BISE Multan · Class 11 · Chemistry

BISE Multan · 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: 2481 · 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)
If the rate equation of the reaction $2 A + B \to p r o d u c t s$ 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)
  None of these
Q1(2)
Stronger the oxidizing agent, greater is the:
- (A)
  Oxidation potential
- (B)
  Reduction potential
- (C)
  Redox potential
- (D)
  E.M.F. of the cell
Q1(3)
Molarity of pure water is:
- (A)
  1
- (B)
  18
- (C)
  55.5
- (D)
  6
Q1(4)
The $p H$ of $10^{- 3} m o l d m^{- 3}$ of an aqueous solution of $H_{2} S O_{4}$ is:
- (A)
  3.0
- (B)
  2.0
- (C)
  1.5
- (D)
  2.7
Q1(5)
$\underline{}$ has $p H$ value more than 7.
- (A)
  Eggs
- (B)
  Milk
- (C)
  Vinegar
- (D)
  Lemons
Q1(6)
In endothermic reactions, the heat content of the:
- (A)
  Reactants is more than that of products
- (B)
  Products is more than that of reactants
- (C)
  Reactants and products is equal
- (D)
  Both A and B
Q1(7)
The number of bonds in nitrogen molecule:
- (A)
  One sigma, one pi
- (B)
  Two sigma, one pi
- (C)
  Three sigma only
- (D)
  One sigma, two pi
Q1(8)
$\underline{}$ has tetrahedron geometry.
- (A)
  $S O_{2}$
- (B)
  $S n C l_{2}$
- (C)
  $C H_{4}$
- (D)
  $B F_{3}$
Q1(9)
Quantum number values for $2 p$ orbitals are:
- (A)
  $n = 2, ℓ = 0$
- (B)
  $n = 1, ℓ = 2$
- (C)
  $n = 1, ℓ = 0$
- (D)
  $n = 2, ℓ = 1$
Q1(10)
Bohr's model can not explain the spectrum of:
- (A)
  $H e$
- (B)
  ${H e}^{+ 1}$
- (C)
  $H$
- (D)
  ${L i}^{+ 2}$
Q1(11)
The molecules of $C O_{2}$ in dry ice form the:
- (A)
  Ionic crystals
- (B)
  Covalent crystals
- (C)
  Molecular crystals
- (D)
  Metallic crystals
Q1(12)
London dispersion forces are the only forces present among the:
- (A)
  Molecules of water in liquid state
- (B)
  Molecules of solid iodine
- (C)
  Atoms of helium in gaseous state at high temperature
- (D)
  Molecules of hydrogen chloride gas
Q1(13)
Equal masses of methane and oxygen are mixed in an empty container at $25^{\circ} C$ , the fraction of total pressure exerted by oxygen is:
- (A)
  $\frac{1}{3}$
- (B)
  $\frac{8}{9}$
- (C)
  $\frac{1}{9}$
- (D)
  $\frac{16}{17}$
Q1(14)
Pressure remaining constant, at which temperature the volume of the gas will become twice of what it is at $0^{\circ} C$ :
- (A)
  $546^{\circ} C$
- (B)
  $200^{\circ} C$
- (C)
  $273 K$
- (D)
  $546 K$
Q1(15)
During the process of crystallization, the hot saturated solution:
- (A)
  Is cooled very slowly to get large sized crystals
- (B)
  Is cooled at moderate rate to get medium sized crystals
- (C)
  Is evaporated to get crystals of product
- (D)
  Is mixed with an immiscible liquid to get crystals
Q1(16)
Isotopes differ in:
- (A)
  Properties which depend upon mass
- (B)
  Arrangement of electrons in orbitals
- (C)
  Chemical properties
- (D)
  Position in the periodic table
Q1(17)
$27 g$ of $A l$ will react completely with how much mass of oxygen to produce $A l_{2} O_{3}$ ?
- (A)
  8g oxygen
- (B)
  16g oxygen
- (C)
  32g oxygen
- (D)
  24g oxygen

Subjective

Source code: 21 · Printed marks: 68 · Time: 2.40 Hours

2025 (1st-A)

INTERMEDIATE PART-I (11th Class)

CHEMISTRY PAPER-I GROUP-I

SUBJECTIVE

NOTE: Write same question number and its parts number on answer book, as given in the question paper.

SECTION-I

2.

Attempt any eight parts.

