BISE Multan · Class 11 · Chemistry

BISE Multan · Class 11 · Chemistry · 2025 · First Annual · Group 2

2025 · First Annual

Transcribed from the identified examination paper. Check the board, session and course before use. SchoolOrbit is not affiliated with the issuing board.

Objective

Source code: 2484 · Printed marks: 17 · Time: 20 Minutes

You have four choices for each objective type question as A, B, C and D. The choice which you think is correct, fill that bubble in front of that question number, on bubble sheet. Use marker or pen to fill the bubbles. Cutting or filling two or more bubbles will result in zero mark in that question.

OBJECTIVE

Q1(1)
Number of molecules in one $d m^{3}$ of water is close to:
- (A)
  $\frac{6.02}{22.4} \times 10^{23}$
- (B)
  $\frac{12.04}{22.4} \times 10^{23}$
- (C)
  $\frac{18}{22.4} \times 10^{23}$
- (D)
  $55.6 \times 6.02 \times 10^{23}$
Q1(2)
The deviation of a gas from ideal behaviour is maximum:
- (A)
  $- 10^{\circ} C$ and $5.0 a t m$
- (B)
  $- 10^{\circ} C$ and $2.0 a t m$
- (C)
  $100^{\circ} C$ and $2.0 a t m$
- (D)
  $0^{\circ} C$ and $2.0 a t m$
Q1(3)
In order to raise the boiling point of water upto $110^{\circ} C$ , the external pressure should be:
- (A)
  765 torr
- (B)
  Between 200 torr and 760 torr
- (C)
  Between 760 torr and 1200 torr
- (D)
  Any value of pressure
Q1(4)
$\underline{}$ is pseudo solid.
- (A)
  $C a F_{2}$
- (B)
  Glass
- (C)
  $N a C l$
- (D)
  $K C l$
Q1(5)
The wave number of light emitted by a certain source is $2 \times 10^{6} m^{- 1}$ . The wave length of this light will be:
- (A)
  $5 \times 10^{7} m$
- (B)
  $500 m$
- (C)
  $200 n m$
- (D)
  $500 n m$
Q1(6)
Quantum number values for $2 p$ orbitals are:
- (A)
  $n = 2, ℓ = 1$
- (B)
  $n = 1, ℓ = 2$
- (C)
  $n = 1, ℓ = 0$
- (D)
  $n = 2, ℓ = 0$
Q1(7)
$\underline{}$ species has unpaired electrons in antibonding molecular orbital.
- (A)
  ${O_{2}}^{2 -}$
- (B)
  ${N_{2}}^{2 -}$
- (C)
  $B_{2}$
- (D)
  $F_{2}$
Q1(8)
$\underline{}$ molecule has planer triangular shape with respect to VSEPR theory.
- (A)
  $C H_{4}$
- (B)
  $B e C l_{2}$
- (C)
  $N H_{3}$
- (D)
  $B F_{3}$
Q1(9)
Calorie is equivalent to:
- (A)
  $0.4184 J$
- (B)
  $41.84 J$
- (C)
  $4.184 J$
- (D)
  $418.4 J$
Q1(10)
The $p H$ of $10^{- 4} m o l d m^{- 3}$ of $H C l$ is:
- (A)
  3.0
- (B)
  4.0
- (C)
  3.7
- (D)
  5.0
Q1(11)
The solubility product of $A g C l$ is $2.0 \times 10^{- 10} m o l e^{2} . d m^{- 6}$ . The maximum concentration of $A g^{+}$ ion in the solution is:
- (A)
  $1.41 \times 10^{- 5} m o l e . d m^{- 3}$
- (B)
  $2.0 \times 10^{- 10} m o l e . d m^{- 3}$
- (C)
  $1.0 \times 10^{- 10} m o l e . d m^{- 3}$
- (D)
  $4.0 \times 10^{- 20} m o l e . d m^{- 3}$
Q1(12)
An aqueous solution of ethanol in water may have vapour pressure:
- (A)
  Equal to that of water
- (B)
  Equal to that of ethanol
- (C)
  More than that of water
- (D)
  Less than that of water
Q1(13)
Stronger the oxidizing agent, greater is the:
- (A)
  Oxidation potential
- (B)
  Reduction potential
- (C)
  Redox potential
- (D)
  E.M.F of cell
Q1(14)
The rate of reaction:
- (A)
  Increases as the reaction proceeds
- (B)
  May decrease or increase as the reaction proceeds
- (C)
  Remains the same as the reaction proceeds
- (D)
  Decreases as the reaction proceeds
Q1(15)
One mole of $S O_{2}$ contains:
- (A)
  $6.02 \times 10^{23}$ atoms of sulphur
- (B)
  $18.1 \times 10^{23}$ molecules of $S O_{2}$
- (C)
  $6.02 \times 10^{23}$ atoms of oxygen
- (D)
  4 grams atoms of $S O_{2}$
Q1(16)
The volume occupied by $1.4 g$ of $N_{2}$ at S.T.P. is:
- (A)
  $2.24 d m^{3}$
- (B)
  $1.12 d m^{3}$
- (C)
  $22.4 d m^{3}$
- (D)
  $112 c m^{3}$
Q1(17)
Solvent extraction is an equilibrium process and it is controlled by:
- (A)
  Law of mass action
- (B)
  The amount of solvent used
- (C)
  Distribution law
- (D)
  The amount of solute

Subjective

Source code: 22 · Printed marks: 68 · Time: 2.40 Hours

Write same question number and its parts number on answer book, as given in the question paper.
Q2: Attempt any eight parts. 8 × 2 = 16.
Q3: Attempt any eight parts. 8 × 2 = 16.
Q4: Attempt any six parts. 6 × 2 = 12.
Section-II: Attempt any three questions. 3 × 8 = 24.

