1st Year Chemistry Past Papers

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• The number of moles of hydrogen atoms in 92g alcohol (C2H5OH) are:
• (a) 5 moles
• (b) 6 moles
• (c) 10 moles
• (d) 12 moles
• The number of moles of CO2 which contain 8.0g of oxygen:
• (a) 1.50
• (b) 1.0
• (c) 0.50
• (d) 0.25
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• The comparative rates at which the solute move in paper chromatography depend on:
• (a) Size of paper
• (b) Rf values
• (c) Temperature
• (d) Size of chromatographic tank
• The liquid having highest boiling point is:
• (a) Hydrofluoric acid
• (b) Hydrogen sulphide
• (c) Water
• (d) Ammonia
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• Which impurity makes the shape of sodium chloride crystal needle like:
• (a) MgSO4
• (b) Urea
• (c) MgCO3
• (d) Glucose
• When one beta (B) particle is emitted from the nucleus of an atom its:
• (a) Atomic number increases by 1
• (b) Atomic number decreases by 1
• (c) Atomic mass increases by 1
• (d) Atomic mass decreases by 1
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• The charge on proton is:
• (a) 1.6022×10-C
• (b) 1.6022×10C
• (c) 1.6022×10-19C
• (d) 1.6022×10¹°C
• In nitrogen molecule (N2), each nitrogen atom contributes in sharing for formation of bond:
• (a) One electron
• (b) Two electrons
• (c) Three electrons
• (d) Four electrons
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• Which one has highest value of ionization energy: 
• (a) Be  
• (b) C   
• (c) F  
• (d) O
• The pressure of oxygen in bomb calorimeter is:
• (a) 10 atm.
• (b) 15 atm.
• (c) 20 atm
• (b) 25 atm.
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• For which system does the equilibrium constant, K. has units of (concentration):
• (a) N2+3H2 2NH3
• (b) 2NO2 N2O4
• (c) H2+12 2HI
• (d) PCl5PCl3+ Cl2
• Which one affects the value of K.?
• (a) Concentration
• (b) Temperature
• (c) Pressure
• (d) Catalyst
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• The gases show more deviation at:
• (a) Low temperature and low pressure
• (b) High temperature and low pressure
• (c) High temperature and high pressure
• (d) Low temperature and high pressure
• Which one affects the value of K.?
• (a) Concentration
• (b) Temperature
• (c) Pressure
• (d) Catalyst
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• One molar solution of glucose (C6H12O6) contains the amount of solute in 500cm³ solution:
• (a) 180g
• (b) 45g
• (c) 90g
• (d) 270g
• molarity of pure water is:
• (a) 1
• (b) 18
• (c) 55.5
• (d) 16
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• The oxidation state of oxygen in KO2 is:
• (a) -1
• (b) -2
• (c) -1/2
• (d) +2
• The order of for the reaction 2N2O5 ---- 2N2O4 + O2 is: 
• (a) Zero Order
• (b) First Order
• (c) Second Order
• (d) Third Order
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• 2. Write short answers of any EIGHT parts.
• (i) differentiate between cation and anion.
• (ii) Many chemical reactions taking place in our surrounding involve the limiting reactants. Justify it.
• (iii) How is percentage (%) yield calculated?
• (iv) What is R value? Give its unit if any.
• (v) How can you dry crystals by different ways?
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• (vi) Calculate numerical value of R in S.I. units, for one mole of a gas at STP.
• (vii) Explain Avogadro's law briefly.
• (viii) Define diffusion and effusion of gases.
• (ix) What happens to the acidic and basic properties of aqueous solutions when pH varies from zero to 14?
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• (x) Prepare acidic and basic buffers with one example in each case.
• xi) What will be the effect of increase of pressure and temperature on the following reaction? 
• N2(g) +3H2(g) 2NH3(g) ΔΗ = -92.46kJ
• (xii) Define solubility product constant and derive solubility product expression for Ag2CrO4
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• 3. Write short answers of any EIGHT parts.
• (i) Define allotropy. Give two allotropic forms of carbon.
• (ii) Explain that evaporation is a cooling process.
• (iii) Define isomorphism with an example.
• (iv) What are Debye forces? Explain.
• (v) What is bond order? Give an example.
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• (vi) The dipole-moment of CO2 is zero but that of CO is 0.12D. Give reason.
• (vii) Define Pi (π) bond with an example.
• (viii) Bond distance is the compromise distance between two atoms. Explain.
• (ix) Prove that AE = q
• (x) Define spontaneous reactions with two examples.
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• (xi) What is meant by conjugate solutions?
• (xii) Define molarity and molality.
• 4. Write short answers of any SIX parts.
• (i) State Moseley's law. Give its mathematical formula.
• (ii) Give two defects of Rutherford's atomic model.
• (iii) Why is it necessary to decrease the pressure in the discharge tube to get the cathode rays?
• (iv) Write electronic configuration of Cu(29) and Sc(21).
• (v) What are secondary cells? Give two examples.
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• (vi) What is oxidation number? Calculate oxidation number of Mn in KMnO4
• (vii) How does a salt bridge maintain the electrical neutrality in a galvanic cell?
• (viii) What is heterogeneous catalysis? Give one example.
• (ix) Define half life period of a reaction. Give one example.
• 5. (a) What are metallic solids? Discuss their properties.
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• (b) 8.657g of compound were decomposed into elements and gave 5.217g of carbon, 0.962g of hydrogen, 2.478g of oxygen. Calculate the percentage composition of the compound under study.
• 6. (a) Define plasma state. How is it formed? Describe its four applications.
• (b) Derive the general formula to calculate the radius of 'nth' orbit of H-atom by using Bohr's atomic model.
• 7. (a) Define dipole moment. Give its applications.
• (b) Define and explain Hess's law of constant heat summation with two examples.
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• 8. (a) Define law of mass action. Derive equilibrium constant expression for a given reversible reaction: aA+bB CC + dD
• (b) What is standard hydrogen electrode (SHE)? How is it used to measure the electrode potential of Zinc (Zn).
• 9. (a) 3g of a non-volatile, non-electrolyte solute 'X' are dissolved in 50gm of ether (molar mass = 74) at 293K. The vapour pressure of ether falls from 442 torr to 426 torr. Under these conditions calculate molar mass of solute 'X'
• (b) what is meant by energy of activation? Explain its importance for chemical reactions.
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