BISE Multan · Class 11 · Chemistry

BISE Multan · Class 11 · Chemistry · 2026 · First Annual · Group 2 · Old course

2026 · 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: 6482 · 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)
The volume occupied by $1.4 g$ of $N_{2}$ at S.T.P is:
- (A)
  $2.24 d m^{3}$
- (B)
  $22.4 d m^{3}$
- (C)
  $1.12 d m^{3}$
- (D)
  $11.2 d m^{3}$
Q1(2)
The number of isotopes in oxygen is:
- (A)
  One
- (B)
  Three
- (C)
  Two
- (D)
  Four
Q1(3)
The partial pressure of $O_{2}$ in the lungs is:
- (A)
  $116 t o r r$
- (B)
  $159 t o r r$
- (C)
  $560 t o r r$
- (D)
  $760 t o r r$
Q1(4)
Observed pressure of gas in van der Waals equation on the walls of container is less than actual pressure due to:
- (A)
  Haphazard motion
- (B)
  Elastic motion
- (C)
  Repulsive force
- (D)
  Inter molecular attractive forces
Q1(5)
In protein Hydrogen bonding link one spiral to the other, the hydrogen bonding is; between:
- (A)
  $C$ and $H$ atoms
- (B)
  $N$ and $H$ atoms
- (C)
  $O$ and $H$ atoms
- (D)
  $O$ and $N$ atoms
Q1(6)
Noble gases are most stable of all other elements because:
- (A)
  These gases react with one another
- (B)
  These are mono atomic gases, with complete parent shell
- (C)
  Their ionization energies are low
- (D)
  Their $s$ and $p$ orbitals not completely filled
Q1(7)
Triple bond is present in:
- (A)
  $O_{2}$
- (B)
  $H_{2}$
- (C)
  $N_{2}$
- (D)
  $C l_{2}$
Q1(8)
pH of $0.1 M$ $C H_{3} C O O H$ is:
- (A)
  2.89
- (B)
  4.74
- (C)
  7.44
- (D)
  4.92
Q1(9)
Which has the highest $K_{s p}$ ?
- (A)
  $C a C O_{3}$
- (B)
  $B a S O_{4}$
- (C)
  $B a C O_{3}$
- (D)
  $M g C O_{3}$
Q1(10)
Solid which have vapour pressure at a temperature below their melting points when heat start, it is:
- (A)
  Subliming
- (B)
  Melting
- (C)
  Decomposing
- (D)
  Condensing
Q1(11)
Grey tin crystals belong to crystals system:
- (A)
  Tetragonal
- (B)
  Cubic
- (C)
  Orthorhombic
- (D)
  Rhombohedral
Q1(12)
When electron moves with velocity of $2.188 \times 10^{6} m s^{- 1}$ then its wavelength in nanometer will be:
- (A)
  $3.3 n m$
- (B)
  $333 n m$
- (C)
  $33.3 n m$
- (D)
  $0.33 n m$
Q1(13)
The energy of ionization of an atom is the energy difference between orbital:
- (A)
  $E_{2} - E_{1}$
- (B)
  $E_{1} - E_{2}$
- (C)
  $E_{\infty} - E_{n}$
- (D)
  $E_{\infty} - E_{1}$
Q1(14)
For a given process the heat changes at constant pressure $q_{p}$ and at constant volume $q_{v}$ are related to each other:
- (A)
  $q_{p} = q_{v}$
- (B)
  $q_{p} < q_{v}$
- (C)
  $q_{p} > q_{v}$
- (D)
  $q_{p} = \frac{q_{v}}{2}$
Q1(15)
A solution of glucose is $10 % w / v$ , the volume in which its $1$ gram mole is dissolved will be:
- (A)
  $1.8 d m^{3}$
- (B)
  $1.0 d m^{3}$
- (C)
  $200 c m^{3}$
- (D)
  $900 c m^{3}$
Q1(16)
Those cells which can be recharged:
- (A)
  Secondary cells
- (B)
  Primary cells
- (C)
  Dry cells
- (D)
  Alkaline cells
Q1(17)
With increase of $10^{\circ} C$ temperature the rate of reaction doubles, due to:
- (A)
  Decrease in activation energy of reaction
- (B)
  Decrease in the number of collisions between reactant molecules
- (C)
  Increase in $E_{a}$
- (D)
  Increase in number of effective collisions

Subjective

Source code: 22(O) · Printed marks: 68 · Time: 2.40 Hours

2026 (1st-A)

INTERMEDIATE PART-I (11th Class)

CHEMISTRY (OLD COURSE)

PAPER-I

GROUP-II

SUBJECTIVE

Roll No:

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

SECTION-I

2.

Write answers of any eight parts.

