₂ N₂O₄
  (D) 2HF  H₂ + F₂
  
  
• 18 g glucose is dissolved in 90 g of water . the relative lowering of vapour pressure is equal to: 

               (A)
               (B) 5.1
               (C)
               (D) 6

• Stronger the oxidizing agent, greater is the:
  
  (A) oxidation potential
  (B) reduction potential
  (C) redox potential
  (D) E.M.F of cell

• If a strip of Cu metal is placed in a solution of FeSo₄:
  
  (A) Cu will be deposited
  (B) Fe is precipitated out
  (C) Cu and Fe both dissolve
  (D) no reaction occurs
  
  
• The unit of the rate constant is the same as that of the rate of reaction in :
  
  (A) first order reaction
  (B) second order reaction
  (C) zero order reaction
  (D) third order reaction

Inter (Part-I) Gujranwala Board 2013
Chemistry Paper: I
Time : 3:10 Hours   Marks: 83
SUBJECTIVE

2. Write short answers to any EIGHT question: (2x8=16)

• N₂ and CO have same number of electrons, protons and neutrons. Justify.
• Define the term molecule Give two examples also.
• No individual neon atom in the sample of the element has a mass of 20.18 amu. Explain with reason.
• Explain sublimation. Give two example.
• What do you know about Rf value of a component in paper chromatography?
• Derive the units for gas constant R in general gas equation when pressure is in Nm-2 and volume in m3.
• Water vapurs do not behave ideally at 273 K. Explain
• State Boyle’s law of gases.
• One feels sense of cooling under the fan after bath.
• Heat of sublimation of iodine is very high although it is a molecular solid. Give reason.
• Diamond is hard and an electrical insulator. Give reason.
• Ionic crystals are highly brittle . Explain with reason.

3. Write short answers to any EIGHT question. (2x8=16)

• The radius of first orbit of hydrogen atom is 0.529 Ao Caculate the radius of 3rd orbit of hydrogen atom.
• Whichever gas is used in the discharge tube, the nature of the cathode rays remains the same. Why?
• What are the defects in Rutherford’s atomic model?
• Write the electronic configuration of Cr for which atomic number is 24.
• Sketch the molecular orbital picture of O2 .
  Separate the following molecules as polar or non-polar.
       a)CO₂
       b) CH₃OH
       c) CCℓ₄
       d) HF
• Define bond energy with two parameters which determine its strength .
• Why ionization energy decreases down the group although the nuclear charge increase?
• What is state and state function? Explain with example.
• State enthalpy of combustion with example.
• Why during the synthesis of NH₃ temperature is kept low?
• Define solubility product with example.

4. Write short answers to any SIX questions: 2x6=12)

• What will be the effect of increase of pressure and temperature o the following reaction?
  N₂ (g) + 3H₂(g) ⇋ 2NH₃(g) ⇋ H = -92.46 KJ
• Define molal boiling constant with an example.
• Why ethylene glycol is added in radiator of automobile?
• Why aqueous solution of sodium acetate is alkaline in nature
• How electrochemical series help us in determining the chemical reactivity of metals?
• Balance the following equation by Redox method?
  ← HNO₃ + HI NO + 1₃ + H₂ O
• Write electrode reaction of electrolysis of fused sodium chloride.
• Define autocatalysis with an example.
• How surface area affects the rate of a chemical reaction?

(Section –II)

5.  a) What are liquid crystals? Give three use in daily life. 4
     b) A well-Known ideal gas is enclosed in a container having volume 500 cm³ at S.T.P. Its mass comes out to be 0.72 g. What is the molar mass of this gas? 4
6.  a) What is hybridization? Discuss sp₂ hybridization with example. 4
     b) Define enthalpy of neutralization also discuss glass calorimeter pressure. 4
7.  a) Write down four applications of Dalton’s law of partial pressure. 4
     b) Derive an expression for the radius of nth Bohr’s orbit of H. Atom. 4
8.  a) What is electrochemical series? Give its applications. 4
     b) What is solubility product? The solubility of CaF2 in water at 25o C is found t be 2.05 x 10-4 mol dm -3. What is the value of Ksp at this temperature? 4
         (Atomic Mass of Ca =40, F = 19)
9.  a) What are azeotropic mixture ? Explain them with the help of graphs. 4
     b) Write a detailed note on activation energy. Explain with graphs. 4

(Section-II)
(Practical)

Attempt any three part. 3 x 5 = 5

(ii) Write down standard solution, chemical equation with mole ratio, indicator with end point procedure and calculation wit supposed readings for part a, b, and c. (1+1+1+1+1)
(iii.) Write down material required, diagram and procedure for part d and e.

10. a) 4.9 g of a dibasic acid has been dissolved per dm .Determine the molecular weight of the acid.
      b) The given solution contains 5.0 g of impure KMnO₄ dissolved per dm³. Determine the percentage purity of sample. (Molecular mass of KMnO₄ = 158)
      c) 12.4 g of Na₂ S₂O₃. x H₂O has been dissolved per 500