Chemistry 2014
(Objective)
Group-I
Inter I
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.I Choose the correct answer

Question#1

• How many isotopes are present in palladium?
  
  (a) Four
  (b) five
  (c) Six
  (d) Seven
  
  
• The mass of one mole of electrons is:
  
  (a) 1.008mg
  (b) 0.55mg
  (c) 0.184
  (d) 1.673 mg
  
  
• Chromatography in which the stationary phase is solid is called:
  
  (a) Partition
  (b) Thin layer
  (c) Adsorption
  (d) Paper
  
  
• Solvent extraction is an equilibrium process and it is controlled by:
  
  (a) Law of mass action
  (b) Distribution law
  (c) The amount of solvent
  (d) The amount of solute
  
  
• Which gas will diffuse more rapidly?
  
  (a) CO₂
  (b) NH₃
  (c) HCl
  (d) SO₂
  
  
• The molar volume of CO2 is maximum at:
  
  (a) STP
  (b) 127⁰C and 1 atm
  (c) O⁰C and 2 atm
  (d) 273⁰C and 2 atm
  
  
• Acetone and chloroform are soluble in each other due to:
  
  (a) Intermolecular
  (b) Ion- Dipole forces
  (c) Instantaneous dipole
  (d) All of above
  
  
• The molecule CO₂ in dry ice from the:
  
  (a) Ionic crystal
  (b) Covalent crystal
  (c) Molecular crystal
  (d) All type of crystal
  
  
• Neutron was discovered by:
  
  (a) Rutherford
  (b) Chadwick
  (c) Goldstein
  (d) Thomson
  
  
• Splitting of spectral lines when atoms are subjected to strong electric field is called:
  
  (a) Zeeman effect
  (b) Stark effect
  (c) Photo electric effect
  (d) Compton effect
  
  
• Which of the hydrogen halides has the highest percentage of ionic character:
  
  (a) HCl
  (b) HBr
  (c) HF
  (d) HI
  
  
• VSEPR theory was proposed by:
  
  (a) Kossel
  (b) Lewis
  (c) Nylholm and Gillespie
  (d) Sidwick
  
  
• Calorie is equivalent to :
  
  (a) 0.4184 J
  (b) 41.84 J
  (c) 40184 J
  (d) 418.4 J
  
  
• The solubility product of AgCl is 2.0x10^-10 mole ² dm^-6. The maximum concentration of Ag⁺ ion in the solution is:
  
  (a) 2.0x10^-10 mol dm^-3
  (b) 1.41x10^-5 mol dm^-3
  (c) 1.0x10^-10 mol dm^-3
  (d) 4.0x10^-20 mol dm^-3
  
  
• The molal boiling point constant is the ratio of the elevation in boiling point to:
  
  (a) Molarity
  (b) Molality
  (c) Mole fraction of solvent
  (d) Mole fraction of solute
  
  
• Stronger the oxidation agent, greater is the:
  
  (a) Oxidation potential
  (b) Reduction potential
  (c) Redox potential
  (d) E.M.F of cell
  
  
• Velocity is constant is the rate of reaction when the concentration of reactants are:
  
  (a) Zero
  (b) Unity
  (c) Two
  (d) Three

SUBJECTIVE TYPE

2. Answer briefly any EIGHT parts from the following: (8x2=16)

• One mg of K₂CrO₄ is thrice the number of ions than mamba of formula units when ionized in water, give reason.
• Calculate the number of water molecules in 27 g of H₂O (Molar mass of H₂O=18)
• How will you identify the limiting reactant'
• Define sublimation.
• Differentiate between partition and adsorption chromatography.
• What are the applications of Dalton's law?
• What is Avogadro's law of gases,
• Why real gases deviate from ideal behavior.
• Evaporation causes cooling, give reason.
• Food is cooked quickly in pressure cooker, give reason.
• Sodium is softer than copper but both are good electrical conductor, give-reason
• Diamond is an insulator, give reason.

3. Answer briefly any EIGHT parts from the following:(8x2=16)

• State any two defects of Bohr’s atomic model.
• What is atomic emission spectrum?
• Find the values of magnetic quantum number, m, When azimuthal quantum number, l is 3
• Why is the double bond stronger than a single bond?
• Bond angles of CH₄, NH₃ and H₂O are different although all have SP³ Justify
• The melting and boiling points of ionic compounds are higher as compared to covalent compound. Why?
• Draw the shapes of ‘s’ and ‘p’ orbital.
• Write Lewis structure of CS₂ and CCl₄.
• Define enthalphy of atomization. Give an example.
• Differentiate between spontaneous and non spontaneous reactions.
• Define law of mass action.
• Write down the relation between PH, POH and Pkw

4. Answer briefly any SIX parts from the following: (6x2=12)

• Explain the term "reversible reaction" and "equilibrium state"
• Define Azeolropic mixtures. Give example
• One molal solution is dilute as compare to one molar solution of glucose. Why?
• Define colligative properties of solution. Give their names.
• Na and K tan displace hydrogen gas from acids but pd and Cu can not. Explain
• Write down the function of salt bridge..
• Why a porous plate or a salt bridge is no required in lead storage cell.
• Differentiate between average and instantaneous rate of reaction.
• Define with example "Auto-Catalysis"

Section – II

Note: Attempt any three questions.
Question#5
(a) Define Vapour pressure., How it is measured by Manometeric Method.
(b) What is Empirical formula? Also discuss combustion Analysis in detail

Question#6
(a) State the postulates of VSEPR theory?
(b) State and explain Hess Law of constant heat summation with an example?

Question#7
(a) 250 Cm³ of the sample of hydrogen effuses four times rapid1y as 250 cm ³ of an unknown gas. Calculate the molar mass of unknown gas.
(b) What are quantum numbers. Discuss principal and Azimuthal quantum numbers.

Question#8
(a) CH₃COOH+ C₂H₅OH H+ CH₃COOC₂H₅+H₂O Sample draw after time "t” contains concentration of the species found to be [CH₃COOH] =0.025 mole dm^-3, [C₂H₅OH]= 0.032 mole dm^-3 [CH₃COOC₂H₅]=0.05 mole dm^-3 [H₂O] = 0.04 mole dm-3 Find out the direction of reaction to get equilibrium if K is 4 
(b) Explain Fuel cell with its construction, electrolytic reaction and diagram.

Question#9
(a) Define Raoult's Law and derive the equation ∆p =p⁰x₂
(b) Differentiate between homogeneous catalysis and heterogeneous catalysis.

(PRACTICAL)
Section- III

10. Attempt any THREE parts:
Write down the standard solution, chemical equation with mole ratio, indicator with end point procedure and supposed reading with calculation for A, B and C.
Write down the material required diagram and procedure for part D and E.

(A) 105 g of impure NaOH are dissolved in 250 Cm³ solution. Find out %age impurity? (Na=23 H=1.008, O=16)
(B) 2.78g of FeSO₄ x H₂O are dissolved in 100 Cm³ solution. Find out the value of x. (Fe-56, S 32)
(C) How will you determine iodine in the given sample solution?
(D) How will you purify the benzoic acid from water solution?
(E) How will you separate a mixture of inks by paper chromatography.