8×2=16

(i)
$23 g$ of sodium and $238 g$ of uranium have equal number of atoms in them. Justify.
(2)
(ii)
Calculate the percentage of nitrogen and phosphorus in $(N H_{4})_{3} P O_{4}$
(1+1)
(iii)
The actual yield of reaction is always less than theoretical yield. Give reason.
(2)
(iv)
Give main characteristics of the solvent used for crystallization.
(2)
(v)
Differentiate between adsorption and partition chromatography.
(1+1)
(vi)
What is Joule Thomson effect? Give its significance.
(1+1)
(vii)
$S O_{2}$ is comparatively non-ideal at $273 K$ but behaves ideally at $327^{\circ} C$ . Why?
(2)
(viii)
Define Avogadro's law of gases.
(2)
(ix)
Calculate oxidation number of $C r$ in $C r_{2} (S O_{4})_{3}$ and $K_{2} C r_{2} O_{7}$
(1+1)
(x)
Impure $C u$ can be purified by electrolytic process. Justify.
(2)
(xi)
What is autocatalysis? Give one example.
(1+1)
(xii)
Radioactive decay is always first order reaction. Justify.
(2)

3.

Write answers of any eight parts.

8×2=16

(i)
Evaporation takes place at all temperatures. Explain with reason.
(ii)
Heat of sublimation of iodine is very high. Explain with reason.
(iii)
In the closest packing of atoms of metals, only $74 %$ space is occupied.
(iv)
Sodium chloride and caesium chloride have different structures.
(v)
The $e / m$ value for positive rays is different for different gases.
(vi)
Compare line emission and line absorption spectra.
(vii)
What are X-rays?
(viii)
Distribute electrons in orbitals of $_{57} L a$ and $_{29} C u$
(ix)
The change of volume disturbs the equilibrium position for some of the gaseous phase reactions but not the equilibrium constant.
(x)
What is justification for the increase of ionic product with temperature?
(xi)
What happens to the acidic and basic properties of aqueous solutions when pH varies from zero to $14$ ?
(xii)
Define Lowry Bronsted and Base concept.

4.

Write answers of any six parts.

6×2=12

(i)
What is the cause of chemical combination?
(2)
(ii)
What is electron affinity? How it varies in periodic table?
(1+1)
(iii)
Why bond energy of multiple bonds is greater than single bond?
(2)
(iv)
Why reactions of ionic compounds are fast?
(2)
(v)
Prove that $Δ H = q_{p}$
(2)
(vi)
What is enthalpy of combustion?
(2)
(vii)
What is molarity?
(2)
(viii)
Why relative lowering of vapour pressure is independent of temperature?
(2)
(ix)
What are hydrates? Give example.
(1+1)

SECTION-II

NOTE: Write answers of any three questions.

3×8=24

5.
(a)
Magnesium metal reacts with $H C l$ to give hydrogen gas. What is the minimum volume of $H C l$ solution ( $27 %$ by weight) required to produce $12.1 g$ of $H_{2}$ . The density of $H C l$ solution is $1.14 g / c m^{3}$ . $M g (s) + 2 H C l (a q) ⟶ M g C l_{2} (a q) + H_{2} (g)$
(4)
(b)
What are liquid crystals? Give their uses in daily life.
(1+3=4)
6.
(a)
Define Boyle's law. Also give its experimental verification.
(1+3=4)
(b)
Describe the discovery of electron by discharge tube experiment.
(4)
7.
(a)
Write four postulates of valence shell electron pair repulsion theory.
(1×4=4)
(b)
Define Enthalpy of reaction. How enthalpy of reaction is measured by glass calorimeter? Draw diagram too.
(1+2+1=4)
8.
(a)
The solubility of $C a F_{2}$ in $H_{2} O$ at $25^{\circ} C$ is found to be $2.05 \times 10^{- 2} m o l e d m^{- 3}$ . What is the value of $K_{p}$ at this temperature?
(4)
(b)
Explain Standard Hydrogen Electrode(SHE).
(4)
9.
(a)
Describe Beckman's Method for the determination of Depression in Freezing point.
(4)
(b)
What is catalysis? Write down its types and explain one type in detail.
(1+1+2=4)
22(O)-2026(1st-A)-1000 (MULTAN)

Original source references (5)

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

Objective · 6482 · Printed marks: 17 · Time: 20 Minutes
Objective · 6484 · Printed marks: 17 · Time: 20 Minutes : same questions, source numbering preserved separately
Objective · 6486 · Printed marks: 17 · Time: 20 Minutes : same questions, source numbering preserved separately
Objective · 6488 · Printed marks: 17 · Time: 20 Minutes : same questions, source numbering preserved separately
Subjective · 22(O) · Printed marks: 68 · Time: 2.40 Hours