Inter (Part-1) Lahore Board 2014
Chemistry  paper 1(Objective Type)
Time Allowed: 20 Minutes Max.Marks: 17
(Group-1)
Note: Four possible answers A,B,C and D to each question are given.The choice which you think is correct,fill that circle in front of that question with Marker or Pen ink.Cutting or filling two or more circles will result in zero mark in that question.

• Dry Ice (Solid CO₂) is an example of solid :
  
  (a)Covalent
  (b)Molecular
  (c)Ionic
  (d)Metalic
  
  
• Specific rate constant is equal to rate of reaction, when concentration of reactants are:
  
  (a)Zero
  (b)Four
  (c)Three
  (d)Unity
  
  
• Number of bonds in N2 molecule :
  
  (a)1ϭ +1л
  (b)2ϭ + 1л
  (c)1ϭ + 2л
  (d)1л + 3ϭ
  
  
•  Largest number of molecules are in :
  
  (a)6 gmH₂O
  (b)8 gm C₂H₅OH
  (c)8 gmCO
  (d)8 gm N₂O₅
  
  
• Glycerine decomposes at its :
  
  (a)Melting point
  (b)Boiling point
  (c)Freezing point
  (d)Critical point
  
  
• Maximum no.of electrons in an orbital is :
  
  (a)6
  (b)10
  (c)14
  (d)2
  
  
• Gooch crucible is made of :
  
  (a)Clay
  (b)Asbestos
  (c)Porcelain
  (d)Iron
  
  
• Oxidation No.of oxygen in OF2 is :
  
  (a)Zero
  (b)-1/2
  (c)+2
  (d)-1
  
  
• Molarity of pure water is :
  
  (a)1
  (b)18
  (c)5
  (d)6
  
  
• Solvent extraction is a process :
  
  (a)Exothermic
  (b)Endothermic
  (c)Equillibrium
  (d)Non- equilibrium
  
  
• Ph of 10ˉ³ mole dmˉ³ of an aqueous solution of H₂SO₄ is :
  
  (a)3
  (b)7
  (c)2
  (d)5
  
  
• If “a” and “b” are zero for certain gas then gas is :
  
  (a)Ideal
  (b)Real
  (c)Non-ideal
  (d)May be any diatomic gas
  
  
• CSF has ionic character :
  
  (a)60%
  (b)80%
  (c)92%
  (d)100%
  
  
• Mass of one mole of electron is :
  
  (a)008 mg
  (b)55mg
  (c)84 mg
  (d)673 mg
  
  
• 66CU(Equation
  
  (a)Proton
  (b)Position
  (c)Electron
  (d)Neutron
  
  
• In Endothermic reaction ∆H is taken as:
  
  (a)Positive
  (b)Negative
  (c)Zero
  (d)May be any value
  
  
• Escape out of gas molecules one by one through tiny hole is :
  
  (a)Diffusion
  (b)Effusion
  (c)Osmosis
  (d)All of these

Inter (Part-1) Lahore Board 2014
Chemistry paper 1 (Essay Type)
Time Allowed: 3:10 hours Max.Marks : 83
(Group-1)
(SECTION-1)

2.write short answers to any Eight (8) questions : 16

• No individual neon atom in the sample of the element has a mass of 20.18 amu.
• Give assumption of stoichiometry.
• Calculate mass in kg of 2.6 *10²⁰ molecules of SO2.
• Why is there a need to crystallize the crude product?
• What is sublimation? Give one example of sublime solid.
• Exlain boyl’s law according to kinetic molecular theory of gases .
• What are isotherms?
• Define Avogadro’s law.
• Explain why evaporation takes place at all temperatures .
• Why heat of sublimation of iodine is very high ?
• Why ionic crystals do not conduct electricity in the solid state ?
• Define transition temperature with an example .

3.write short answers to any EIGHT (8) questions:

• Write down the electronic configuration of Fe (26) and Br (35)
• What is the difference between continuous spectrum and line spectrum ?
• Give any two properties of neutrons.
• What is Hund’s rule?
• How does ionization energy vary in periodic table ?
• Why is the radius of a cation smaller than its parent taom ?
• Define bond order. Calculate bond order of hydrogen molecule.
• Define co-ordinate covalent bond and give an example.
• What is state function?give two examples.
• What do you know about internal energy of a system?
• Explain why ionic solids are brittle.
• Iodine dissolves readily in carbon tetrachloride ,why ?

4.write short answers to nay six (6) questions):

• Define PH of a solution.Give its mathematical equation.
• Why is the vapor pressure of a solution less than pure solvent ?
• Calculate the percentage by weight of NaCl if 2g of it is dissolved in 20g of H2O.
• What is meant by water of crystallization ?Give an example .
• What is difference between metallic conduction and electrolytic conduction?
• Define standard electrode potential .
• Give chemical reactions taking place at anode and cathode in a fuel cell.
• Write down any two characteristics of enzyme catalysis.
• Define order of reaction.give one example .

