NEET WEEKLY TEST CHEMISTRY (SDA AND CHANMARI) (12.09.2026)

1. On increasing the pressure, the direction in which the gas phase reaction proceeds to re-establish equilibrium is predicted by applying Le-Chatelier’s principle. Consider the reaction:

Which of the following is correct, if the total pressure at which the equilibrium is established is increased without changing the temperature?

3. For the equilibrium A ⇌ B, the variation of the rate of the forward (a) and reverse (b) reaction with time is given by: Answer – (ii)

4. Which is not a conjugate acid/base pair?

1. H₂CO₃ and CO₃²⁻
2. HSO₄⁻ and SO₄²⁻
3. H₂PO₄⁻ and HPO₄²⁻
4. H₃O⁺ and H₂O

5. Glucose and Fructose react with an excess of Phenylhydrazine to yield the exact same Osazone derivative because:

1. C-1 and C-2 are involved in osazone formation, while C-3, C-4, C-5, C-6 have identical configurations
2. Both Glucose and Fructose have identical molecular weights
3. Phenylhydrazine converts Fructose into Glucose completely prior to reaction
4. Osazone formation eliminates all chiral centers in the molecule

6. For the reaction A + 3B ⇌ 2C + D, initial mole of A is twice that of B. If at equilibrium moles of B and C are equal, then percent of B reacted is:

1. 10%
2. 20%
3. 40%
4. 60%

7. Assertion (A): α-D-Glucose and β-D-Glucose show the phenomenon of mutarotation in aqueous solution.
   Reason (R): In aqueous solution, both anomers open up into the open-chain form, establishing a dynamic equilibrium between α, open-chain, and β forms.

1. Both A and R are true, and R is correct explanation of A
2. Both A and R are true, but R is not the correct explanation
3. A is true but R is false
4. A is false but R is true

8. If K₁ and K₂ are the respective equilibrium constants for the two reactions,
XeF₆(g) + H₂O(g) ⇌ XeOF₄(g) + 2HF(g)
XeO₄(g) + XeF₆(g) ⇌ XeOF₄(g) + XeO₃F₂(g)
The equilibrium constant of the reaction,
XeO₄(g) + 2HF(g) ⇌ XeO₃F₂(g) + H₂O(g)
will be:

1. K₁/(K₂)²
2. K₁·K₂
3. K₁/K₂
4. K₂/K₁

9. Fructose is an example of a/an:

1. Aldohexose
2. Ketohexose
3. Aldopentose
4. Ketopentose

10. For the reaction,
CH₄(g) + 2O₂(g) ⇌ CO₂(g) + 2H₂O(l), ΔᵣH = −170.8 kJ mol⁻¹
Which of the following statement is not true?

1. At equilibrium, the concentrations of CO₂(g) and H₂O(l) are not equal.
2. The equilibrium constant for the reaction is given by Kₚ = [CO₂]/[CH₄][O₂].
3. Addition of CH₄(g) or O₂(g) at equilibrium will cause a shift to the right.
4. The reaction is exothermic.

11. A carbohydrate that cannot be hydrolyzed further into simpler polyhydroxy aldehydes or ketones is called a:

1. Monosaccharide
2. Disaccharide
3. Oligosaccharide
4. Polysaccharide

12. Ionisation constant of CH₃COOH is 1.7 × 10⁻⁵ and concentration of H⁺ ions is 3.4 × 10⁻⁴. Then, find out initial concentration of CH₃COOH molecules.

1. 3.4 × 10⁻⁴
2. 3.4 × 10⁻³
3. 6.8 × 10⁻⁴
4. 6.8 × 10⁻³

13. Assertion (A): Fructose has ketonic group yet it reduces Tollen’s reagent.
    Reason (R): Formation of enediol intermediate by fructose in alkaline medium converts it partially into glucose and mannose.

