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Chemistry 11 Past Paper 2024 | Notely

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All Chemistry 11 papers

Class 11 · Past paper

Chemistry 11 past paper 2024

52 published questions in this index. The full practice view lets you work through them and track your own attempts.

16 MCQs36 written questionsPractise this paper

Question index

1
A liquid is thought to be pure ethanol. Which of the following is the best way to test its purity?
MCQ1 marksannual
1
Calculate the volume of oxygen produced by decomposition of $3.04 \times 10^{24}$ formula units of $KClO_3$ according to the given equation: $2KClO_3 \rightarrow 2KCl + 3O_2$
Part B3 marksannual
1
What is hybridization? Explain the hybridization of $CH_4$ and $BeCl_2$ with orbital diagrams.
Part C7 marksannual
2
Volume occupied by $2\text{ g}$ of $SO_2$ gas at S.T.P will be:

This is a skimmable index, not a replacement for the study surface. Open the practice view to answer questions and use the linked study material.

MCQ1 marksannual

2

Calculate the wave number ($\bar{\nu}$) of $H_\alpha$ in Balmer series and second line in Paschen series of hydrogen spectrum.

Part B3 marksannual

2

Why do real gases deviate from gas laws at low temperature and high pressure? Also explain the deviation by general graphical representation of compressibility factor versus pressu…

Part C7 marksannual

3

The largest/maximum number of molecules are present in:

MCQ1 marksannual

3

In an industrial process 40 g of H₂ produces 100 g of NH₃. Calculate the percentage yield of this reaction: N₂ + 3H₂ → 2NH₃

Part B3 marksannual

3

State first law of thermodynamics. Write its mathematical expression with reference to heat and work. Explain it for a gas confined to a cylinder having a moveable piston, and deri…

Part C6 marksannual

4

Justify the following statements with reference to azimuthal quantum number: (i) s-orbital has maximum two e⁻ (ii) p-orbital can accommodate maximum six electrons.

Part B3 marksannual

4

Balance the given redox equations by oxidation number method: (i) $HNO_3 + H_2S \rightarrow NO + S + H_2O$ (ii) $P + H_2O + HNO_3 \rightarrow H_3PO_4 + NO$.

Part C6 marksannual

5

The third line of Balmer series appears due to the transition of electron from:

MCQ1 marksannual

5

Calculate the number of molecules of $SO_2$ gas if its volume is $500\text{ cm}^3$ at S.T.P.

Part B3 marksannual

5

What is buffer solution? Write its types with composition. Explain buffer action when small amount of base is added in it.

Part C6 marksannual

6

Which of the following covalent bond has lowest bond energy?

MCQ1 marksannual

6

Why is CO₂ linear while H₂O is bent or V-shaped, although the atomicity of both molecules is the same?

Part B3 marksannual

6

What are colligative properties of solutions? Explain quantitative aspects of freezing point depression with general graphical representation to derive the molar mass of solute.

Part C6 marksannual

7

Shape of $PH_3$ molecule is:

MCQ1 marksannual

7

Calculate the number of molecules of $CO_2$ when $4.8 \times 10^{24}$ molecules of $CH_4$ reacts with excess of water according to the following reaction: $CH_4 + 2H_2O \rightarrow…

Part B3 marksannual

7

What are London dispersion forces? Explain any three factors which affect these forces with suitable example in each factor.

Part C7 marksannual

8

Which pair of gases diffuses with the same rate at same temperature and pressure?

MCQ1 marksannual

8

Draw the shapes of following molecules according to VSEPR theory: (i) $SO_2$ (ii) $H_2S$ (iii) $CBr_4$

Part B3 marksannual

8

Differentiate between cubic close packing and hexagonal close packing in metals. Also compare metallic solids with molecular solids in three ways.

Part C7 marksannual

9

Which of the following is **NOT** present in plasma?

MCQ1 marksannual

9

Briefly describe the following: (i) Line spectrum (ii) Stark effect (iii) Continuous spectrum

Part B3 marksannual

10

Which of the following processes is **NOT** endothermic?