(SECTION-2)
Note: Attempt any THREE questions
Question#5

(a) What are liquid crystals ? Give their uses in daily life . 4
(b) write down the steps to calculate empirical formula . 4

Question#6
(a) describe the bonding in O2 according to molecular orbital theory and explain its paramagnetic property. 4
(b) Define and explain Hess’s law and give its applications. 4

Question#7

(a) write down Milikan’s oil drop method for the measurement of charge of an Electron. 4
(b) one mole of methane gas is maintained at 300 K, its volume is 250 cm³ ,calculate the pressure exerted by the gas when it is non ideal . 4

Question#8

(a)Describe Nickel Cdmium Cell (rechargeable ). 4
(b) Ca(OH)₂ is a sparingly soluble compound .its solubility product is 6.5*10ˉ⁶ .Calculate the solubility of Ca(OH)_{2. .} .4

Question#9

(a)define the following terms:

1. Molarity
2. Molality
3. Mole fraction
4. parts per million

(b) write a brief note on the following :

1. Homogeneous Catalysis
2. Heterogeneous catalysis

(SECTION-3) (practical part )
Note:Attempt any three questions .
Write down standard solution ,chemical equation with mole ratio,indicator with end point ,procedure and supposed reading with calculation for part A,B,and C. 1,1,1,1,1 Write down material required, diagram and procedure for part D and E. 1,1,3

A) 5.6g of MOH are dissolved per dm³ of solution .Find out the atomic mass of M . 5
B) 27.8 g of FeSO_{4 .} *H₂O are dissolved per dm³of a solution .Find the value of x. 5
C) 30 g of a sample of sodium thiosulphate (Na₂S₂O₃ .5H₂O) has been dissolved per dm³ of a solution . Find out the %age purity of the sample . 5
D) Separate Pb⁺² and Cd⁺² ions by paper chromatography. 5
E) prepare pure and dry crystals of benzoic acid . 5

Inter (Part -1) Lahore Board 2014
Chemistry Paper 1 (Objective Type)
Time Allowed: 20 Minutes Max. Marks:17
(Group-II)
Note: Four possible answers A,B ,C and D to each question are given.The choice which you think is correct, fill that circle in front of that Question with Maker or Pen ink. Cutting or filling two or more circlesWill result in zero mark in that question.

• Which one of the following is a pseudo solid:
  
  (A)caF₂
  (B) Nacl
  (C) Borax 
  (D) Glass 2
  
  
• If the rate equation of a reaction 2A + B→products is rate = K ^│A│ │B│and A is Present in large excess order of reaction is:
  
  (A) First order
  (B) Second order
  (C) third order
  (D) Zero order
  
  
• Which of the hydrogen halid has the highest percentage of ionic character:
  
  (A) HI
  (B) HBr
  (C) HCl
  (D) HF
  
  
• In combustion analysis H₂O vapours are absorbed by:
  
  (A) Mg(ClQ₂)₂
  (B) Mg(ClO₃)₂
  (C) Mg(ClO₄)₂
  (D) 50% KOH
  
  
• Water may boil at 120⁰C when external pressure is:
  
  (A) 369 torr
  (B) 700 torr
  (C) 760 torr
  (D) 1489 torr
  
  
• 6 The maximum number of electrons in a sub-shell is given by:
  
  (A) 2l +1
  (B) 2l -1
  (C) 2(2l+1)
  (D) 2(2l-1)
  
  
• 7 Which one of the following substance is used as decolourizing agent:
  
  (A) Silica Gel
  (B) Conc.H₂SO₄
  (C) Animal charcoal
  (D) Asbestos
  
  
• 8 Cathode in NICAD cell is:
  
  (A) Ag₂0
  (B) NiO₂
  (C) Cd
  (D) Zn
  
  
• 9 the solution of glucose is 10% w/v . The volume in which 1g mole of it is Dissolved will be:
  
  (A) 1 dm³
  (B) 1.5 dm³
  (C) 1.8 dm³
  (D) 900 cm³
  
  
• 10 Which is not used as drying agent in vacuum desiccator is:
  
  (A) P₂O₅
  (B) Cacl₂
  (C) MgCl₂
  (D) Silica Gel
  
  
• 11 When HCl is added to H₂S aqueous solution its ionization:
  
  (A) Increase
  (B) Decreases
  (C) Remains contant
  
  
• 12 Which gas will diffuse more rapidly:
  
  (A) HCl
  (B) CO₂
  (C) NH₃
  (D) dSP³
  
  
•  13 The number of moles of CO₂ which contains 8.0 g of oxygen:
  
