Inter (Part-I) Bahawalpur Board 2016
Chemistry
Part I (Objective Type)
Time Allowed: 20 Minutes 
Max. Marks: 17

Note: Write answers to the questions on the answer sheet provided. four possible answers A, B, C and D to each questions are given which answer is correct, fill the relevant circle with pen ink to each question on the answer sheet provided:

Question #1
Circle the correct option i.e. A/B/C/D. Each part carries one mark.

• The top of Mount Everest water boil at:

a) 70°C
b) 71°C
c) 69°C
d) 68°C

• The nature of positive rays depends on:

a) The nature of the residual gas
b) The nature of the electrode
c) The nature of discharge tube
d) All these

• The Molar volume of CO2 is maximum at:

a) 273°C and 2 atm
b) 0°C and 2 atm
c) 127°C and 1 atm
d) STP

• In Sp² Hybridization, the orbitals are oriented at angle of:

a) 107.5°
b) 109.5°
c) 120°
d) 180°

• The Octet Rule is not followed by:

a) NH₃
b) CF₄
c) CCI₄
d) PCI₅

• Iodine is a:

a) Ionic solid
b) Metallic solid
c) covalent bond
d) molecular solid

• Density of H2O is maximum at:

a) 0°C
b) 2°C
c) -1°C
d) 4°C

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

a) The size of paper used
b) R_f values of solvent
c) Temperature of experiment
d) Size of Chromatographic tank used

• Many elements have fractional element masses this is because:

a) Mass of atom itself fractional
b) Atomic masses are averages mass of isobars
c) Atomic masses are average masses of isotopes proportional to their relative abundance
d) Atomic masses are average masses of isotopes

• The bond angle between two H-S bonds H₂S is:

a) 180°
b) 104.5°
c) 109.5°
d) 92°

• Molarity of pure water is:

a) 2.2
b) 18
c) 55.5
d) 5.55

• The oxidation number of chromium is Cr₂O₃ is:

a) 6
b) -6
c) +3
d) +4

• Stronger the Reducing Agent, greater is the:

a) Oxidation potential
b) Reduction potential
c) Redox potential
d) E.M.F of Cell

• Oxidative potential of SHE is:

a) 0
b) 1
c) 2
d) 4

• The rate of reaction:

a) Decreased as reaction proceed
b) Increases as reaction proceed
c) Remain same as reaction proceed
d) May decreases or increases as reaction proceed

• Critical temperature of NH3 is:

a) 132.44°C
b) -132.44°C
c) 0°C
d) 136.25°C

• 27g of AI will react completely with how much mass of O₂ to produce AI₂O₃:

a) 8g of Oxygen
b) 16g of Oxygen
c) 32 g of oxygen
d) 24g of Oxygen

Inter (Part-I) Bahawalpur Board 2016
Chemistry
Part I (Subjective Type)
Time Allowed: 3.10 Hours 
Max. Marks: 83

Note: It is compulsory to attempt 8 parts each from Q.no.2 and Q.No.3 while attempt 6 parts from Q.no.4 and attempt any 3 questions from part II. Write same q.no and its part no as given in the question paper:

Question #2

• Define Molarity is giving formula to calculate it.
• What is conjugated Solution. Give one example.
• Calculate the oxidation number of “Mn” in KMnO₄.
• Define Electrode Potential.
• Why NaCI and KNO₃ are used to tower melting point to ice?
• Give reactions taking place during recharging of lead accumulator battery.
• Define Instantaneous rate and average rate of reaction.
• How can half life can be used to determine order of reaction?
• Define Energy of Activation. Give Arrhenius equation?

Question #3

• State Heisenberg’s uncertainly principle.
• Why do we need buffer solution?
• Distribute the electrons in the orbitals of ₂₉Cu and ₃₅Br.
• Why CO₂ and CH₄ has no Dipole solution?
• Why e/m values of positive rays for different gases are different but those for cathode rays the e/m values are the same?
• What is Moseley’s Law? Give its mathematical expression.
• Define Enthalpy of Solution. Give two examples.
• Differentiate between Polar covalent bond and Non- Polar covalent Bond.
• Some Spontaneous reaction require energy to start. Give example
• Why the second ionization energy value of an element is always greater than the first ionization energy value?
• Why the solubility of KI in water increase with increase in temperature?
• Why the ions pairs of electron on an atom occupy greater space than bond pairs?

Question #4

• Define relative atomic mass.
• How limiting reactant be defined?
• State distribution law.
• Give uses of chromatography.
• Define Critical temperature.
• Give two applications of plasma.
• Evaporation causes cooling. Give reason.
• Give four properties of ionic solids.
• Calculate the value of ideal gas constant R in dm³ atm.
• Define Anisotropy.
• One feels sense of cooling under the fan after the bath. Give reason.
• Calculate the mass in grams of 2.90 moles of KMnO₄.

PART-II

Question #5
(a) Give detail difference between continuous and discontinuous solubility curve?
(b) Give four characteristics of catalyst.

Question #6
(a) Define atomic orbital hybridization. Explain the shape of Ethyne Molecule on the basis of atomic Orbital Hybridization.
(b) Explain the construction and working of fuel cells.

Question #7
(a) Ca (OH)₂ is a sparingly soluble compound. Its solubility product is 6.5x1^-6 Calculate the solubility of Ca(OH)₂.
(b) State and explain Hess’s law of constant Heat summation.

Question #8
(a) State Graham’s law of diffusion. Write down its Experimental verification.
(b) What is J.J Thomsons experiment for determining e/m value of electron?

Question #9
(a) What are the liquid crystals? Give three applications of liquid crystals.
(b) calculate the number of grams of AI₂S₃ which can be prepared by the reaction of 20g of AI and 30g of Sulphur. How much the non-limiting reactant is in excess.
2∆I +3S → ∆I₂S₃

Part-III (Practical part)

Question #10
(A) Separate the mixture of ink by paper chromatography.
(B) Purify the given sample of Benzoic Acid by Crystallization method.
(C) 8g of mixture of NaOH and NaCI have been dissolved per dm³ of solution. Find percentage of NaOH by volumetric method.
(D) 27.8g of FeSO₄ . xH₂O have been dissolved per dm³ of solution. Find value of “x” by volumetric method.
(E) The given solution contains 30g of impure iodine dissolved per dm³ of solution. Find percentage purity of sample by volumetric method.