8 × 2 = 16

(i)
Calculate mass in grams of $2.74$ mol of $K M n O_{4}$ .
(2)
(ii)
Explain that many chemical reactions taking place in our surrounding involve the limiting reactants.
(2)
(iii)
Why actual yield is always less than theoretical yield?
(2)
(iv)
Write any four characteristics of a good solvent for crystallization of a compound.
(2)
(v)
Define sublimation. Name any two sublimates.
(2)
(vi)
Explain Linde's method of liquefaction of gases.
(2)
(vii)
Why real gases deviate from ideal behaviour?
(2)
(viii)
Differentiate between diffusion and effusion of gases.
(2)
(ix)
Calculate the oxidation number of $C r$ (Chromium) in (a) $K_{2} C r O_{4}$ (b) $K_{2} C r_{2} O_{7}$
(1+1)
(x)
What are redox reactions? Give example.
(1+1)
(xi)
What is reaction Kinetics?
(2)
(xii)
Differentiate between average and instantaneous rate of reaction.
(2)

3.

Attempt any eight parts.

8 × 2 = 16

(i)
Justify that ionic crystals are highly brittle.
(2)
(ii)
Define (a) Anisotropy (b) Cleavage of crystal
(2)
(iii)
What do you know about transition temperature?
(2)
(iv)
Water is liquid at room temperature but $H_{2} S$ is a gas. Give reason.
(2)
(v)
The $e / m$ ratio for positive rays is $1836$ times less than that of cathode rays. Justify.
(2)
(vi)
How the emission spectrum is obtained?
(2)
(vii)
State the Heisenberg's uncertainty principle.
(2)
(viii)
Write down the electronic configuration of: (a) Cobalt( $27$ ) (b) Bromine( $35$ )
(2)
(ix)
What are the buffer solutions? Give one example.
(1+1)
(x)
What is Lowry-Bronsted idea of acids and bases?
(2)
(xi)
How do buffers act?
(2)
(xii)
Define the solubility product.
(2)

4.

Attempt any six parts.

6 × 2 = 12

(i)
How electronegativity values of elements help us in understanding the nature of chemical bond?
(2)
(ii)
The size of the cation is always smaller than its parent atom. Justify with example.
(1+1)
(iii)
Pi $(π)$ bond is more diffused than Sigma $(σ)$ bond. Why?
(2)
(iv)
Define coordinate covalent bond. Give two examples.
(1+1)
(v)
Define enthalpy of formation. Give one example.
(1+1)
(vi)
Burning of coal is spontaneous process. Justify.
(2)
(vii)
What are hydrates? How are they formed?
(1+1)
(viii)
Boiling points of the solvents increase due to the presence of solutes. Justify.
(2)
(ix)
What is the molality of the solution prepared by dissolving $5 g$ of glucose in $250 g$ of water?
(2)

SECTION-II

NOTE: Attempt any three questions.

3 × 8 = 24

5.
(a)
When limestone $(C a C O_{3})$ is roasted, quick lime $(C a O)$ is produced according to the following equation. The actual yield of $C a O$ is $2.5 k g$ , when $4.5 k g$ of limestone is roasted. What is the percentage yield of this reaction. $C a C O_{3} \to C a O + C O_{2}$
(4)
(b)
What is Plasma? Give its any four applications.
(4)
6.
(a)
Define Covalent solids. Give its types. Also write down any two properties of these solids.
(1+3=4)
(b)
Define $s p^{3}$ hybridization. Explain the shape of $N H_{3}$ molecule.
(1+3=4)
7.
(a)
Write down the four defects of Bohr's atomic model.
(4)
(b)
Describe Bomb Calorimeter method for calculation of enthalpy of a substance.
(4)
8.
(a)
The solubility of $P b F_{2}$ at $25^{\circ} C$ is $0.64 g / d m^{3}$ . Calculate $K_{s p}$ of $P b F_{2}$ .
(4)
(b)
Describe half-life method and method of large excess for the finding of the order of reaction.
(4)
9.
(a)
What are continuous and discontinuous solubility curves? Explain with graphs.
(2+2=4)
(b)
Define electrode potential. Write down the measurement of electrode potential of $Z n$ (Zinc) with diagram.
(1+2+1=4)
21-2025(1st-A)-18000 (MULTAN)

Original source references (5)

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

Objective · 2481 · Printed marks: 17 · Time: 20 Minutes
Objective · 2483 · Printed marks: 17 · Time: 20 Minutes : same questions, source numbering preserved separately
Objective · 2485 · Printed marks: 17 · Time: 20 Minutes : same questions, source numbering preserved separately
Objective · 2487 · Printed marks: 17 · Time: 20 Minutes : same questions, source numbering preserved separately
Subjective · 21 · Printed marks: 68 · Time: 2.40 Hours