Inter (Part-I) Multan Board 2015
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 molal boiling point constant is the ratio of the elevation in boiling point to:-

  (A) Molarity
  (B) Molality
  (C) Mole fraction of solvent
  (D) Mole fraction of solute

• Stronger the oxidizing agent, greater is the:-

  (A) Oxidation potential
  (B) Reduction potential
  (C) Redox potential
  (D) E.M.F. of cell

• If the rate equation of a reaction 2A+B→product is, rate = K[A]² [B ] and A is present in large excess, then order of reaction is:-

(A) 1
(B) 2
(C) 3
(D) 4

• The mass of one mole of electron is:-

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

• The largest number of molecules are present in:-

  (A) 6 g of H₂O
  (B) 4.8 g of C₂H₅OH
  (C) 2.8 g of CO
  (D) 5.4 g of N_{2 5}O

• The comparative rates at which the solutes move in paper chromatography depend on:-

  (A) The size of paper
  (B) Rf value of solutes
  (C) Temperature
  (D) Size of chromatographic tank

• The molar volume of CO₂ is maximum at:-

  (A) STP
  (B) 127^oC and 1atm
  (C) 0^oC and 2atm
  (D) 273^oC and 2atm

• The deviation of a gas from ideal behavior is maximum at:-

(A) −10^OC and 5.0 atm
(B) −10^OC and 2.0 atm
(C) 100^OC and 2.0 atm
(D) 0^OC and 2.0 atm

• NH₃ shows a maximum boiling point among the hydrides of Vth group elements due to:-

  (A) Very small size of Nitrogen
  (B) Lone pair of electrons present on Nitrogen 
  (C) Pyramidal Structure of NH₃
  (D) Enhanced electronegative character of Nitrogen 

• Ionic solids are characterized by:-

(A) Low melting point
(B) High vapour pressure
(C) Good conductivity in solid state
(D) Solubility in polar solvents 

• In ground state of an atom, the electron is present:-

  (A) In the nucleus
  (B) In the second shell
  (C) Nearest to nucleus
  (D) Farthest from the nucleus

• Orbitals having same energy are called:-

  (A) Hybrid orbitals
  (B) Valence orbitals
  (C) Degenerate orbitals
  (D) d–orbitals

• ____ molecule has zero dipole moment.

(A) NH₃
(B) CHCl3
(C) H₂O
(D) BF₃

• ____ is the Hydrogen halide which has the highest percentage of Ionic character.

  (A) HCl
  (B) HBr
  (C) HF
  (D) HI

• 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 

• Which statement about the following equilibrium is correct:- 2SO₂ + O₂ 2SO₃∆H =−183KJ mol⁻¹

(A) The value of Kp falls with rise in temperature
(B) The value of Kp falls with increasing pressure 
(C) Adding V_{2 5}O catalyst increase the yield of SO₃
(D) The value of Kp is equal to Kc

• The pH of 10⁻³ moledm⁻³ of an aqueous solution of H₂SO₄ is:-

(A) 3.0
(B) 2.7
(C) 2.0
(D) 1.5

Inter (Part-I) Multan Board 2015
Chemis
Part I (Subjective)
Time Allowed: 2.10 Hours 
Max. Marks: 83 

Section I

2. Attempt any eight parts. 8 × 2 = 16

• No individual neon atom in the sample of element has a mass of 20.18 amu.
• How many Oxygen atoms are present in 4.8g of Ozone (O = 16 amu) (iii) What is the function of Ionization Chamber in Mass Spectrometer?
• What is the difference between Adsorption and Partition Chromatography?
• Give two uses of Chromatography.
• What are the causes for deviation of gases from Ideality?
• Give two applications of Plasma.
• What are Spontaneous and Non-spontaneous processes? Give one example of each case.
• State the Hess’s Law of Constant Heat Summation.
• What is the effect of increase of temperature on the yield of the product for the reaction SO2(g ) + O2( g ) SO3( g ) + Heat
• What is Buffer Solution? Give an example.
• How does a buffer act? Explain with an example. 

