INTERMEDIAMATE PART-I
CHEMISTRY PAPER-1
TIME ALLOWED: 20 Minutes
OBJECTIVE
MAXIMUM MARKS: 17
Note: You have four choices 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 lining two or more circles will result in zero mark in that question. Attempt as many questions as given in objective type question paper and leave others blank. Write the letter A, B, C or D in the column (write correct option) against each question, If there is a contradiction in the bubble and hand written answer, bubble option will he considered correct.

Question#1

• If absolute Temperature of a gas is doubled and pressure is reduced to one half, Volume of gas will :
  
  (A) Remain unchanged
  (B) Increase four times
  (C) Increase two times
  (D) Be d&ubled
  
  
• The deviation of a gas from ideal behaviour is maximum at:
  
  (A) 10⁰ C and 5.0 atm
  (B) -10⁰ C and 2.0 atm
  (C) -100⁰ C and 2.0 atm
  (D) 0⁰ C and 2.0 atm
  
  
• Aceton and chloroform are soluble in each other due to :
  
  (A) Ion-dipole interaction
  (B) Instantaneous dipole
  (C) Intermolecular
  (D) All of these
  
  
• Which of the following is a Pseudo solid:
  
  (A) CaF₂
  (B) Glass
  (C) NaCℓ
  (D) All
  
  
• Rutherford's model of storm failed because:
  
  (A) The atom did not have a nucleus and electrons
  (B) It did not account for the attraction between proton and neutron
  (C) It did not account for the stability of the atom
  (D) There is actually no space between nucleus and electrons
  
  
• Splitting of spectral lines when atoms are subjected to strong electrical field is called:
  
  (A) Zeeman effect
  (B) Stark effect
  (C) Photoelectric effect
  (D) Compton effect
  
  
• Which of the molecular species has unpaired electrons in antibonding molecular orbitals?
  
  (A) O²⁺₂
  (B) B₂ 
  (C) F
  (D) N²⁺₂
  
  
• Which of the Hydrogen halides has highest percentage of ionic character?
  
  (A) HCℓ
  (B) HBr
  (C) HF
  (D) HI
  
  
• The change in heat energy of a chemical re-action at constant temperature and pressure is called:
  
  (A) Heat of sublimation
  (B) Bond energy
  (C) Internal energy change
  (D) Enthalpy change
  
  
• Which statement about the following equilibrium is correct?
  
  2S0_2(g) + O_{2(g) ═} 2S0_2(g)    𝝙H = -188.3 Kj mol^1-
  (A) The value of Kp falls with rise in temperature
  (B) The value of Kp falls with increase in pressure
  (C) Adding V₂O₅ Catalyst increase the equilibrium yield of SO₃
  (D) The value of Kp is equal to Kc
  
  
• Molaray of pure water is:
  
  (A) I
  (B) 18
  (C) 55.5
  (D) 6
  
  
• If the salt bridge is not used between two half cells, then the voltage:
  
  (A) Decreases rapidly
  (B) Decreases slowly
  (C) Does not change
  (D) Drops to zero
  
  
• If strip of C_u metal is placed in a solution of FeSO₄:
  
  (A) No reaction take place
  (B) Fe is precipitated out
  (C) C_u will be deposited
  (D) C_u and Fe both dissolve
  
  
• In zero order reaction, the rate is independent of:
  
  (A) Temperature of reaction
  (B) Concentration of reactants
  (C) Concentration of products
  (D) None of these
  
  
• One mole of SO₂ contains:
  
  (A) 6.02 x 10²³ atoms of Oxygen
  (B) 18.1 x10²³ molecules of SO₂
  (C) 6.02 x l0²³  atoms of Sulphur
  (D) 4 gram atoms of SO₂
  
  
• The mass of one mole of electron is:
  
  (A) 1.008 mg
  (B) 0.55 mg
  (C) 0.184 mg
  (D) 1.673 mg
  
  
• During the process of crystallization, the hot saturated solution is:
  
