Inter (Part-I)
Lahore Board 2013
Chemistry (New Scheme)
Paper: I (Group-I)
Time: 20 Minutes
Marks: 17
OBJECTIVE
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 in the answer-book. Cutting or filling two or more circles will result in zero mark in that question.

• Which statement is not true?

(A) Isotopes with even atomic masses are comparatively abundant.
(B) Isotopes with odd atomic masses are comparatively.
(C) Isotopes even atomic masses and even atomic number are comparatively abundant.
(D) Isotopes with even atomic masses and odd atomic numbers are comparatively abundant.

• 27 g of Al will react completely with how much mass of O₂ to produce Al₂O₃?

(A) 8 g of oxygen
(B) 16 g of oxygen
(C) 32 g of oxygen
(D) 24 g of oxygen

• Solvent extraction method is particularly useful technique for separation when the product to be separated is:

(A) non-volatile or thermally unstable
(B) volatile or thermally stable
(C) non-volatile or thermally stable
(D) volatile or thermally unstable

• Number of molecules in one dm³ of water is close to:

(A)                        

(B)

(C)            

(D)

• London dispersion forces are the only forces present among the:

(A) Molecules of water in liquid state
(B) atoms of helium in gaseous state at high temperature
(C) Molecules of solid iodine
(D) molecules of hydrogen chloride gas.

• The molecules of CO₂ in dry ice from the:

(A) ionic crystals
(B) covalent crystals
(C) molecular crystals
(D) any type of crystals

• Quantum number values for 2₁ orbitals are:

(A) n = 2, ℓ = 1
(B) n = 1, ℓ = 2
(C) n = 1, ℓ = 0
(D) n = 2, ℓ = 0

• The nature of positive rays depends on:

(A) The nature of electrode
(B) The nature of discharge tube
(C) The nature of residual gas
(D) The temperature

• An ionic compound A⁺ B^- is most likely to be formed when:

(A) The ionization energy of A is high and electron affinity of B is low
(B) The ionization energy of A is low and electron affinity of B is high
(C) Both the ionization energy of A and electron affinity of B are high
(D) Both the ionization energy of A and electron affinity of B are low

• Formation of chemical bond takes place when:

(A) Energy is absorbed
(B) Forces of repulsion overcome forces of attraction
(C) Forces of attraction are equal to forces of repulsion
(D) Forces of attraction overcome forces of repulsion.

• For the given process the heat change at constant pressure (q_p) and at constant volume (q_v) are related to each other as:

(A) q_p = q_v
(B) q_p < q_v
(C) q_p > q_v
(D)

• Which statement about the following aquarium is correct?
  2SO_2(g)+ O_2(g) ͢ 2SO_3(g)
  ∆H = - 188.3 KJ/mple

(A) The value of K_p falls with rise in temperature
(B) The value of K_p falls with increase in pressure
(C) Adding V₂O₅ catalyst increases the equilibrium yield of sulphur trioxide
(D) The value K_p = K_c

• Ionic product of water (Kw) increase when temperature increases form 0to 100:

(A) 25 times
(B) 75 times
(C) 55 times
(D) 65 times

• Which solution has the highest voiling point?

(A) 5.85% solution of sodium chloride
(B) 18.00% solution of glucose
(C) 6.00% solution of urea
(D) all have the same boiling point

• Which statement is not correct about galvanic cell?

(A) Anode is negatively charged
(B) Reduction occurs at anode
(C) Cathode is positively charged
(D) Reduction occurs at cathode

• Oxidation state of chromium in K₂CrO₄ is:

(A) 5
(B) 6
(C) 3
(D) 7

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

(A) first order reaction
(B) second order reaction
(C) zero order reaction
(D) third order reaction

Inter (Part-I)
Lahore Board 2013
Chemistry (New Scheme)
Paper: I (Group-I)
Time: 3:10 Hours
Marks: 83
SUBJECTIVE

(Section-I)

2. Write shore answers to any EIGHT (8) question: (16)

• Law of conservation of mass has to be obeyed during stoichiometric calculation, give reason.
• One mg of K₂CrO₄ has trice the number of ions than the number of formula units when ionized in water, justify.
• How many molecules of water are three in 10g of ice?
• Differentiate between adsorption chromatography and partition chromatography.
• Give the importance of sublimation.
• Explain Boyle’s law with the help of ICMT.
• SO₂ is comparatively non-ideal at 273 K but behave ideally at 327.
• Give two application of plasma.
• Ice occupies more space than water, give reason.
• Water and ethanol can mix in all proportions, give reason.
• Ionic solids do not conduct electricity in solid state, give resion.
• Diamond is insulator and hard, give reason.

