Inter (Part-I) Sargodha 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.

• Isotopes differ in

(A) Properties which
(B) Arrangement of
(C) Chemical
(D) The extent to which

• The volume occupied by 1.4 g of N₂ at S.T.P is

(A) 2.24 dm³
(B) 22.4 dm³
(C) I.12dm³
(D) 112cm³

• Solvent extraction is an equilibrium process and it is controlled by

(A) Law of mass action
(B) The amount of solvent used
(C) Distribution law
(D) The amount of A solute

• Pressure remaining constant, at which temperature the volume of a gas will become twice of what it is at 0⁰C

(A) 546⁰C
(B) 200⁰C
(C) 546 K
(D) 273 K

• Equal masses of methane and oxygen are mixed in an empty container at 25⁰C . The fraction of total pressure exerted by oxygen is:

(A) 1/3
(B) 9/8
(C) 1/9
(D) 16/17

• Ionic solids are characterized by:

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

• In order to maintain the boiling point of water at 110⁰C , the external pressure should be:

(A) Between 760 torr and 1200 torr
(B) Between 200 torr and 760 ton
(C) 765 torr
(D) Any value of pressure

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

(A) 500 nm
(B) 500 m
(C) 200 nm
(D) 5x10⁷m

• Orbitals having same energy are called:

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

• The number of bonds in nitrogen molecule is:

(A) One σ and One π
(B) One σ and Two π
(C) Three sigma bonds only
(D) Two σ and One π

• The value of third ionization energy of Mg is

(A) 1450 kJ mol^-1
(B) 7730 kJ mol^-1
(C) 7850 kJ mol^-1
(D) 1890 kJ mol^-1

• Calorie is equivalent to:

(A) 0.4184 J
(B) 41.84 J
(C) 4.184 J
(D) 4.814 J

• The term pH was introduced by:

(A) Henderson
(B) Sorenson
(C) Goldstein
(D) Thomson

• Molarity of pure water is:

(A) 1
(B) 18
(C) 55.5
(D) 6

• 18 g of glucose is dissolved in 90 g of water. The relative lowering of vapour pressure is equal to:

(A) 1/5
(B) 5.1
(C) 1/51
(D) 6

• The cathodic reaction in the electrolysis of dil. H₂SO₄ with Pt electrode is:

(A) Reduction
(B) Oxidation
(C) Both oxidation and reduction
(D) Neither oxidation or reduction

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

(A) 1
(B) 2
(C) 3
(D) None of these

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

Section I

2. Answer briefly any Eight parts from the followings: 8 x 2 =16

• A compound may have same empirical formula as well as the molecular formula. Justify.
• What is percentage yield? Give its significance.
• No individual neon atom in the sample of element has a mass of 20.18 a.m.u
• Give four qualifies of a solvent used in crystallization process.
• How the coloured impurities present in a solid are removed?
• H₂ and He are ideal gases at room temperature but Cl₂ and SO₂ are non ideal. Explain.
• The process of respiration obeys the Dalton's law of partial pressure. Explain. Acid-base neutralization process is always exothermic. Give reason.
• Why is it necessary to mention the physical states of reactants and products in a thermochemical equation?
• What is ionic product of water? How does this value change by change in temperature.
• What is a buffer solution? Give one example.
• A catalyst does not affect the equilibrium position and K, of a reversible reaction. Explain.

3. Answer briefly any Eight parts from the followings: 8 x 2 =16

•  What are London Dispersion forces.
•  Vacuum distillation can be used to avoid decomposition of sensitive liquid. Why?
•  Define Polymorphism and Isomorphism. Give one example of each.
•  Justify that diamond is non-conductor of electricity.
•  What particles are formed by the decay of free neutron? Write balanced equation.
•  Define (a) Atomic absorption spectrum (b) Atomic emission spectrum.
•  Give the electronic configuration of an element having atomic number 29.
•  Calculate the wave number of photon, when the electron jumps from n=5 to n=2.
•  Why the atomic radius decreases along period and increases along group?
•  Why Sigma bond is stronger than Pi-bond?
•  Why helium gas do not exist in diatomic state?
•  What is paramagnetic character? Give the reason for paramagnetic character of oxygen.

4. Answer briefly any Six parts from the followings: 6 x 2 =12

•  Define molarity of a solution.
• The total volume of the solution by mixing 100cm³ of water with 100 cm³ of alcohol may not be equal to 200cm³ justify it.
• Define colligative properties of solution.
• Calculate oxidation number of "Mn" in KMnO₄.
• What is electrolysis? Give example.
• A salt Bridge maintain electrical neutrality in the cell, justify.
• Differentiate b/w Instantaneous and average rate of reaction.
• The radio active decay is alwais a first order reaction, justify.
• 50% of hypothetical first order reaction completes in one hour. The remaining 50% needs more than one hour to convert itself into products why?

Section ------ II

 Note: Attempt any three questions. (8 x 3=24)

Question #5
(a) What are liquid crystals? Give their uses in daily life.
(b) Mg metal reacts with HCI to give hydrogen gas. What is the minimum volume of HCl solution (27% by weight) required to produce 12.1g of H The density of HCl is 1.14g/cm³ Mg +2HCl → MgCl₂+ H₂

Question #6
(a) Write applications of Dalton's law of partial pressures.
(b) Discuss principal and Azimuthal Quantum numbers.

Question #7.
(a) Write important postulates of VSEPR theory and explain structure of (NH₃) Ammonia according to it.
(b) Discuss the measurement of enthalpy of a reaction with the help of Bomb calorimeter.

Question #8
(a) Write a comprehensive note on activation energy.
(b) Calculate the pH of a buffer solution in which 0.11 molar CH ₃COONa is 0.09 molar acetic acid solution are present (K₀ of CH₃COOH is1.85x10^-5)

Question #9
(a) What is Raoult's law? Give its three statements.
(b) Describe the construction and working of Voltaic or Galvanic cell.

Section -------III (PRACTICAL)

10.Note(i) Attempt any Three parts (5 x 3 = 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

(a) Separate and identify Lead and Cadmium ions in a mixture solution by Paper chromatography?
(b) Purify benzoic acid by water solution?
(c) 3g of NaOH and Na₂SO₄ are dissolved in 500cm³ solution. Find out “x”
(d) 39.2g of FeSO₄ (NH₄)₂ .xH₂O are dissolved per dm³ solution. Find out the value of ' x’
(e) 5g of iodine are dissolved in 250 cm³ solution. Find out %age impurity.