Chemistry 
Paper I
(Objective type)
(Inter-A-2014)
Time :20 min
Inter(Part – I),
Group-1
Marks : 17
Lahore board 2016
Session : (2012-2014)

Note: Four possible answers A, B, C and D to each question are give. The choice which you think I correct, fill that circle I front of that question with Marker or Pen ink in the answer-book. Cutting or filling two or more circle will result in zero mark in that question

• In the ground state of an atom, the electron is present:
  
  A) In the nucleus
  B) Nearest to the nucleus
  C) In the second shell
  D) Farthest from the nucleus
  
  
• In zero order reaction, the rate is independent of
  
  A) Temperature of reaction
  B) Concentration of products
  C) Concentration of reactants
  D) Light
  
  
• The net heat change in a chemical reaction is same, whether it is brought about in two or more different ways in one or several steps. It is known as:
  
  A) Henry’s law
  B) Hess’s law
  C) Joule’s principle
  D) Law of conservation of energy
  
  
• One mole of SO₂contains
  
  A) 02×10₂₃atoms of oxygen
  B) 02×10₂₃atoms of Sulphur
  C) 1×10₂₃ molecules of SO₂
  D) 4 gram atoms of SO₂
  
  
• The molecular of CO₂ in dry ice from the:
  
  A) Ionic crystals
  B) Molecular crystals
  C) Covalent crystals
  D) Metallic crystals
  
  
• The number of bonds in nitrogen molecule is:
  
  A) One O and one TT
  B) One O and two TT
  C) Three sigma only
  D) Two O and TT
  
  
• Solvent extraction method is particularly useful technique for separation, when the product to be separated is:
  
  A) Non-volatile or thermally unstable
  B) Non-volatile or thermally stable
  C) Volatile or thermally stable
  D) Volatile or thermally unstable
  
  
• If a strip of Cu metal is placed in a solution of FeSO₄
  
  A) Cu will be deposited
  B) Fe is precipitated out
  C) Cu and Fe both dissolve
  D) No reaction take place
  
  
• 18 g glucose is dissolved in 90 g of water. the relative lowering of vapor pressure is equal to:
  
  A) 1/5
  B) 1
  C) 1/51
  D) 6
  
  
• The deviation of a gas from ideal behavior is maximum at:
  
  A) -10 C and 5.0 atm
  B) -10C and 2.0 atm
  C) 100C and 2.0 atm
  D) 0C and 2.0 atm
  
  
• For which system does equilibrium constant, K, has units of (concentration)^-1
  
  A) N₂ + 3H₂ ⇌ 2NH₃
  B) H₂ + I₂ ⇌ 2HI
  C) 2NO₂ ⇌ N₂O₄
  D) 2HF ⇌ H₂ + F₂

• The order of the rate of diffusion of gases NH₃ , SO₂, C_l2 and CO₂ is :
  
  A) NH₃ >SO₂>CL₂ >CO₂
  B) NH₃ >CO₂>SO₂ >Cl₂
  C) Cl₂>SO₂>CO₂>NH₃
  D) NH₃>CO₂>Cl₂>SO₂
  
  
• Which of the hydrogen halides has the highest percentage of ionic character:
  
  A) HCL
  B) HBr
  C) HF
  D) HI
  
  
• 27 g of Al will react completely with how much mass of O₂ to produce Al₂O₃:
  
  A) 8 g of oxygen
  B) 18 g of oxygen
  C) 32 g of oxygen
  D) 24 g of oxygen
  
  
• Quantum number value for 2p orbitals are:
  Which of the following represents the total energy of mass spring system during SHM?
  
  A) n=2,L=1
  B) n=1,L=2
  C) n=1,L=0
  D) n=2,L=0
  
  
• The pH of 10^-3 mol dm^-3 of an aqueous solution of H₂SO₄ is:
  
  A) 3.0
  B) 2.7
  C) 2.0
  D) 1.5
  
  
• In order to mention the boiling point of water at 110C, the external pressure should be:
  
  A) Between 760 torr and 1200 torr
  B) Between 200 torr and 760 torr
  C) 765 torr
  D) 320 torr

Chemistry 
Paper I (Essay type)
(Inter-A-2014)
Time:2.40Min
Inter (Part – I),
Group-1
Marks : 68 
Lahore board 2016
Session : (2012-2014)

SECTION-1

2. Write short answer to any eight (8) questions: (16)

• N₂ and co has the same number of electrons, protons and neutrons. Justify it.
• Calculate the number of moles of O atoms in 9.00 gram of Mg (NO₃)
• Define molecular ion.how it is formed?
• How crystals are dried by reliable method?
• Write four properties of a good solvent.
• Calculate the value of “R” gas constant in IS units?
• State Avogadro’ law of gasses. Give two examples.
• The plot of PV versus P is a straight line at constant temperature and with a fixed number of moles of an ideal gas. Justify.
• Define solubility product, drive solubility. Product expression for sparingly soluble compound Ag₂CrO
• Calculate the pH of 10^-4 mole dm^-3 of Ba(OH)₂
• Why aqueous solution of CH₃COONa is basic in nature?
• What is the name of four major parts of apparatus used in Landsberger’s method for elevation of boiling point?

