Educational Wealth: 2012

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Old papers</h2>
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English (classical poetry) </h3>
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                          Part 1 --- 2012 </h2>
Time : 3 hrs Paper 1                                                Marks:100  
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                                        Classical Poetry</h3>
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Old papers-Punjab university English(classical Poetry) -2012

Old papers English (classical poetry) click here to read other papers English classical poetry Punjab university laho...

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 Lahore board old papers</h2>
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<tr><td class="tr-caption" style="text-align: center;">Bise Lahore</td></tr>
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  Inter (Part 1) Lahore Board 2012</h3>
 Chemistry Paper I                                        (Objective Type)

Time Allowed: 20 Minutes                                Max. Marks: 17
                                                  
(Group-I) 
 Note: Four possible answers A, B, C and D to each question are given. The choice which you think is correct, fill that circle in front of that question with Marker or Pen ink.  
Cutting or filling two or more circles will result in

zero mark in that question. Write the letter A, B, C

or D in the column (write correct option) against each question also. If there is a contradiction in the bubble and hand written answer, bubble option will be considered correct.  
Q. 1.1 .The mass of one mole of electrons is :  
           (A) 1.008 mg (B) 0.55 mg (C) 0.184mg (D)

1.673 mg 
 (2)     The number of moles of C02 which contain

8.0 g of oxygen   
           is:'

(A) 0.25 (B) 0.50 (C) 1.0 (D) 1.50  
(3)       The drying agent used in a desiccator is :  
           (A) AgCl (B) NlCf (C) CaCf2 (D) AfCf  
(4)       Pressure remaining constant, at which

temperature the  
           volume of a gas will become

twice of what it is at 0 °C 
           (A) 546°C (B) 200°C (C) 546 K (D) 273 K.  
 (5)      The partial pressure of oxygen in the lungs is :  
          (A) 760 torr (B) 670 torr (C) 159 ton-

(D) 116 torr 
 (6)    The existence of an element in more than one

crystalline  
          form is called: 
         (A) Allotropy (B) Isotropy (C) Isomorphism

(D)  
         Polymorphism  
 (7)    Acetone and chloroform are soluble in each

other due to:  
         (A) Intermolecular hydrogen bonding

(B) Ion-dipole  
         interaction (C) Instantaneous

dipole (D) Covalent Bonding  
(8)     Nature of the positive rays depend on :  
         (A) The nature of  the cathode (B) The nature of

the  
              anode The nature of the  residual gas

(D) The nature of  
             the discharge tube  
 (9)   Splitting of spectral lines when atoms are

subjected to  
          strong electric field is called :  
          (A) Zeeman effect (B) Stark effect

(C) Compton effect  
          (D) Photoelectric effect  
(10) Which of the following molecule has

zero dipole moment:  
          (A) NH3 (B) CHCl3 (C) H2O (D) BF3 
 (11) The number of bonds in nitrogen molecule is:  
          (A) One sigma and one pi (B) One sigma and

two pi  
          (C) Three sigma only (D) Two sigma

and one pi  
 (12) If an endothermic reaction is allowed to take

place very rapidly  
         in the air, the temperature of

the surrounding an:  
         (A) Remain constant (B) Increases (C) Decreases 
         (D) Remain unchanged  
 (13) The term pH was introduced by:  
        (A) Henderson (B) Sorenson (C) Goldstein

(D) J.J. Thomson  
(14) Molarity of pure water is: 
         (A) 1 (B) 18 (C) 55.5 (D) 6

(15) The oxidation number of  
           chromium in

K2Gr2C7 is:

(A) 14 (B) 12 (C) 6 (D)13  
 (16) Reduction always takes place at:  
         (A) Anode (B) Cathode (C) Both electrodes

(D) Salt bridge  
(17) In zero order reaction, the rate is independent

of :  
        (A) Temperature of reaction

(B) Concentration of reactants  
        (C) Concentration of products

(D) Concentration of  
               reactants and products  
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                             Inter (Part-1) Lahore Board 2012 </h3>
Chemistry Paper I                                              (Essay Type)  
 Time Allowed: 2.40 Hours                                   Max.Marks: 68 
                                         (GROUP-I)  
                                         SECTION-I  
2. Write short answers to any EIGHT (8)

