2012
Paper : Chemistry
Inter Part I

(Objective) 

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:

• The volume occupied by 1.4 g of N₂ at S.T.P is:
  a) 2.24dm³
  b) 4 dm³
  c) 1.12 dm³
  d) 112 dm³
  
  
• 2- Pressure remaining constant at which temperature the volume of the gas will become twice what it is at O°C:
  
  a) 546°C
  b) 200°C
  c) 546K
  d) 273 K
  
  
• The comparative rate at which solutes move in paper chromatography depends on:
  
  a) Size of paper
  b) Rf value of solute
• c) Temperature of experiment
  d) size of the chromatographic tank
  
  
• The mass of one mole of electron is:
  
  a) 1.008 mg
  b) 0.55 mg
  c) 0.184mg
  d) 1.673 mg
  
  
• The molar volume of CO2 is maximum at:
  
  a) S.T.P
  b) 127°C and 1 atm
  c) O°C and 2 atm
  d) 273°C and 2 atm
  
  
• Orbitals having same energy are called:
  
  a) Hybrid orbital
  b) Valence Orbital
  c) Degenerate Orbital
  d) Mixed orbital
  
  
• Ionic solids are characterized by:
  
  a) Low melting points
  b) Good conductivity in solid state
  c) High vapours pressure
  d) Solubility in polar solvents
  
  
• Which of the following Halogens has the highest boiling point:
  
  a) F₂
  b) CI₂
  c) I₂
  d) Br₂
  
  
• Quantum number for values for 2p orbitals are:
  
  a) n=2, l=1
  b) n=1, l=2
  c) n=1, l=0
  d) n=2, l=0
  
  
• For a given process the heat changes at constant pressure(qp) and at constant value(qv) are related to each others:
  
  a) qp=qv
  b) qp<qv
  c) qp>qv
  d) qp=1/2qv
  
  
• Which is the following molecule has zero dipole moment:
  
  a) NH₃
  b) CHCI₃
  c) H₂O
  d) CH₄
  
  
• The bond angle in methane molecule is:
  
  a) 104.5°
  b) 107.5°
  c) 109.5°
  d) 120°
  
  
• When NH4CI is dissolved in water the solution formed is:
  
  a) Basic
  b) Acidic
  c) Neutral
  d) Buffer
  
  
• Which one is the strong oxidizing agent:
  
  a) F₂
  b) CI₂
  c) Br₂
  d) I₂
  
  
• For the reaction 2N₂O₅→2N₂O₄+O₂ the order of the reaction is:
  
  a) 2
  b) 1
  c) 3
  d) 0
  
  
• 16- The ph of 10^-3 mole dm^-3 of an aqueous solution of H₂SO₄ is:
  
  a) 3.0
  b) 2.7
  c) 2.0
  d) 1.5 
  
  
• 17- The oxidization number of Cr in K₂Cr₂O₇ is:
  
  a) +3
  b) -6
  c) +6
  d) -3
  
  
  

Subjective type:

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: 

Q.no.2:

•  What is molecular ion? Give an example.
• Define Avogadro’s Numbers. Give its Numerical values.
•  Give four characteristics of a solvent used for crystallization.
•  Give two applications of paper chromatography.
•  No individual neon atom in the sample of element has a mass of 20.18. explain
•  Give quantitative definition of Charles’s Law.
•  Differentiate between Diffusion and effusion of gases.  
•  What is Plasma? Give its two uses.
•  Define critical temperature of a gas. What is the importance for liquefaction of gases?
•  Earthen ware vessels keeps water cool. Explain.
•  Vacuum distillation can be used to avoid decomposition of sensitive liquid. justify it.
• Ionic crystals do not conduct electricity in solid state. Why?

Q.No3:

• How neutron are used in treatment of cancer.
• Differentiate between Atomic Emission and Atomic Absorption Spectrum.
• Define Zeeman’s effect and stark effect.
• Why cationic radius is smaller than its parent atomic radius, give example.
• Define Electronegativity.
• Define state function, give example.
• What do you mean by the internal energy of a system?
• Is it true that a non spontaneous process never happens in the universe? give reason and example.
• What are azeotropic mixtures?
• Why some of the properties are called colligative?
• Write a note on Silver oxide battery.
• Define reaction Kinetics and rate of reaction.

Q.No.4: 

• Define coordinate covalent bond with two examples.
• Explain variation of Ionization energy in the periodic table.
• What are Buffer solutions? Give one example.
• Explain the solubility of glucose in water is increased by increasing the temperature.
• What is the effect of catalyst on Equilibrium constant.
• Define reversible and irreversible reactions.
• Calculate the oxidation number of chromium in i- K2CrO34      ii- Cr2O7
• Impure copper can be purified by electrolytic process. explain it.
• Define Instantaneous and average rate of reaction.

Part-II

Q.no.5:
(a) What is combustion analysis? How can you calculate the percentage of Carbon, Hydrogen and oxygen in an organic compound by this method? 
(b) What are the covalent solids? Discuss their properties in detail.

Q.no.6:
(a) Explain VSEPR theory with suitable examples. 
(b) When two moles of H₂ and 1.0 mole of O₂ at 100° C and 1 torr pressure react to produce 2.0 moles of gaseous water 484.5 KJ of energy are evolved, What are the values of H∆ and E∆ for the production of one mole of H₂O(g)?   

Q.No.7:
(a) A sample of N₂ gas is enclosed in a vessel of volume 380 cm³ at 120 ° C and pressure of 101325 N.m^.-2. This gas is transferred to 10 dm³ flask and cooled to 27° C.  Calculate the pressure in Nm^-2 exerted by the gas at 27 ° C.
(b) Give the postulates of BOHR’ s Atomic theory.

Q.no.8:
(a) Define Ph and POH. How they are related with PKW?
(b) Write comprehensive note on silver oxide and Nickel Cadmium batteries,

Q.no.9:
(a) Describe the four points of differences between ideal and non ideal solution.
(b) Define half life period of reaction. Describe half life method to determine the order of reaction.