Past Paper Chemistry 1st Year BISE Lahore 2008

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Inter (Part-l) Lahore Board 2008

Chemistry Paper I (Objective Type)

Time Allowed: 20 Minutes Max. Marks: I7

Note: Write answers to the questions on the objective answer sheet provided. Four possible answers A, B,

C and D to each, question are given. Which answer you consider correct, fill the circle in front of A, B, C or

D with Marker or Pen ink to each question on the answer sheet provided.

1. Height of peak in mass spectrum show:

(A) Number of isotopes

(B) Mass number

(C) Relative abundance

(D) Number of protons2. Rate of filtration can be increased using:

(A) Desiccator

(B) Chromatographic tank

(C) Cold finger

(D) Suction flask

3. A component having small value of K (distribution constant) mostly remains inefficient:

(A) Stationary phase

(B) Mobile phase

(C) Chromatographic tank

(D) None of these

4. Deviation of a gas from ideal behaviour is maximum at:

(A) 10oC and 5atm

(B) -10oC and 2atm

(C) 400oC and 2atm

(D) 0oC and 2atm

5. If the value of a and b in van der waals equation are close to zero for a gas then the gas is :

(A) Ideal (B) Non ideal (C) Highly polar (D) Liquefied easily

6. Coordination number of Na+

ion in NaCl is:

(A) 1 (B) 2 (C) 4 (D) 67. Vapour pressure of a liquid depends upon:

(A) Amount of liquid

(B) surface area

(C) Temperature

(D) Size of container

8. e/m value for positive rays is maximum for:

(A) H (B) O (C) He (D) N


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9. According to Bohrs atomic model, radius of second orbit of hydrogen atom is:

(A) 0.529oA (B) 2.116

oA (C) 4.0

oA (D) 5.0

oA

10. Which of the following species has unpaired electrons in antibonding molecular orbitals:

(A) H2 (B) He2 (C) O2+2

(D) N2-2

11. The molecular orbital can contain maximum electrons equal to:

(A) 1 (B) 2 (C) 3 (D) 4

12. Enthalpy change for the reaction CH4 + 2O2 CO2 + 2H2O is called enthalpy of:

(A) Formation

(B) Combustion

(C) Neutralization

(D) Atomization

13. By adding NH4Cl to NH4OH solution the ionization of NH4OH:

(A) Increases

(B) Decreases

(C) Remains same

(D) Increases 100 times14. PH pf tomato is:

(A) 1.2 (B) 4.2 (C) 7.2 (D) 9.2

15. In the mixture of 28 grams of N2 and 96 grams of O2 the mole fraction of N2 is:

(A) 1.1 (B) 0.51 (C) 0.25 (D) 0.11

16. Electrolysis is used for:

(A) Electroplating

(B) Manufacture of Na

(C) Manufacture of Al

(D) All

17. The catalyst used for the reaction HCOOH H2 + CO2 is:

(A) Copper (B) Alumina (C) Silica (D) Iron


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Inter (Part-l) Lahore Board 2008

(SECTION l)

Chemistry Paper I (Essay Type)

Time Allowed: 2.40 Hours Max. Marks: 68

Note: Out of Q. No. I, 2, 3 and 4 write any Twenty-Two (22) short answers. While writing answer write

question No and its part carefully. Each part carries two marks. 44

1. (i) Prove that one mole of CO2, N2, H2 contain equal number of molecules.

(ii) The atomic masses may be in fractions. Why?

(iii) Why experimental yield is mostly less than the theoretical yield?

(iv) What is solvent extraction?

(v) Define sublimation with an example.

(vi) Give two important scales of thermometry. How are these related?

(vii) Gases deviate move from ideal behavior at 0oC than at 100

oC. Why?

(viii) Calculate the value of gas constant R in S.I units.

2. (i) Differentiate between oxidation and reduction.

(ii) Calculate the oxidation state of Cr in K2Cr2O7 and Cr2O3.

(iii) The standard oxidation potential of Zn is +0.76V and its reduction potential is -0.76V. justifu

it.

(iv) Ionic crystal does not conduct electricity in solid state. Give reason.

(v) Diamond is hard and electrical insulator. Why?

(vi) Define lattice energy. Give example.

(vii) The crystal showing isomorphism mostly have the same atomic ratio. Justify.

(viii) Write the electronic configuration of the elements: (i) Cu = 29 (ii) K = 19.

3. (i) Define Paulis exclusion principle.

(ii) What is stark effect?

(iii) Give any two points which show the ideality of a solution.

(iv) Define molarity and modality. Give their mathematical expression.(v) Differentiate between hydration and hydrolysis with one example each.

(vi) What are conjugate solution? Give an example.

(vii) Why atomic radius is greater than cationic radius?

(viii) Why 2nd

ionization energy of an element is always greater than 1st

ionization energy.

4. (i) Explain that bond are more diffuse than sigma bond.

(ii) Differentiate between bonding molecular orbital and anti-bonding molecular orbital.

(iii) Define state and state functions.


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(iv) Comment that enthalpy of neutralization is merely the heat of formation of one mole of a

liquid.

(v) Derive Kc expression for the reaction:

CH3COOH + C2H5OH CH3COOC2H5 + H2O

(vi) What is an ionic product of water? Give its value at room temperature.

(vii) What are basic buffer solutions?

(viii) What is catalysis? Give an example.

(ix) Differentiate between average and instantaneous rate of reaction.

(SECTION ll)

Note: Attempt any THREE questions

5. (a) What is mass spectrometer? How is it used to determine the relative atomic masses of

isotopes. 4

(b) Calculate the mass of 1 dm3

of NH3 gas at 30oC and 1000 mmHg pressure considering that

NH3 behaving ideally. 4

6. (a) What are molecular solids? Give their properties. 5

(b) Write a note on construction and working of bomb calorimeter. 3

7. (a) What are cathode rays? How these rays are produced? Write their properties. 4

(b) N2 and H2 gases are combined to give NH3 gas. The value of Kc in this reaction at 500oC is

610-2

. Calculate the value of Kp for this reaction. 4

8. (a) Explain what do you understand by the term electro negativity. Discuss its variation in the

periodic table. How does it affect the bonds strengths? 4

(b) Give two statements of Raoults law. Also differentiate between ideal and non-ideal

solutions. 4

9. (a) What is standard electrode potential? Explain the measurement of electrode potential. 4

(b) Explain the effect of temperature on the rate of diffusion. 4

Past Paper Chemistry 1st Year BISE Lahore 2008

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