3. Write short notes on any EIGHT (8) questions: (16)

• Why does evaporation cause cooling?
• Define molar heat of fusion and molar heat of vaporization
• What is transition temperature? Give its one example.
• Write four properties of molecular solids
• Cathode rays are material in nature.justify it
• Write the two drawbacks of Rutherford’s model of atoms
• Define Heisenberg’s uncertainty principle and give its mathematical expression.
• What is orbital? Draw the shape of P orbital.
• Differentiate between molarity and molality.
• Calculate the oxidation number of manganese in KMnO₄.
• What is function of salt bridge in voltaic cell?
• Write two advantages of fuel cells.

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

• Why the abnormality of bond energy and bon strength in HI is less prominent then that of HCL?
• Why the dipole moment of CO₂ is zero but that of SO₂ is 1.61 D?
• Why the melting points, boiling points, heat of sublimation and heat of vaporization of electrovalent compounds are higher as compared with those covalent compounds?
• Why BF₃ is non-polar but SO₂ is polar?
• Differentiate between law of conservation of energy and Hess’s law.
• Why it is necessary of mention the physical states of reactants and products in a thermo chemical equation of a reaction?
• How surface area affects the rate of reaction? Give one example.
• What do you mean by activation energy of a reaction?
• What is auto catalyst? Give one example.

SECTION-II
NOTE: attempt any three questions:

Q.NO.5

(a )NH₃ gas can be prepared by heating together two solids NH₄CL and Ca(OH)₂.if a mixture of 100 gm of each solid is heated then calculate the number of grams of NH₃ produced:
2NH₄CL(s) +Ca (OH) 2(s)à CaCl₂(s) +2NH₃ (g) +2H₂O (L)Atomic mass of H=1.008, N=14, Cl=25.5, O=16, Ca=40
(b)Define liquid crystals and give their three uses.

Q.NO.6

(a)Give the four applications of Dalton’s law of partial pressure.
 (b)How charge on electron is measured by using Milikan’s oil drop method?

Q.NO.7

(a)Define enthalpy and prove that q_p=∆ H.
(b)Explain paramagnetic nature of O₂ according to molecular orbital theory.

Q.NO.8

(a)The solubility of CaF₂ in water at 25C is found to be 2.05 *10^-4 mole dm^-3.what is the value of Ksp at this temperature?
(b)What is the order of reaction?describe two methods for finding order of reaction.(half life method and method of large excess).

Q.NO.9

(a)what is the hydration and hydrolysis?describe with two examples in each.
(b)Write a note on standard hydrogen electrode.how is it used to determine the electrode potential?

Chemistry
Paper I
(Objective type)
(Inter-A-2014)
Time :20 min
Inter (Part – I),
Group-II
Marks : 17
Lahore board 2016
Session : (2012-2014)

Note: Four possible answers A, B, C and D to each question are give. The choice which you think I correct, fill that circle I front of that question with Marker or Pen ink in the answer-book. Cutting or filling two or more circle will result in zero mark in that question

• One mole of SO₂ contains:
  
  A) 02x10²³ atoms of oxygen
  B) 02x10²³ atoms of sulphur
  C) 02x10²³ molecules of SO₂
  D) 4 g atoms of SO₂
  
  
• The volume occupied by 1.4 g of N₂ STP is:
  
  A) 24dm³
  B) 4dm³
  C) 12dm³
  D) 112cm³
  
  
• 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
  
  
• Pressure remaining constant at which temperature the volume of gas will become twice of what it is at 0C.
  
  A) 546C
  B) 200C
  C) 546 K
  D) 273 K
  
  
• Which of the following will have the same number of molecules at STP:
  
  A) 280 cm³ of CO2 and 280 cm3 of N₂O
  B) 44g of N₂ and .6 Dm³ of CO
  C) 2dm³ of O₂ and 32 g of O₂
  D) 28 g of N₂ and 5.6 dm³ of oxygen
  
  
• In order to mention the boiling point of water at 100C the external pressure should be:
  
  A) 765 torr
  B) Between 200 torr and 760 torr
  C) between 760 torr and 1200 torr
  D) any value of pressure
  
  
• Which of the following is a pseudo solid:
  
  A) CaF₂
  B) Glass
  C) NaCL
  D) all of these
  
  
• Quantum number value for 2p orbitals are:
  
  A) n=2,L=1
  B) n=1,L=2
  C) n-1,L=0
  D) n=2,L=0
  
  
• Splitting of spectral lnes of the hydrogen atom under the influence of magnetic field is called:
  
  A) Stark effect
  B) Compton effect
  C) Zeeman effect
  D) photoelectric effect
  
  
• The number of bond in nitrogen molecule is:
  
  A) One O and one TT
  B) Three O only
  C) Two O and one TT
  D) One O nad two TT
  