  (A) 0.25
  (B) 0.50
  (C) 0.75
  (D) 1.0
  
  
• 14 The hybridization of carbon in C₂H₄ is:
  
  (A) SP³
  (B) SP²
  (C) SP
  (D) dSP³
  
  
• 15 The nature of positive rays depends upon:
  
  (A) Nature of electrode
  (B) Nature of residual gas
  (C) Nature of discharge tube
  (D) Pressure inside the discharge tube
  
  
• 16 Which is not a state function:
  
  (A) Energy
  (B) Heat
  (C) Temperature
  (D) Volume
  
  
• Pressure remaining constant at which temperature the volume of a gas will Become twice of what it is at O ^oC:
  
  (A) 546 K
  (B) 273 K
  (C) 546 ⁰C
  (D) 200 ⁰C

Inter (Part-I) Lahore Board 2014
Chemistry Paper I (Essay Type)
Time Allowed: 3J0 hours Max. Marks: 83 (Group-II)
(SECTION-1)

2. Write short answers to any EIGHT(8) questions: 16

• Write function of Mg- (CC04)2 and KOH in combustion analysis. Define molecular ion, write its uses.
• Why we calculate %age yield?
• Define sublimond and sublimate.
• Write main uses of chromatography.
• Justify that volume of gas becomes theoretically zero at —273. °C, Evaporation causes cooling. Why?
• Ionic crystals are highly brittle. Why?
• Cleavage is an anisotropjc behaviour, explain it. Why boiling point of H20 is greater than HF?

3. Write short answers to any EIGHT (8) questions : 16

• Calculate the mass of electron when its elm value is 13588 x 1011 C K g^-1
• Write two importances of Moseley law.
• Define Pauli's Exclusion Principle with an example.
• Write a nuclear reaction for the decay of free neutron.
• 7E-bonds are more diffused than o-bonds Give reason.
• What is bond order? Give an example.
• Define electronegativity. Give its trend in the periodic table.
• Define coordinate covalent bond and giv one example.
• What is thermochemical equation? Give two examples.
• Define heat of neutralization with an example.
•  What is common ion effect? Give an example.
• What is Pk_a and Pk_b?

4. Write short answers to any SIX (6) questions. 12

• What i5 Henderson's equation?
• Define geotropic mixtures. Give one example.
• Boiling points of the solvents increase due to the presence of solutes. Justify it.
• Define molarity and molality.
• What is the purpose of salt bridge'?
• Calculate the oxidation number of `Mn’in KMnO₄
• What is difference between electrolytic and voltaic cell?
• Define activation energy and activated complex.
• Define order of reaction with the help of an example.

(SECTION-1I) Note: Attempt any THREE questions
Question#5
(a) What are molecular solids? Give examples and explain their properties.
(b) What is stoichiometry? Give it assumptions. Mention two important laws, which help to perform the stoichiometric calculations. 4

Question#6
(a) . Explain structure of CH₄ on the basis of hybridization theory.
(b) Prove that :E=q_v

Question#7
(a) Calculate the mass of 1 dm³ of NH₃ gas at 30°C and 1000 mm Hg pressure, considering that NH₃ is behaving ideally. 4
(b) Give the defects of Bohr's atomic model.

Question#8
(a) What is standard hydrogen electrode (SHE)? How it is used to measure the electrode potential of zinc? 4
(b) Calculate the pH of a buffer solution In which 0.11 molar CH3COONa and 0.09 molar aceticacid solutions are present. Ka for CH30001 is 1.85 x 10-5. 4

Question#9
(a) Describe the freezing point depression method for the determination of molecular mass of an organic compound. 4
(b) How rate of reaction depends upon the following factors : 0) Nature of reactants (ii) Surface area.

(SECTION-111) (Practical Part)
Note: Attempt any THREE questions.

(ii) Write down standard solution, chemical equation with mole ratio, indicator with end point, procedure and supposed reading with calculation for Part A, B, and C

(iii) Write down material required, diagram and procedure for Part D and E. 1,1,3

(A) 12.0 grams of a commercial sample of washing soda has been dissolved per di of solution. Determine the percentage of Na 2CO3 in the sample. volumetrically. (Molecular Mass of Na2001 106 ) 5

(B) 6.0 grams of a mixture of K Mn0₄ and _K2SO4 have been dissolved per do 3 of solution. Find out the percentage of each component volumetrically. (Molecular mas of NISIINKN4n04 = 158). 5

(C) 20.0 grams of commercial iodine (12) is dissolved per dm' solution. Find out percentage purity of the sample volumetrically, (Molecular mass of I₂ = 254. 5
(D) Separate mixture of three inks by chromatography, 5
(E) Purify commercial sample of sodium chloride by passing 1- HC1 gas. 5