MCQ1 marksannual

10

Distinguish between **Sigma** and **Pi bond** in three ways.

Part B3 marksannual

11

If crystallization of **NaCl** is carried out in the presence of urea then its shape will be:

MCQ1 marksannual

11

Calculate the average molar mass of air at sea level at $0^\circ C$, if density of air is $1.29\text{ kg/m}^3$.

Part B3 marksannual

12

The strong conjugate base among the given options is:

MCQ1 marksannual

12

Justify the following statements: (i) Petrol evaporates earlier than water (ii) Water has lower vapour pressure than ethyl alcohol.

Part B3 marksannual

13

A reaction will proceed in forward direction to maximum extent if value of $K_c$ is:

MCQ1 marksannual

13

What is the effect on the volume of gas if you simultaneously: (i) Its pressure is halved and its kelvin temperature is doubled (ii) Its pressure is doubled and its kelvin temperat…

Part B3 marksannual

14

For a reaction $A \rightarrow \text{Product}$, doubling the concentration of **A** quadruples the rate. The reaction is:

MCQ1 marksannual

14

Why heat of vaporization ($\Delta H_v$) is always greater than heat of fusion ($\Delta H_f$) for a substance?

Part B3 marksannual

15

Swelling of dead bones in water is due to:

MCQ1 marksannual

15

Calculate the numerical value of general gas constant **R** for one mole of gas at S.T.P: (i) In SI units (ii) Pressure in atm, volume in $dm^3$.

Part B3 marksannual

16

Which of the following is **NOT** a state function?

MCQ1 marksannual

16

Write any three characteristics of Plasma.

Part B3 marksannual

17

**Zn** acts as anode in Daniel cell but acts as cathode in Al-Zn cell because:

MCQ1 marksannual

17

Predict the shape of ZnS by using formula of radius ratio, if radius of Zn²⁺ is 74 pm and radius of S²⁻ is 184 pm.

Part B3 marksannual

18

If initial concentration of $N_2O_4$ in moles is **a** and **x** moles of it converted to $NO_2$, then derive the general relation of equilibrium constant ($K_c = \frac{4x^2}{V(a-x…

Part B3 marksannual

19

Calculate the value of $K_p$ at $1050^\circ C$ if $K_c$ is $2.3 \times 10^{22}$ for the following reaction: $2CO_{(g)} + O_{2(g)} \rightleftharpoons 2CO_{2(g)}$.

Part B3 marksannual

20

Write $K_{sp}$ expressions for following compounds: (i) $Ca_3(PO_4)_2$ (ii) $Na_2SO_4$.

Part B3 marksannual

21

What is levelling effect of water? How this effect is compensated?

Part B3 marksannual

22

Draw potential energy diagram for both exothermic and endothermic reactions according to collision theory.

Part B3 marksannual

23

Rate equation for given reaction is $R = K[NO]^2[H_2]$. Reaction occurs in two steps and oxygen atom is intermediate then write reaction mechanism: $2NO + 2H_2 \rightarrow N_2 + 2H…

Part B3 marksannual

24

How relative lowering of vapour pressure ($\frac{\Delta P}{P^\circ} = X_2$) can be used to calculate molar mass of solute?

Part B3 marksannual

25

Describe phenol water system and explain upper consulate temperature.

Part B3 marksannual

26

Write thermochemical equations from the given information: (i) Standard enthalpy of formation of $CaCO_3$ is $-1207\text{ kJ/mol}$ (ii) Standard enthalpy of combustion of $CH_3COOH…

Part B3 marksannual

27

Calculate $E^\circ_{\text{cell}}$ for Li-Zn cell and write cell reactions. $E^\circ_{\text{Li}}$ is $-3.05\text{ V}$ and $E^\circ_{\text{Zn}}$ is $-0.76\text{ V}$.

Part B3 marksannual

28

Write chemical reactions that occur at cathode and anode in alkaline dry cell.

Part B3 marksannual