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

• State spin quantum number (s) briefly.
• What is Planck’s quantum theory?
• Write properties of positive rays.
• Why value for the cathode rays is just equal to that of electorn?
• Define ionization energy and write its variation in the the periodic table.
• The bond angles of H₂O and NH₃ are not 109.5̊ like that of CH₄. Although O-atom and N-atom are SP³ hybridized like C- in CH₄, give reason.
• The dipole moments of CO₂ and CS₂ are zero but that of SO₂is 1.61D.
• What is the basic assumption of VSEPR theory, and discuss the shape of a molecule (BF₃) containing three electron pairs?
• Define the term state function, give two examples.
• Explain the term enthalpy.
• State Le-Chatelier’s principle.
• What is buffer capacity?

4. Write short answers to SIX (6) question: (12)

• Give the two application of the solubility product.
• Depression in freezing point is a colligative property, justify.
• What is meant by molality? Give its formula.
• Why NaCℓ and KNO₃ are used to lower the melting points of ice?
• Define electrochemical series.
• Lead accumulators is a chargeable battery, justify.
• Calculate oxidation number of manganese in KmnO₄ and sulphur in SO₄^2- .
• Define specific rate constant.
• What are enzymes? How they act as catalyst?

(Section-II)

Note: Attempt any THREE question,

5. a) What is boiling point? What is the effect of external pressure on boiling point? Why the temperature of a liquid remains constant at boiling point although heat is continuously supplied? (4)
b) An ideal gas is enclosed in a container having volume 500 CM³ at S.T.P. Its mass comes out to be 0.72 g. What is the molar mass of this gas? (4)

6. a) Explain the molecular orbital structures of following molecules on the basis of the MOT:
(i) N₂ (Nitrogen) (ii) O₂ (Oxygen). (4)
b) State first law of thermodynamics. Prove that ∆E = q_v- (4)

7. a) State Dalton’s Law of Partial Pressure, also give its three application.
b) Describe Millikan’s Oil Drop Method for the measurement of charge on electron. (4)

8. a) Describe the construction and the working of standard hydrogen electrode. (4)
b) What is the percentage ionization of acetic acid in a solution in which 0.1 moles of it has been dissolved per dm³ of the solution? (4)

9. a) Give three statements of Raoult’s law and also mention how Raoult’s law helps in determining the ideality of solution. (4)
b) What is Arrhenius equation? How it can be used to calculate activation energy of a reaction? (4)

(Section-III)
(Practical Part)

Note (i) Attempt ant THREE parts.

(ii) Write down standard solution, chemical equation with mole ratio, indicator with end point, procedure and supposed readings to calculation for Part A, B, and C. (1.1.1.1.1)

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

5. The given solution contains 5.6 g of alkali metal hydroxide ‘MOH’ dissolved per dm³. Find out the atomic mass of metal ‘M’ volumetrically. (5)
6. Determine the % composition of 8 g mixture of KMnO₄ and K₂SO₄ per dm³ by volumetric method (Molecular Mass of KMnO₄ = 158) (5)
7. 8 g of Na₂S₂O₃. XH₂O have been dissolved per dm³. Find out the value of ‘X’ by volumetric method. (Molecular Mass of Na₂S₂O₃ = 158) (5)
8. Uzair mix up the two inks. How you could separate them by using paper chromatographic method? (5)
9. How you could prepare the crystals of benzoic acid from water by using crystallization method? (5)

Inter (Part-I)
Lahore Board 2013
Chemistry (New Scheme)
Paper: I (Group-II)
Time: 20 Minutes
Marks: 17
OBJECTIVE
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 in the answer-book. Cutting or filling two or more circles will result in zero mark in that question.

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

(A) Intermolecular hydrogen bonding
(B) Ion-dipole interaction
(C) Instantaneous dipole
(D) All of these

• The solubility product of AgCl is 2.0 x 10^-10 mole², dm^-6. The maxumum concentration of Ag⁺ ion in the solution is:

(A) 2.0 x 10^-10 mole dm^-3
(B) 1.4 x 10^-5 mole dm^-3
(C) 1.0 x 10^-10 mole dm^-3
(D) 4.0 x 10^-20 mole dm^-3

• The existence of a compound in more than one crystalline forms is called:

(A) Anisotropy
(B) Isomorphism
(C) Allotorpy
(D) Polymorphism

• For the reaction NaOH + HCℓ + H₂O → NaCl + H₂O, the change in wnthaply is called:

(A) Heat of reaction
(B) Heat of formation
(C) heat of neutralization
(D) Heat of combustion

• How many isotopes are present in palladium?

(A) four
(B) Five
(C) Six
(D) Seven

• The geometry of ethane is:

(A) Trigonal planar
(B) linear
(C) V-shaped
(D) Tetrahedral

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

(A) First order reaction
(B) second order reaction
(C) Third order reaction
(D) Zero order reaction

• A solution of glucose is 10% w/v. the volume in which I gram mole of it is dissolved will be:

(A) 1 dm³
(B) 1.8 dm³
(C) 200 cm³
(D) 900 cm³

• The oxidation number of chromium in K₂Cr₂O₇ is:

(A) 14
(B) 12
(C) 6
(D) 13

• 27 g of Al will react completely with how much mass of O₂, to produce Aℓ₂O₃:

(A) 8 g of oxygen
(B) 16 g of oxygen
(C) 32 g of oxygen
(D) 24 g of oxygen

• The velocity of phonton is :

(A) Independent of the wavelength
(B) depends on its wavelength
(C) Equal to square of its amplitude
(D) depends on its source

• Stronger the oxidizing agent, greater is the:

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

• Which of the hydrogen halides has the highest percentage of ionic character?