SECTION-I

Q2(i)
$N_{2}$ and $C O$ have the same number of electrons, protons and neutrons. Justify.
(2 marks)
Q2(ii)
Law of conservation of mass has to be obeyed during stoichiometric calculations. Why?
(2 marks)
Q2(iii)
No individual Neon $(N e)$ atom in the sample of element has a mass of $20.18 a . m . u .$ Why?
(2 marks)
Q2(iv)
Why sintered glass crucible is preferred over Gooch Crucible?
(2 marks)
Q2(v)
Name four important features of solvents chosen for crystallization.
(2 marks)
Q2(vi)
State Charle's Law and write its mathematical form.
(2 marks)
Q2(vii)
Define Graham's law of diffusion and write its mathematical form.
(2 marks)
Q2(viii)
Define critical temperature and pressure.
(2 marks)
Q2(ix)
Define oxidation state with two examples.
(2 marks)
Q2(x)
Calculate oxidation number of $P$ in (a) $H_{3} P O_{3}$ (b) $N a_{3} P O_{4}$
(2 marks)
1. a
  $H_{3} P O_{3}$
  (1 mark)
2. b
  $N a_{3} P O_{4}$
  (1 mark)
Q2(xi)
Differentiate between rate and rate constant of a reaction.
(2 marks)
Q2(xii)
Justify that the radioactive decay is always a first order reaction.
(2 marks)
Q3(i)
Boiling needs a constant supply of heat. Give reason.
(2 marks)
Q3(ii)
Why heat of sublimation is greater than heat of vapourization?
(2 marks)
Q3(iii)
Metals are malleable and ductile. Justify.
(2 marks)
Q3(iv)
Define isomorphism with example.
(2 marks)
Q3(v)
Whichever the gas is used in the discharge tube, the nature of the cathode rays remains the same. Why?
(2 marks)
Q3(vi)
What is $(n + ℓ)$ rule?
(2 marks)
Q3(vii)
Write two points of importance of Moseley law.
(2 marks)
Q3(viii)
What is Plank's Quantum theory?
(2 marks)
Q3(ix)
What are $K_{c}$ and $K_{p}$ and how these are related?
(2 marks)
Q3(x)
During the synthesis of $N H_{3}$ , the temperature is kept low. Why?
(2 marks)
Q3(xi)
What are buffer solutions? How an acidic buffer is prepared?
(2 marks)
Q3(xii)
What is common ion effect? Give an example.
(2 marks)
Q4(i)
Define ionization energy and electron affinity.
(2 marks)
Q4(ii)
How do you compare the bond strength of polar and non-polar molecule?
(2 marks)
Q4(iii)
Why is electron affinity of uninegative ion positive?
(2 marks)
Q4(iv)
How %age of ionic character can be calculated?
(2 marks)
Q4(v)
What is spontaneous process? Give an example.
(2 marks)
Q4(vi)
Define first law of thermodynamics.
(2 marks)
Q4(vii)
Freezing point of solvents is depressed due to the presence of salute. Justify.
(2 marks)
Q4(viii)
Define homogenous and non-homogenous phase.
(2 marks)
Q4(ix)
Molality is independent of temperature but molarity depends upon temperature. Justify it.
(2 marks)

SECTION-II

Q5(a)
$N H_{3}$ gas can be produced by heating together two solids $N H_{4} C l$ and $C a (O H)_{2}$ . If a mixture containing $100 g$ of each solid is heated then calculate the number of grams of $N H_{3}$ produced.
(4 marks)
Q5(b)
Write down any eight postulates of Kinetic Molecular theory.
(4 marks)
Q6(a)
Describe Manometric method for determination of vapour pressure of a liquid.
(4 marks)
Q6(b)
Define $s p^{2}$ -Hybridization. Explain the structure of ethene $(C H_{2} = C H_{2})$
(4 marks)
Q7(a)
Discuss Heisenberg uncertainty principle in detail.
(4 marks)
Q7(b)
Explain Born-Haber cycle in detail with example.
(4 marks)
Q8(a)
$C a (O H)_{2}$ is sparingly soluble compound. Its solubility product is $6.5 \times 10^{- 6}$ . Calculate the solubility of $C a (O H)_{2}$ .
(4 marks)
Q8(b)
Explain Homogeneous and Heterogeneous catalysis with at least two examples of each.
(4 marks)
Q9(a)
State and explain Raoult's Law in three different forms.
(4 marks)
Q9(b)
Describe the fuel cells in detail with diagram and chemical equations.
(4 marks)

Original source references (4)

The original files and numbering are retained. Equivalent files do not repeat the questions above.

Objective · 2484 · Printed marks: 17 · Time: 20 Minutes
Objective · 2486 · Printed marks: 17 · Time: 20 Minutes : same questions, source numbering preserved separately
Objective · 2488 · Printed marks: 17 · Time: 20 Minutes : same questions, source numbering preserved separately
Subjective · 22 · Printed marks: 68 · Time: 2.40 Hours