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Inter (Part 1) Lahore Board 2012
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
Inter (Part-1) Lahore Board 2012
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.
(SECTION - II)
Note: Attempt any THREE questions1 . (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
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