(A) HF
(B) HBr
(C) HCℓ
(D) Hl

• The term pH introduced by:

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

• Pressure remaining constant at which temperature of the volume of a gas will become twice of what it is at 0:

(A) 546
(B) 200
(C) 546K
(D) 273K

• The value for the positive rays maximum for:

(A) Hydrogen
(B) Helium
(C) Oxygen
(D) Nitrogen

• I² dissolves in water in the presence ok KI due to the formation of:

(A) I₂
(B) I^-
(C) I₃
(D) I₄

Inter (Part-I)
Lahore Board 2013
Chemistry (New Scheme)
Paper: I (Group-I)
Time: 3:10 Hours
Marks: 83
SUBJECTIVE
(Section-1)

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

• Why theoretical yield is greater than actual yield?
• What is mass spectrum?
• Define empirical formula and molecular formula with example
• What is solvent extraction?
• Write down the name of Eight solvent used in crystallization.
• Calculate the value of R in SI unit.
• Give four fundamental postulates of molecular theory of gases.
• Derive graham’s law of diffusion in the light of kinetic molecular theory of gases
• Why one feels sense of cooling under the fan after bath?
• Write down two applications of liquid crystals.
• Define isomorphism and polymorphism with example.
• Why ionic crystals are highly brittle?

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

• Give reason for the production of positive rays.
• Calculate mass of an electron from its value.
• How the K-series, L-series and M-series of x-rays spectrum are produced?
• State Heisenberg’s Uncertainty Principle and give its mathematical expression.
• Why the ionic radius of Cℓ^- ion increases from 99 pm to 181 pm?
• How a coordinate covalent bond differs from a covalent bond?
• Why the energy of antibonding molecular orbital is higher than corresponding bonding molecular orbitals?
• Why the dipole moment of SO₂ is 1.61 D but that of SO₃ is zero?
• State the Hess’s law of constant heat summation.
• Define enthalpy of atomization and give an example.
• Write two application of equilibrium constant.
• Write two uses of buffer solution.

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

• Define pH and pOH.
• Why beckmann’s thermometer is used to measure the depression in freezing point?
• Differentiate between ideal and non-ideal solution.
• One molal solution of glucose is dilute as compared to one molar solution of glucose . Justify it.
• Write down two functions of salt bridge in a galvanic cell.
• Write down reaction taking place at the electrodes on the discharging of Nickle-Vadmium Cell.
• Calculate the oxidation number of Cr in K₂CrO₄ and Cr₂O₇^-2.
• Define and give an example of the process of activation of a catalyst.
• What happens to the rate of a chemical reaction with the passage of time?

(Section-II)
Note: Attempt any THREE question.

5. a) What are ionic solids?Give their properties in detail. 4
b) Calculate the number of grams of Aℓ₂S₃ which can be prepared by the reaction of 20g of Aℓ and 30g of sulphur. How much the non-limiting reactant is in excess? 4
(Atomic masses: Aℓ :27; S: 32)

6. a) Define electron affinity. Name the factors affecting it. How does it vary in the periodic table? 4
b) Define enthalpy of reaction. How is it measured by glass calorimeter? 4

7. a) Describe Lind’s method for the liquefaction of gases. 4
b) Describe Millikan’s Oil Drop Method for the measurement of charge on electron. 4

8. a) Describe the electrolysis of molten sodium chloride and a concentrated solution of sodium chloride. 4
b) N₂ (g) , H₂ (g) combine to give NH₃ (g). The value of K_c in this reaction is 6.0 x 10^-2 . Calculate the value of K_p for this reaction. 4

9. a) State and explain Raoult’s Law in three forms. 4
b) Explain Arrhenius equation. How does it help us to calculate the energy of activation of reaction? 4

Section-III)
(Practical Part)

Note (i) Attempt ant THREE parts.

(ii) Write down standard solution, chemical equation with mole ratio, indicator with
end point, procedure and supposed readings to calculation for Part A, B, and C.
(1.1.1.1.1)

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

A) 4 g of a mixture of Na₂CO₃ and Na₂SO₄ are dissolved in 500 cm³
Find out the %age composition of the mixture.( Molecular mass of Na₂CO₃ = 106) (5)

B) 3 g of partially oxidized ferrous sulphate are dissolved in 100 cm³ Find out %age oxidation. (Molecular mass of FeSO₄ = 152). (5)

C) 20 g of Na₂S₂O₃ are dissolved in dm³ Fine out the %age of sulphur.
(Molecular mass of Na2S₂O₃ = 158) . (5)

D) Identify Cu²⁺ and Cd²⁺ ions by paper chromatography. (5)