SARGODHA BOARD 2017
PAPER CHEMISTRY PART-1
Time: 20 MM.(Group-1) (Objective Part)
Marks: 17
Note: You have four choice 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.

 

SARGODHA BOARD 2017
PAPER CHEMISTRY PART-1
Time: 3:10 Hours(Group-1)(Subjective Part)
Marks: 83 Section-I


Q.2 Answer any Eight parts. All parts carry equal marks.

  1. Why theoretical yield of a chemical reaction is greater then the actual yield?
  2. What are ions? Under what conditions, They are produced
  3. What is the justification of two strong peaks in mass spectrum for Bromine while for Iodine, only one peak at 127 a.m.u. is indicated?
  4. What are different steps involved in process of crystallization?
  5. What is the different between Gooch's crucible and Sintered glass crucible?
  6. What are uses of chromatography?
  7. Why SO2 is comparatively non ideal at 273 K but behaves ideally at 327 °C? (viii) Write four applications of plasma?
  8. What is the difference between centigrade scale and Fahrenheit scale and which relationship is used for their interconversion?
  9. What do you mean by acidic buffers and bask buffers? Give one example of each?
  10. How solubility product can be determined from solubility? Give one example? (xii) How extent of a reversible chemical reaction can be indicated by equilibrium constant?

Q.3 Answer any Eight parts. All parts carry equal marks.

  1. What is transition temperature Give one example.
  2. Why ionic solids are highly brittle?
  3. Define molar heat of vaporization with one example
  4. What are intramolecular forces of attaractions. Give one example.
  5. Differentiate between atomic emission spectrum and atomic absorption
  6. Define Zeeman's effect.
  7. State Hund's rule.
  8. Give two postulates of Planks theory.
  9. Differentiate between ideal and non-ideal solutions.
  10. Why concentration in term of molality is independent of temperature while molarity depends upon temperature?
  11. Describe function of salt bridge in voltaic cell.
  12. Why Na, K can displace hydrogen from acids but Pt. and Cu cannot?

Q.4 Answer any Six parts. All parts carry equal marks.

  1.  Cationic radius is smaller then the parent atom. Why?
  2. Dipole moment of CO2 is zero while that of water is 1.85 D. Why?
  3. Define bond order. Give one example.
  4. What is octet rule? Give one example.
  5. Define spontaneous and non-spontaneous process.
  6. Burning of candle is spontaneous process. How?
  7. Write any two characteristics of enzyme catalysis.
  8. What is autocatalyst? Give one example.
  9. Define instantaneous and average rate of reaction

Section-II

NOTE: Attempt any Three questions. All questions carry equal marks.
Q. 5 a. When lime stone (CaCO3) is roasted quick lime (CaO) is produced according to the following equation. The actual yield of CaO is 2.5 kg, when 4.5 kg of lime torte is roasted. What is the percentage yield of this reaction.
CaCO2  CaO + CO2
b. What is meant by the term hydrogen bonding? How does hydrogen bonding explain the properties of Proteins.

Q. 6 a. Derive General gas equation also calculate the value of "R" in S.I units.
b. What are quantum Numbers? Explain Azimuthal Quantum number and magnetic Quantum number,

Q. 7 a. Define ionization Energy. How ionization energy varies along the group and across the period.
b. What is “ First Law of Thermodynamics” Prove that v

Q. 8 a. Ca1culate the percentage ionization of acetic acid in a solution in which 0.1 moles of it has been dissolved per dm3 of the Solution. Kc =1.85x10-5
b. Define standard electrode potential. Explain tint rneasurement of electrode potential of copper.

Q. 9 a. What is Roult's law? Give its three statements.
b. Write a detailed note on determination of rate of reaction by Chemical Method.

SARGODHA BOARD 2017
PAPER CHEMISTRY PART-1
Time: 20 MM.(Group-2)(Objective Part)
Marks: 17
Note: You have four choice 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.

SARGODHA BOARD 2017
PAPER CHEMISTRY
PART-1
Time: 3:10 Hours
(Group-2)
(Subjective Part)
Marks: 83
Section-I

Q.2 Answer any Eight parts. All parts carry equal marks.

  1. Define the term 'atomicity', Give example
  2. No individual neon atom in the sample has mass of 20.18 amu, justify.
  3. Why actual yield is usually less than the theoretical yield?
  4. How crystals are dried in vacuum desiccator?
  5. State Law of distribution constant.
  6. Why is there a need to crystalize the crude product?
  7. Calculate the value of ‘R’ (ideal gas constant) in SI units
  8. Derive Boyle's law from kinetic molecular theory of gases.
  9. Why pilots feel uncomfortable breathing in pressurized cabin?
  10. The change of volume disturbs the equilibrium position for some of the gaseous phase but not the equilibrium constant, justify
  11. What is the solubility product? Derive solubility product expression
    for Ag2CrO4
  12. Give the effect of pressure on the following reversible reaction
    PCl5⇔ PCl3+Cl2

Q.3 Answer any Eight parts. All parts carry equal marks.

  1. Give reason that evaporation causes cooling.
  2. Explain that iodine dissolves readily in tetra chloromethane
  3. Why ionic crystals are highly brittle?
  4. Amorphous Solid like glass is also called super cooled liquid, Explain.
  5. Why e/m value of the cathode rays is just equal to that of election?
  6. Why is it necessary to decrease the pressure in the discharge tube to get the cathode rays?
  7. State Pauli - Exclusion principle
  8. Describe Zeeman Effect
  9. Explain that boiling point of Solvent increases due to the presence of solutes.
  10. Non ideal solutions do not obey Raoult's Law. Give reason
  11. Describe Salt bridge
  12. Explain that Lead accumulator is a chargeable battery.

Q.4 Answer any Six parts. All parts carry equal marks.

  1.  Why NH3 can form co-ordinate covalent bond with H+ but CH4not?
  2. The size of anion is greater than its parent atom. Justify
  3. Draw the geometry of SO2 and SO3 on the basis of VSEPR Theory.
  4. Explain the octet rule with one example.
  5. Define System and State function.
  6. Define the terms standard enthalpy of neutralization and standard enthalpy of atomization.
  7. Define homogeneous and heterogeneous Catalysis with one example of each
  8. The radioactive decay is always a first order reaction. Justify
  9. How higher temperature increases the rate of reaction?

Section-II

NOTE: Attempt any Three questions. All questions carry equal marks.
Q. 5 a. A well known 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?
b. What are molecular solids? Give their characteristics.

Q. 6 a. What is meant by liquefaction of gases? Describe Linde's method of liquefaction of gases,
b. What are quantum numbers? Explain principal quantum number.

Q. 7 a. Explain Co-ordinate Covalent bond,
b. Explain glass calorimetric method for the measurement of enthalpy of reaction.

Q. 8 a. The solubility of CaF2 in water at 25° C is found to be 2.05x10-4 mol dm-3. What is the value of K3p at this temperature?
b. Define electrolysis. Explain the electrolysis of very dilute solution of NaNO3

Q. 9 a. What do you mean by depression of freezing point of solvent by a solute? Derive molecular mass of compound by it?
b. Write a note on
(i) Homogeneous Catalysis
(ii) Heterogeneous Catalysis