Faisalabad Board 2013
Chemistry
Inter (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.

• NH₃ shows a maximum boiling point among

(a)Very small size of nitrogen
(b) Lone pair of electron present on nitrogen
(c) Enhanced electronegative character present
(d) Pyramidal structure of NH,

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

(a) -10°C and 5.0 atm
(b) -10°C and 2.0 atm
(c) 100°C and 2.0 atm
(d) 0°C and 2.0 atm

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

(a) The size of the paper
(b) R, values of solutes
(c) Temperature of the experiment
(d) Size of the chromate-graphic tank used

• The number of moles of CO, which contains 8.0g of oxygen.

(a) 0.25
(b) 0.50
(c) 1.0
(d) 1.50

• The mass of one mole of electrons is:

(a) 1.008 mg
(b) 0.55mg
(c) 0.184 mg
(d) I .673mg

• If the rate equation of a reaction 2,4+ B products is, rate = [4[/3] and A is present in large excess, then the order of reaction is:

(a) 1
(b) 2
(c) 3
(d) None of these

• If the salt bridge is not used between two half cells, then the voltage:

(a) Decreases rapidly
(b) Decreases slowly
(c) Does not change
(d) Drops to zero

• Stronger the oxidizing agents, greater is the:

(a) Oxidation potential
(b) Reduction potential
(c) Redox potential
(d) EMF of the cell

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

(a) 5
(b) 5.1
(c) 1/51
(d) 6

• For which system does the equilibrium constant K, has unit of (conceniration)-1

(a) N;+3H₂NH₃ 
(b) H₂+1₂,2H₁₃
(c) 2N₀N₂0₄ 
(d) 2HF H₂+F₂,

• The pH of 10' mol dm' of an aqueous solution of H, SO, is: 

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

• 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 of the hydrogen halide has the highest percentage of ionic character?

(a) HF
(b) HC1
(c) HBr
(d) HI

• The number of bonds in nitrogen molecule is:

(a) One sigma and one pi
(b) One sigma and two pi
(c) Three sigma only
(d) two sigma and one pi

• Quantum number values for 2p orbitals are:

(a) n =, 2, I = I
(b) n= 1, 1= 2
(c) n = 1, 1= 0
(d) n - 2, I = 0

• Orbitals having same energy are called:

(a) Hybrid orbitals
(b) Valence orbitals
(c) Degenerate orbitals
(d) d-orbitals

• The molecules of CO, in dry ice from the:

(a) Ionic crystals
(b) Covalent crystals
(c) Molecular crystals
(d) Any type of crystals 

Inter (Part-I) Faisalabad Board 2013
Chemistry
Part I (Subjective)
Time Allowed: 2.10 Hours 
Max. Marks: 83 

Section I

Q2 Attempt any EIGHT short questions. (8 x 2 = 16)

1. Write fromulas used for the determination of percentage of C & H.
2. I lgm of carbon is reacted with 32gm of 0₂, to give CO₂,. Which one is limiting reactant?
3. Explain N₂ and CO gave the same number of electrons protons and neutrons.
4. Differentiate between stationary phase and mobile phase.
5. What is disadvantage of slow cooling in crystallization?
6. Ikliat is absolute zero? What happens to real gases while approaching it?
7. Write Si units of 'a' and Wander Wall's constant).
8. Define diffusion and effusion.
9. How sea life survives under frozen sea?
10. Why heat of sublimation is greater than heat of vaporization?
11. Give four applications of liquid crystals.
12. Ionic crystals do not conduct electricity in the solid state. Explain.

Q3 Attempt any EIGHT short questions. (8 x 2 = 16)

1. Give any two nuclear reactions.
2. Give the electronic configuration of an element atomic number 29.
3. Define Hund's rule with an example.
4. Give drawbacks of Rutherford's atomic model.
5. What is the trend of ionization energy in the periodic table in a group and why?
6. How electronegativity values of elements help us in understanding the nature of chemical bond?
7. Draw and explain the geometry of NH₃, molecule according to valence shell electron pair repulsion theory.
8. Define bond order and what is bond order of O²⁺₂?
9. Define Hess's law of constant heat summation.
10. What is it necessary to mention the physical states of reactants and products in a thermochemical reaction? Explain with an example.
11. What are buffer solutions'? Give one use of buffer solution.
12. Why solid Nh₄CL is added in qualitative analysis of 3rd group basic radicals before adding NH₄,OH ?

Q4 Attempt any SIX short questions. (6 x 2 = 12)

1. How NaCl can be purified by common ion effect?
2. The sum of mole fractions of all the components is always equal to unit for any solution. Justify it.
3. Define colligative properties. Name two important colligative properties.
4. What are hydrates? How they are formed?
5. What is the function of salt bridge in a galvanic cell?
6. What are electrode reactions in lead accumulator battery'?
7. Impure Cu can be purified by electrolytic process. Give reason.
8. Define rate of reaction and order of reaction.
9. Write two characteristics of enzyme catalysis.

SECTION  II

Question #5
(a) What is electron pool theory regarding to metallic solids? Also give its four properties.  (4)
(b) When limestone is roasted, quicklime (CaO) is produced according to the following equation. The actual yield of CaO is 2.5 kg, when 4.5kg of limestone is roasted. What is the percentage yield of this reaction?    (4)
CaCO₃(g)—>Ca0(g),+ CO₂(g), When atomic mass of Ca = 40, C = 12, 0 = 16.

Question #6
(a) Define Sp2 hybridization and on its basis explain the structure of ethene.(4)
(b) Describe how the enthalpy of combustion of a substance is measured by bomb calorimeter?   (4)

Question #7
(a) What is a kinetic molecular theory of gases? Derive Boyle's law from kinetic equation.         (4)
(b) What are x-rays? Give the conclusions drawn by Mosely from the study of spectral lines.    (4)    

Question #8
(a) Give the industrial importance of electrolysis process in detail.         (4)
(b) Calculate the pH of: (i)10-4mol.dm-3ofHCL(ii) 1.0mol.dm-3of H2X is only 50% dissociated. (H2X is dibasic acid).  (4)

Question #9
(a) Explain Raoult's law when both components are volatile.           (4)
(b) Define order of reaction. How does half life method can be used for its determination.        (4)

Attempt any THREE questions. (5x 3 = 15)

Question #10
(a) Standardize the given NaOH solution. (Molecular mass of NaOH — 40)  (5)
(b) Find out the percentage purity of Mohr's salt solution, 5g of which is dissolved in 100cm' of solution. (Molecular mass of Molir's salt = 392) (5)
(c)Determine the atomic mass of M in M2S2O3, which is I5.8g dissolved in one dm' of solution iodometrically. (Atomic mass of S = 32)
(d) Separate Pb2+ and Cd2+ ions by chromatography. (5)
(e) Prepare pure and dry crystals of benzoic acid.