3. Attempt any eight parts. 8 × 2 = 16

• Why the values of boiling points of noble gases increase from top to bottom within a group?
• Why the temperature of a boiling liquid does not rise even if heat is continuously supplied to it?
• Ionic solids do not conduct electricity in the solid state but become good conductors in the solution or molten state. Justify it. 
• Explain the term unit cells dimensions.
• Whichever gas is used in the discharge tube, the nature of cathode rays remains same? Why?
• Distribute electrons in the orbitals of 29Cu and 24Cr .
• How do you come to know that the velocities of electrons in higher orbits, are less than those in lower orbits of Hydrogen atom?
• State Hund’s rule and Pauli’s exclusion principle.
• The size of Chlorine atom is smaller than Cl⁻¹ Justify it. 
• Define Electron Affinity and give an example.
• Represent the molecular orbitals of N₂ molecule in the increasing order of energy.
• Why NH₃ molecule and NH₄⁺ ion have different structures?

3. Attempt any six parts. 6 × 2 = 12

• Define Molarity of a solution. How is Molarity related to mass of solute? 
• What is critical solution temperature? Give an example.
• Why the Beckmann’s thermometer is used to note the depression of freezing point?
• What is Oxidation Number? Determine the Oxidation Number of Phosphorus in H₃PO₄.
• How is Anodized Aluminium prepared? Give the advantages of Anodization of Al.
• What is a Salt Bridge? How it maintains electrical neutrality in the half cell solutions? 
• The order of a reaction may be in fractions. Justify with the help of an example.
• Name two physical methods used to determine the rate of a reaction.
• A catalyst is specific in its action.

SECTION-II

NOTE: - Attempt any three questions of the following:-

Question #5
(a) Define Ionic Solids. Discuss the properties of Ionic Solids. (4)
(b) Silicon Carbide (SiC) is an important ceramic material. It is produced by allowing sand (SiO₂ ) to react with Carbon at high temperature. SiO₂ + 3C → SiC+ 2CO When 100 kg sand is reacted with excess of Carbon, 51.4kg of SiC is produced. What is the percentage yield of SiC? (4)

Question #6
(a) What is Dalton’s law of Partial Pressure? Also discuss its applications. (4)
(b) Explain Rutherford’s Model of Atom. (4)

Question #7
(a) Explain bonding in O₂ according to Molecular Orbital Theory. Also describe its paramagnetic property. (4)
(b) Define Enthalpy. Prove ∆H = qp (4)

Question #8
(a) The solubility of CaF₂ in water at 25^oC is found to be 2.05 × 10⁻⁴ moldm⁻³. What is the value of K_sp at this temperature? (4)
(b) What is Catalysis? Differentiate between Homogeneous and Heterogeneous Catalysis  with one example in each. (4)

Question #9
(a) Write a comprehensive note on Raoult’s law. (4)
(b) Discuss the Working and Chemistry of Alkaline Battery and Fuel Cells. (4)

SECTION-III (PRACTICAL PART)

Question #10
NOTE:- (i) Attempt any three parts. ( 3 x 5 = 15)

Write down material required, diagram and procedure for part A & B. ( 1 + 1 + 3) = (5)
Write down standard solution, chemical equation with mole ratio, indicator with end point, procedure and supposed reading with calculation for part C, D & E. ( 1 + 1 + 1 + 1 + 1 ) = (5)

• Separate the mixture of three inks by Chromatography.
• Purify commercial sample of Sodium Chloride by common Ion effect.
• 15.0 grams of Na₂CO₃ is dissolved per dm³ of solution. Determine percentage purity of sample volumetrically. (Molecular mass of Na₂CO₃ = 106 )
• 10.0 g of KMnO₄and K₂SO₄ dissolved per dm³ of solution. Find percentage purity of the sample volumetrically. (Molecular mass of KMnO₄ = 158)
• 14.0 grams of I₂ (iodine) dissolved per dm³ . Find out the percentage purity of the sample volumetrically. (Molecular mass of I₂= 254)