BISE Gujranwala · Class 11 · Chemistry

BISE Gujranwala · Class 11 · Chemistry · 2025 · First Annual · Group 1

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: 6483 · 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 circle in front of the relevant question number. Use marker or pen to fill in the circles. Cutting or filling of two or more circles will result zero mark in that question.

OBJECTIVE

Q1(1)
The amount of energy is released by absorbing electron in
- (A)
  Ionization energy
- (B)
  Electron affinity
- (C)
  Electronegativity
- (D)
  Atomization energy
Q1(2)
Acetone and Chloroform are soluble in each other due to
- (A)
  Intermolecular Hydrogen Bonding
- (B)
  Ion dipole interaction
- (C)
  Instantaneous dipole
- (D)
  Intramolecular Hydrogen Bonding
Q1(3)
The cathodic reaction in the electrolysis of dil. $H_{2} S O_{4}$ with Pt electrodes is
- (A)
  Reduction
- (B)
  Oxidation
- (C)
  Both Oxidation and Reduction
- (D)
  Neither Oxidation nor Reduction
Q1(4)
In the rate equation of a reaction $2 A + B ⟶$ products is, rate $= k [A]^{2} [B]$ , and A is present in large excess, then order of reaction is
- (A)
  1
- (B)
  2
- (C)
  3
- (D)
  Zero
Q1(5)
Absolute zero is equal to
- (A)
  $273^{\circ} C$
- (B)
  $- 273^{\circ} C$
- (C)
  $0^{\circ} C$
- (D)
  $273 K$
Q1(6)
1 mole of ${O H}^{- 1}$ ion is equal to
- (A)
  $18 g$
- (B)
  $16 g$
- (C)
  $10 g$
- (D)
  $17 g$
Q1(7)
When '6' d orbital is complete, the entering electron goes into
- (A)
  7 f
- (B)
  7 s
- (C)
  7 p
- (D)
  7 d
Q1(8)
Density of ice is less than that of water due to
- (A)
  Empty spaces in structure of ice
- (B)
  Tetra hydral shape of crystals of ice
- (C)
  Large bond length
- (D)
  Large bond angles
Q1(9)
The number of moles of $C O_{2}$ which contain $8.0 g$ of Oxygen
- (A)
  0.25
- (B)
  0.50
- (C)
  1.00
- (D)
  1.50
Q1(10)
For which system does the equilibrium constant 'Kc' has unit of $(c o n c e n t r a t i o n)^{- 1}$ ?
- (A)
  $N_{2} + 3 H_{2} ⇌ 2 N H_{3}$
- (B)
  $H_{2} + I_{2} ⇌ 2 H I$
- (C)
  $2 N O_{2} ⇌ N_{2} O_{4}$
- (D)
  $2 H F ⇌ H_{2} + F_{2}$
Q1(11)
$18 g$ of glucose dissolved in $90 g$ of water. The relative lowering of vapour pressure is equal to
- (A)
  $\frac{1}{5}$
- (B)
  5.1
- (C)
  $\frac{1}{51}$
- (D)
  6
Q1(12)
The value of Planck's constant is
- (A)
  $6.62 \times 10^{- 34} J . s e c$
- (B)
  $6.62 \times 10^{- 27} J . s e c$
- (C)
  $6.62 \times 10^{- 21} J . s e c$
- (D)
  $6.62 \times 10^{- 31} J . s e c$
Q1(13)
By adding $N H_{4} C l$ to $N H_{4} O H$ solution the ionization of $N H_{4} O H$
- (A)
  Increases
- (B)
  Increases 100 times
- (C)
  Remains constant
- (D)
  Decreases
Q1(14)
The change in heat energy of a chemical reaction at constant temperature and pressure is called
- (A)
  Enthalpy Change
- (B)
  Bond Energy
- (C)
  Heat of Sublimation
- (D)
  Internal Energy Change
Q1(15)
The molar volume of $C O_{2}$ is maximum at
- (A)
  STP
- (B)
  $127^{\circ} C$ and $1 a t m$
- (C)
  $0^{\circ} C$ and $2 a t m$
- (D)
  $273^{\circ} C$ and $2 a t m$
Q1(16)
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
Q1(17)
Which of the molecules has zero dipole moment
- (A)
  $N H_{3}$
- (B)
  $C H C l_{3}$
- (C)
  $H_{2} O$
- (D)
  $B F_{3}$

Subjective

Source code: 217 · Printed marks: 68 · Time: 2:40 Hours

Note: Section I is compulsory. Attempt any THREE (3) questions from Section II.
Q2: Write short answers to any EIGHT (8) questions. (2×8 = 16)
Q3: Write short answers to any EIGHT (8) questions. (2×8 = 16)
Q4: Write short answers to any SIX (6) questions. (2×6 = 12)