  
• Which of the following speies has unpaired electrons in antibonding molecular
  
  A) O²⁺₂
  B) N^2-₂
  C) B₂
  D) F₂
  
  
• The change in heat energy of a chemical reaction at constant temperature and pressure is called:
  
  A) Enthalpy change
  B) Bond energy
  C) Heat of sublimation
  D) Internal energy

• The pH of 10^-3 mol dm^-3 of an aqueous solution of H₂SO₄ is:
  
  A) 0
  B) 7
  C) 0
  D) 5
  
  
• Which statement about the following equilibrium is correct:
  2SO₂(g)+O₂(g) 2SO_3ß ∆H = - 188.3K Jmol-1
  
  A) The value of Kp falls with a rose in temperature
  B) The value of Kp falls with increasing pressure
  C) Addinf V₂O₅ catalyst increase the equilibrium’yield of sulphur trioxide
  D) The value of Kp is equal to Kq
  
  
• A solution of glucose is10% w/v, the volume in which one gram mole of it dissolved be :
  
  A) 1dm³
  B) 200 cm³
  C) 1.8dm³
  D) 900cm³
  
  
• If the salt bridge is not used between two half cells then the voltage:
  
  A) Decreases rapidly
  B) Does not change
  C) Decreases slowly
  D) Drops to zero
  
  
• In zero prder reaction the rate is independent of:
  
  A) Temperature of reaction
  B) Concentration of reactants
  C) Concentration of products
  D) Pressure of reaction

Chemistry
Paper I (Essay type)
(Inter-A-2014)
Time 2.40hrs
Inter (Part – I),
Group-II
Marks : 68
Lahore board 2016
Session : (2012-2014

SECTION –I

2. Write short notes on any EIGHT (8) questions: (16)

• One molt of H2SO4 should completely react with two moles of NaOH.how does Avogadro’s number help to explain it?
• Describe that one mole of h2O has two moles of bonds, three moles of atoms, ten moles of electrons and twenty eight moles of the total fundamental particles present in it.
• How H₂ and CO have same number of electrons, protons and neutrons?
• Why concentrated HCL and KMnO₄ solutions cannot be filtered by Gooch’s crucible?
• Write names of major steps involved in crystallization?
• What do you mean by critical temperature of gases?
• What do you mean by absolute zero temperature of gases?
• Why lighter gases diffuse more rapidly than heavier gases?
• What is solubility product? What is solubility product expression for PbCL₂?
• Why change of volume disturbs the equilibrium position for some of the gasses phase reactions but not the equilibrium constant?
• How the molality is independent of temperature but molarity depends upon temperature?
• One mole solution of urea in water is dilute as compared to one molar solution of urea in water but the number of particles of solute in both solutions are same.

3. Write short notes on any Eight (8) questions: (16)

• Describes that heat of sublimation is greater than heat of vaporization.
• Evaporation is a cooling process. Explain.
• Define lattice energy with an examples.
• Why ice floats over the surface of water?
• Write two defects of Rutherford’s atomic model.
• State Pauli’s exclusion principle.
• Give, the electronic configuration of ₂₄
• Write two properties of neutron.
• Describe that boiling point of solvent increase due to the presence of solute.
• Calculate oxidation number of “S” in:
• Cr₂ (SO₄)₃ II) SO^2-₄
• Write recharging of lead accumulator battery
• Define electrochemistry?

4. Write short answer to any six (6) questions: (12)

• Why an ionic radius is greater than atomic radius?
• State electronegativity and electron affinity.
• Write two points of valence bond theory.
• Ionization energy decreases down the group, although nuclear charge increase, explain?
• What is internal energy of a system?
• How surface area affects the rate of reaction>give one example.
• State rate of chemical reaction and give its units.
• Define with example 2^nd order reaction.
• The radioactive decay is always a first order reaction explain.

SECTION-II
Note: attempt any three questions:

Q.NO.5

(a) The combustion analysis of an organic compound shows it to contain 65.44% carbon, 5.50% hydrogen and 29.06% oxygen. What is the empirical formula of the compound? If the molecular mass of the compound is 110.15 gm mole calculate the molecular formula of the compound?
(b) What is vapor pressure of liquid? Also discuss its measurement by manometric method.

Q.NO.6

(a) Give eight postulates of the KMT.
(b) Define quantum number, discuss briefly azimuthal quantum number.

Q.NO.7

(a) Write the main points of valence shell electron pair repulsion theory and explain the structure of ammonia on the basis of this theory.
(b) State and explain Hess’s law of constant heat summation with an example.

Q.NO.8

(a) Ca(OH)₂ is a sparingly soluble compound. Its solubility product (Ksp) is 6.5*10^-6? Calculate the solubility of Ca (OH) ₂
(b) Explain effect of temperature on rate of reaction.

Q.NO.9

(a) State different from of roult’s law. How this law can help us to understand the ideality of a solution?
(b) What is electrochemical series? Explain any three applications of electrochemical series.