questions: 16 
 (i)   One mg of K2C1O4 has twice the number

of 'ions than the  
        number of formula units when

ionized.  
(ii)   4.9 g of H2S04 when completely ionized in

water have equal  
        number of positive and negative

charges but the number of  
        positively charged

ions are twice the number of negatively  
        charged

ions. 
 (iii) 23 g of sodium and 39 g of potassium have equal

number of   
        atoms in them.  
 (iv)  The desiccator is a safe and reliable method for

drying the  
         crystals. Explain.  
(v) Media which are used for filtration should be set

on the basis of  
        precipitates. Explain  
(vi) Hydrogen and Helium are ideal at room

temperature SO2 and Cl  
       are non-ideal. Explain 
 (vii) Pressure of NH3 gas at given condition

is less as calculated by  
        Van der Waals equation

than by general gas equation.  
(viii)  Water vapours do not behave ideally at 273 K.  
 (ix)  Some of the postulates of kinetic molecular

theory of gases are  
        faulty, Justify. 
 (x) Vacuum distillation can be used to avoid

decomposition of a  
        sensitive liquid. Explain. 
 (xi) Heat of sublimation of iodine is very high

Justify.  
 (xii) Earthenware vessels keep water cool. Explain.  
 Write short answers to any EIGHT (8)

questions : 16  
(i) State Pauli-exclusion Principle.

(ii)  
       Calculate mass of an electron when

e/m = l.758 x 10" C.kg -1  
(iii) What is “Moseley’s law"?  
(iv) Define “Dipole Moment” and give its SI unit.  
(v) What is octet rule? Give two examples of

compounds which  
       deviate from it. 
(vi) Draw labeled diagram of Bomb Calorimeter.  
(vii) Define standard enthalpy of formation with a

suitable example.

(viii) What are thermo chemical reaction, give their

types?  
(ix) Aqueous solution of Q1SO4 is acidic in nature.

Justify it.  
(x) Define “Ebullioscopic Constant” with one

example. 
(xi) Give two applications of electrochemical series.  
(xii) Define rate of chemical reactfon and give its

units.  
4. Write short answers to any SIX (6) questions :12  
(i) Explain why n - bonds are more diffused than a

bonds.  
(ii) The melting points, boiling points, heat of

vapourizations and  
       heat of sublimations of

electrovalent compounds are higher than  
       covalent

compounds. Explain.  
(iii) Explain the terms reversible reaction and state of

equilibrium.

(iv) The solubility of glucose in water is increased by

increasing the  
        temperature. Explain. 
(v) Define PH and POH.  
(vi) How does the change of pressure shifts the

equilibrium position  
      in the synthesis of ammonia?  
(vii) Explain how impure Cu can be purified by

electrolytic process.  
(viii) A salt bridge maintains the electrical neutrality

in the cell.  
        Explain. 
 (ix) Differentiate between enthalpy change of reaction

and energy  
        of activation of reaction.  
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                                            (SECTION - II)</h3>
 Note: Attempt any THREE questions  
 1 . (a) What is difference between actual yield and

theoretical yield?  
            Why actual yield is less than

theoretical yield?              4 
      (b) Classify solids on the basis of bonding. How

ionic solids  
            are formed? Give two properties of

1001c

solids                            4  
2. (a) Write the main postulates of VSEPR theory

and explain the structure of ammonia on the basis

of this theory.                      4 
 (b) When 2.00 moles of H2 and 1.00 mole of 02

at 100°C and 1 torr pressure react to produce 2.00

moles of gaseous water, 484.5 KJ of energy is

evolved? What are the values of (i) AH (ii) AE for

the production of one mole of H20(g)?                                     4  
13. (a) 250 cm3 of a sample of hydrogen effuses four

times as rapidly as 250 cm3 of an unknown gas.

Calculate the molar mass of unknown gas.                                                                          4 
 (b) State and explain with an example, the

Hess’s law

of constant heat summation. .                                                                    4  
4.(a) Write a note on synthesis of ammonia gas by

Haber’s Process keeping in mind the applications

of chemical equilibrium in  
industry.                                                                                  4 
 (b) How can you measure electrode potential of an

element with the help of Standard Hydrogen

Electrode (SHE)?                     4  
5. (a) What are ideal solutions? Explain the fractional

distillation of ideal mixture of two liquids                                                      4 
 (b) How does Arrhenius equation help us to calculate

the energy of activation of a reaction?                                                           4  
                             <a href="http://educational-wealth.blogspot.com/2014/03/old-papers-inter-part-i-lahore-board_7095.html" target="_blank"> previous</a>............More Papers..............Next </div>

11th class question paper 2012 -chemistry Bise Lahore

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