  (A) Cooled very slowly to get large sized Crystals
  (B)Cooled at moderate rate to got medium sized crystal
  (C) Evaporated to get the Crystals of the product
  (D) Mixed with an immiscible liquid to get pure crystals of the product

INTERMEDIATE PART-I
CHEMISTRY PAPER-1
TIME ALLOWED: 2.40 Hours
SUBJECTIVE
MAXIMUM MARKS: 68
NOTE: Write same question number and its part number on answer book as given in the question paper.
SECTION-I

2. Attempt any eight parts. 8 x 2 =16

• Define Molecular Ion. How is it generated?
• Calculate the mass in grams of 2.74 moles of KMnO₄
• No individual Neon atom in the sample of Neon element has a mass of 20.18 amu.
• Why sintered glass crucible is preferred to Gooch Crucible.
• Define Adsorption Chromatography and Partition Chromatography.
• Calculate the value of General Gas Constant in S.1 units.
• State Charle's Law and write its mathematical form.
• Gases deviate from ideal behavior more significantly at high and low temperature. Why?
• What is Plasma. Give two uses.
• H₂S is a gas at room temperature but water is liquid. Give reason.
• Give two uses of liquid crystals.
• Diamond is hard and an electrical insulator. Give reason.

3. Attempt any eight parts. 8 x 2 = 16

• State Heisenberg Uncertainty Principle.
• The e/m value of Positive Rays is less than Cathode Rays. Justify.
• Differentiate between Continuous Spectrum and Line Spectrum.
• Define Coordinate Covalent Bond and give one example.
• Explain Octet Rule.
• Define Internal Energy and State Function.
• Differentiate between Spontaneous and Non spontaneous Processes.
• State Enthalpy of Neutralization and give example.
• Differentiate between Hydration and Hydrolysis with two examples.
• The sum of all the mole fractions is equal to one. Discuss.
• Define Electrode Potential.
• Radioactive decay is a first order reaction. Discuss.

4. Attempt any six parts. 6 x 2 =12

• Give any two postulates of Valence Shell Electron Pair Repulsion Theory.
• Define Dipole Moment. Name its two units.
• Show the effect of Common Ion on solubility with an example.
• Define the term Reversible Reaction. Give one example.
• State Law of Mass Action.
• What is Henderson's Equation?
• Calculate Oxidation number of Cr in CrCℓ₃ and K₂Cr₂O_2.
• Give Cathodic and Anodic reactions of electrolysis of concentrated aqueous solution of Sodium Chloride.
• What is negative of a Catalyst? Give example.

SECTION-II

NOTE: Attempt any three questions.
Question#5
(a) Write a note on Avogadro's Number. 4
(b) What is the effect of External Pressure on boiling point of a substance? Give example. 4

Question#6
(a) Explain the Molecular Orbital Theory. Give the molecular orbital configuration and structure of O₂. 4
(b) When 2.00 moles of H₂ and 1.00 mole of O₂ at 100⁰ C and 1 Torr pressure react to produce 2.00 moles of gaseous water, 484.5 KJ of energy are evolved. What are the values of 𝝙 H and 𝝙 E for the production of one mole of H₂O_(g) 4

Question#7

(a) Discuss Chadwick's experiment for the discovery of Neutron. also give the properties of Neutrons. 4
(b) A sample of Nitrogen gas is enclosed in a vessel of volume 380cm³ at 120°C and pressure of 101325 Nm^-2. This gas is transferred to a 10 dm³ flask and cooled to 27⁰ C. Calculate the pressure in Nm^-2 exerted by the gas at 27° C. 4

Question#8
(a) Discuss Law of Mass Action with its mathematical form for general reaction . 4
aA + bB ----- cC + dD 
(b) Balance the following equation by Oxidation number method.4
K₂Cr₂O₂ + HCℓ + CrCℓ₃ + C1₂ + H₂O 

Question#9
(a) Explain “Elevation of boiling temperature". 4
(b) Define
(i) Order of reaction
(ii) Poison
(iii) Activation energy
(iv) Activated complex