Inter (Part-I) Sahiwal Board 2016
Chemistry
Part I (Objective Type)
Time Allowed: 20 Minutes 
Max. Marks: 17

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. Use marker or pen to fill the circles. Cutting or filling two or more circles will result in zero mark in that question.

Question #1
Circle the correct option i.e. A/B/C/D. Each part carries one mark.

• The unit of rate constant is the same as that of the rate of reaction in:

(a) Ist order reaction
(b) 2nd order reaction
(c) Zero order reaction
(d) 3rd order reaction

• Stronger the oxidizing agent, greater is the:

(a) Oxidation potential
(b) Reduction potential
(c) Redox potential
(d) E.M.F of cell

• Molarity of pure water is:

(a) 1
(b) 18
(c) 55.5
(d) 6

• Which statement about the following equilibrium is correct? 2SO₂(4+ O₂(g) 2SO₃ (g) OH = —188.3141mor^-1

(a) The value of K _p falls with a rise in temperature
(b) The value of K _p falls with increasing pressure
(c) Adding V₂O₅ catalyst increases the equilibrium yield of sulphur trioxide.
(d) The value of K_p is equal to K_c .

• The pH of 10^-3 mol dm^-3 of an aqueous solution of H₂SO₄ is:

  (a) 3.0
  (b) 2.7
  (c) 2.0
  (d) 1.5

• Calorie is equivalent ot:

(a) 0.4184 J
(b) 41.84 J
(c) 4.184 J
(d) 418.4 J

• Which of the following molecules has zero dipole moment?

(a) NH₃
(b) CHC1₃
(c) H₂O
(d) BF₃

• The number of bonds in nitrogen molecule is:

(a) One sigma and one pi bond
(b) One sigma and two pi bonds
(c) Three sigma bonds
(d) Two sigma and one pi bond

• When 6d orbital is complete, the entering electron goes into:

(a) 7f
(b) 7s
(c) 7p
(d) 7d

• The wave number of the light emitted by a certain is 2 x10⁶m^-1. The wavelength of this light will be:

(a) 500 nm
(b) 500 m
(c) 200 nm
(d) 5 x 107m

• Which of the following is a pseudo solid?

(a) CaF₂
(b) Glass
(c) NaCl
(d) KC1

• Acetone and chloroform are soluble in each other due to:

(a) Intermolecular hydrogen bonding
(b) Ion-dipole interaction
(c) Instantaneous dipole
(d) Coordinate covalent bonding

• The molar volume of CO, is maximum at:

(a) STP
(b) 127°C and 1 atm
(c) 0°C and 2 atm
(d) 273°C and 2 atm

• Pressure remaining constant, at which temperature the volume of a gas will become twice of what it is at 0°C.

(a) 546°C
(b) 200°C
(c) 546 K
(d) 273 K

• Solvent extraction method is controlled by:

(a) Law of mass action
(b) The amount of solvent used
(c) Distribution law
(d) The amount of solute used

• The largest number of molecules is present in:

(a) 3.6g of H₂O
(b) 4.8 g of C₂H₅OH
(c) 2.8g of CO
(d) 5.4g of N₂O₅

• The mass of one mole of electron is:

(a) 1.008 mg
(b) 0.55 mg
(c) 0.184 mg
(d) 1.673 mg

Inter (Part-I) Sahiwal Board 2016
Chemistry
Part I (Subjective)
Time Allowed: 3.10 Hours 
Max. Marks: 83

Section I

2. Attempt any EIGHT short questions.

• Define Molecular Ion. How is it generated?
• Define Molecular Formula. Give an example.
• Define Isotope. Give an example.
• Differentiate between adsorption and partition chromatography.
• State distribution law.
• Convert 100°f into °C.
• Write two applications of plasma.
• Why gases show non-ideal behavior at night pressure?
• Define hydrolysis. Give two examples.
• State ebullioscopic and cryoscopic constants.
• Define pK_a and pK_b.
• Define solubility product. Give one example.

3. Attempt any EIGHT short questions. (8 x 2 = 16)

• How evaporation is a continuous process?
• How electrical conductivity of metals decreases by increasing temperature?
• Why amorphous solids like glass are also called super cooled liquids?
• Why are ionic crystals highly brittle?
• Why is it necessary to decrease the pressure in the discharge tube to get the cathode rays?
• Why e/m values of positive rays of different gasses are different but those for cathode rays the e/m values are the same?
• What is azimuthal quantum number? Give its significance.
• How are X-rays produced?
• What do you mean by mole fraction of solution?
• Why a porous plate or a salt bridge is not required in leas strong cell?
• Why standard oxidation potential of Zn is 0.76 and its reduction. Potential is -0.76 V?
• Why Na and K can displace hydrogen from acids but Pt, Pd and Cu can not?

4. Attempt any SIX short questions. (6 x 2 = 12)

• State coordinate covalent bond. Give an example.
• Write two points of Valence Bond Theory.
• Lone pairs of electrons on an atom occupy more space. Explain.
• The atomic radius is greater than cationic. Explain.
• Describe state function with an example.
• Define lattice energy with an example.
• What is specific rate constant?
• Differentiate between homogeneous and heterogeneous catalysis.
• Under what conditions activated complex is formed.

SECTION- II

 Attempt any THREE questions:

Question #5
(a) A well known ideal gas is enclosed in container having volume 500cm³ at S.T.P. Its mass comes out to be 0.72g. What is the molar mass of this gas?
(b) Define the followings with examples. (i) Amorphous solids (ii) Habit of a crystal (iii) Allotropy (iv) Transition temperature

Question #6
(a) What is Joule Thomson Effect? How Linde's method is used for liquefaction of gases?
(b) Write the postulates of Bohr's Model of Atom.

Question #7
(a) Explain dipole moment. How is it used to explain the geometry of molecules?
(b) How enthalpy of combustion is determined using bomb calorimeter?

Question #8
(a) How will you determine the order of reaction by Half Life Method?
(b) The solubility of PbF₂ at 25°C is 0.64gdm^-3 . Calculate K _sp, of PbF₂ . Molecular mass of PbF₂ = 245.2g mol^-1 .

Question #9
(a) Define the following terms: (i) Mole Fraction (ii) Molarity (iii) Parts Per Million (iv) Hydration
(b) What is Standard Hydrogen Electrode (SHE)? How is it used to measure the electrode potential of Zinc?