1. Both A and R are true, and R is correct explanation of A
2. Both A and R are true, but R is NOT the correct explanation
3. A is true but R is false
4. A is false but R is true

14. Consider the following reaction in a sealed vessel at equilibrium with concentrations of N₂ = 3.0 × 10⁻³ M, O₂ = 4.2 × 10⁻³ M and NO = 2.8 × 10⁻³ M.
2NO(g) ⇌ N₂(g) + O₂(g)
If 0.1 mol L⁻¹ of NO(g) is taken in a closed vessel, what will be degree of dissociation (α) of NO(g) at equilibrium?

1. 0.00889
2. 0.0889
3. 0.8889
4. 0.717

15. Natural D-Glucose is dextrorotatory, represented by:

1. D-(-)-Glucose
2. D-(+)-Glucose
3. L-(+)-Glucose
4. L-(-)-Glucose

16. The value of Kc of the reaction 2A ⇌ B + C is 2 × 10⁻³. At a given time, the composition of the reaction mixture is [A] = [B] = [C] = 3 × 10⁻⁴ M. Select the correct option:

1. Qc < Kc
2. Qc > Kc
3. Qc = Kc
4. Qc ≠ Kc

17. Glucose on reaction with Hydroxylamine (NH2OH) forms an oxime, which confirms the presence of:

1. Five -OH groups
2. A carbonyl group
3. Primary alcoholic group
4. Straight chain of 6 carbon atoms

18. Which of the following cannot act both as a Bronsted acid and as a Bronsted base?

1. HCO₃⁻
2. NH₃
3. HCl
4. HSO₄⁻

19. Match the Carbohydrate in Column-I with its description in Column-II:


1. P-3, Q-4, R-1, S-2
2. P-4, Q-3, R-2, S-1
3. P-3, Q-1, R-4, S-2
4. P-1, Q-4, R-3, S-2

20. For the given reaction, the degree of dissociation of B was found to be 20% at 300 K and 24% at 500 K.
A(s) + B(g) ⇌ C(g) + 2D(s) + E(s)
The rate of backward reaction:

1. Increases with increase in pressure and temperature.
2. Increases with increase in pressure and decrease in temperature.
3. Depends on temperature only and decreases with increase in temperature.
4. Increases with increase in concentration of B and increase in the temperature.

21. Fructose contains which functional group in its open-chain form?

1. Aldehyde group at C-1
2. Keto group at C-2
3. Keto group at C-1
4. Aldehyde group at C-2

22. Which of the following reactions satisfies the condition Kₚ > Kc?

1. H₂(g) + I₂(g) → 2HI(g)
2. N₂(g) + 3H₂(g) → 2NH₃(g)
3. 2SO₃(g) → 2SO₂(g) + O₂(g)
4. PCl₃(g) + Cl₂(g) → PCl₅(g)

23. Which of the following options has the lowest degree of ionisation?

1. 0001 M CH₃COOH
2. 001 M CH₃COOH
3. 01 M CH₃COOH
4. 1 M CH₃COOH

24. Glucose on prolonged heating with HI forms:

1. Gluconic acid
2. n-Hexane
3. Saccharic acid
4. Hexanoic acid

25. An acid/base dissociation equilibrium is dynamic involving a transfer of proton in forward and reverse directions. Now, with passage of time in which direction equilibrium is favoured?

1. in the direction of stronger base and stronger acid
2. in the direction of formation of stronger base and weaker acid
3. in the direction of formation of weaker base and weaker acid
4. in the direction of formation of weaker base and stronger acid

26. Arrange the hybridization states of carbon in decreasing order of electronegativity:

1. sp > sp² > sp³
2. sp³ > sp² > sp
3. sp² > sp > sp³
4. sp > sp³ > sp²

27. Given:
HF + H₂O ⇌ H₃O⁺ + F⁻ (K_a)
F⁻ + H₂O ⇌ HF + OH⁻ (K_b)
Which of the following relation is correct?

1. K_b = K_w
2. K_b = 1/Kₐ
3. Kₐ × K_b = K_w
4. Kₐ/K_b = K_w

28. Which of the following process is endothermic in nature?
1. O(g) + e- -> O^–(g)
2. O^‑(g) + e- -> O^2-(g)
3. Cl(g) + e- -> Cl^–(g)
4. F(g) + e- -> F^–(g)