SECTION-I

2
Write short answers to any EIGHT (8) questions.
Q2(i)
Differentiate between empirical and molecular formulas.
(2 marks)
Q2(ii)
Define Mole and Avogadro's number.
(2 marks)
Q2(iii)
What is limiting reactant?
(2 marks)
Q2(iv)
Define sublimation. Write down names of two solids which undergo sublimation.
(2 marks)
Q2(v)
Why is there a need to crystallize the crude product?
(2 marks)
Q2(vi)
$S O_{2}$ is comparatively non-ideal at $273 K$ but behaves ideally at $327^{\circ} C$ . Give reason.
(2 marks)
Q2(vii)
Define critical temperature and critical pressure.
(2 marks)
Q2(viii)
Write down two characteristics of plasma.
(2 marks)
Q2(ix)
How is Caustic Soda obtained in Nelson Cell?
(2 marks)
Q2(x)
Calculate the oxidation number of Phosphorus in $N a_{3} P O_{4}$ .
(2 marks)
Q2(xi)
What is pseudo first order reaction? Give one example.
(2 marks)
Q2(xii)
What is activated complex?
(2 marks)
3
Write short answers to any EIGHT (8) questions.
Q3(i)
How evaporation causes cooling?
(2 marks)
Q3(ii)
Why ethane ( $C_{2} H_{6}$ ) is a gas whereas hexane ( $C_{6} H_{14}$ ) is liquid?
(2 marks)
Q3(iii)
Define polymorphism. Give an example.
(2 marks)
Q3(iv)
What is unit cell? Give its dimensions.
(2 marks)
Q3(v)
Write down two properties of positive rays.
(2 marks)
Q3(vi)
Calculate mass of electron from its charge and $\frac{e}{m}$ values.
(2 marks)
Q3(vii)
Give electronic configuration of (a) $_{24} C r$ (b) $_{20} C a$
(2 marks)
1. (a)
  $_{24} C r$
2. (b)
  $_{20} C a$
Q3(viii)
What is atomic emission spectrum?
(2 marks)
Q3(ix)
Write down the Le-Chatelier's Principle.
(2 marks)
Q3(x)
Define common ion effect. Give an example.
(2 marks)
Q3(xi)
How buffer solutions are prepared?
(2 marks)
Q3(xii)
Derive $K c$ units for the reaction: $N_{2} + 3 H_{2} ⇌ 2 N H_{3}$
(2 marks)
4
Write short answers to any SIX (6) questions.
Q4(i)
Dipole moment of $C O_{2}$ is zero but $S O_{2}$ is $1.61 D$ . Why?
(2 marks)
Q4(ii)
Give difference between lone pair and bond pair of electron with example.
(2 marks)
Q4(iii)
$C O_{2}$ is nonpolar whereas $H_{2} O$ is a polar molecule. Why?
(2 marks)
Q4(iv)
Why $N H_{3}$ is pyramidal molecule.
(2 marks)
Q4(v)
Differentiate between Internal Energy change and Enthalpy change.
(2 marks)
Q4(vi)
Define state and state function.
(2 marks)
Q4(vii)
What is water of crystallization? Give one example.
(2 marks)
Q4(viii)
What are ideal solutions? Give one example.
(2 marks)
Q4(ix)
What are Azeotropic mixtures?
(2 marks)

SECTION-II

Attempt any THREE (3) questions from Section II.

Q5(a)
$10.0 g$ of $H_{3} P O_{4}$ has been dissolved in excess of water to dissociate it completely into ions. Calculate the number of molecules of $H_{3} P O_{4}$ in $10.0 g$ of $H_{3} P O_{4}$ . Also calculate the number of positive and negative ions in case of complete dissociation.
(4 marks)
Q5(b)
Write down four applications of Dalton's law of partial pressure.
(4 marks)
Q6(a)
What are molecular solids? Write down any three properties of Molecular solids.
(4 marks)
Q6(b)
Define orbital Hybridization. Explain $s p^{3}$ Hybridization with one example.
(4 marks)
Q7(a)
Discuss in detail Azimuthal Quantum Number.
(4 marks)
Q7(b)
Describe how the enthalpy of combustion of a substance is measured by bomb calorimeter.
(4 marks)
Q8(a)
Define order of reaction. Discuss in detail first order reaction.
(4 marks)
Q8(b)
What is the percentage of ionization of acetic acid in which $0.1$ mole of it has been dissolved per $d m^{3}$ of solution?
(4 marks)
Q9(a)
Write down measurement of boiling point elevation by Landsberg's method.
(4 marks)
Q9(b)
Explain fuel cell in detail with diagram.
(4 marks)

Original source references (2)

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

Objective · 6483 · Printed marks: 17 · Time: 20 Minutes
Subjective · 217 · Printed marks: 68 · Time: 2:40 Hours