29. Which one of the following information can be obtained on the basis of Le Chatelier principle?

1. Dissociation constant of a weak acid
2. Entropy change in a reaction
3. Equilibrium constant of a chemical reaction
4. Shift in equilibrium position on changing value of a constraint

30. Why is the electron gain enthalpy of noble gases positive?

1. High effective nuclear charge
2. Stable fully filled electronic configurations
3. Large atomic radii
4. High shielding effect

31. According to Le-Chatelier’s principle, adding heat to a solid ⇌ liquid equilibrium will cause the:

1. temperature to increase
2. temperature to decrease
3. amount of liquid to decrease
4. amount of solid to decrease

31. Assertion (A): Non-metallic character increases across a period from left to right.
     Reason (R): Effective nuclear charge increases across a period, making electron gain easier and electron removal harder.

1. Both A and R are true, and R is correct explanation of A
2. Both A and R are true, but R is NOT the correct explanation
3. A is true but R is false
4. A is false but R is true

32. If Kc is in the range of ………… appreciable concentrations of both reactants and products are present.

1. 10⁻⁴ to 10⁴
2. 10⁻³ to 10³
3. 10³ to 10⁶
4. 10⁻⁵ to 10³

34. Which halogen has the highest electronegativity?

1. F
2. Cl
3. Br
4. I

35. The reaction quotient (Q) for the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g) is given by Q = [NH₃]²/([N₂][H₂]³). The reaction will proceed from right to left if:

1. Q = 0
2. Q = Kc
3. Q < Kc
4. Q > Kc

36. Why does Lithium chloride show significant covalent character, unlike NaCl which is predominantly ionic?

1. Small size of Li+ cation exerts high polarizing power on Cl-
2. Lithium has higher electron gain enthalpy
3. NaCl has higher lattice energy
4. Sodium is more non-metallic than Lithium

37. On doubling P and V with constant temperature the equilibrium constant will:

1. remain constant
2. become double
3. become one-fourth
4. None of these

38. Reaction of Glucose with bromine water (Br₂/H₂O) yields:

1. Saccharic acid
2. Gluconic acid
3. Sorbitol
4. n-Hexane

39. The equilibrium constants for the reactions at 100 K are:
CoO(s) + H₂(g) ⇌ Co(s) + H₂O(g); K₁ = 65
CoO(s) + CO(g) ⇌ Co(s) + CO₂(g); K₂ = 500
The equilibrium constant for the reaction CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g) at 100 K is:

1. 0.13
2. 7.69
3. 0.0179
4.69.3

40. Why does Oxygen have less negative electron gain enthalpy than Sulphur?

1. Compact 2p subshell leading to electron repulsion
2. High ionization enthalpy of Oxygen
3. Absence of d-orbitals in Oxygen
4. Lower electronegativity of Oxygen

41. The values of Kc for the following reactions are given as: A ⇌ B, Kc = 1; B ⇌ C, Kc = 3; and C ⇌ D, Kc = 5. Evaluate the value of Kc for A ⇌

1. 15
2. 5
3. 3
4. 1

42. Across a period from left to right, non-metallic character generally:

1. Decreases
2. Increases
3. Remains constant
4. First decreases then increases

43. For the reaction N₂O₄(g) ⇌ 2NO₂(g), Kₚ is found to be equal to Kc. This is attained at:

1. 0°C
2. 273 K
3. 1 K
4. 12.19 K

44. Which of the following elements exhibits the highest metallic character in Period 3?

1. Sodium
2. Magnesium
3. Aluminum
4. Silicon

45. Lithium shows diagonal relationship with which element of the third period?

1. Beryllium
2. Magnesium
3. Aluminum
4. Silicon