FULL SYLLABUS CHEMISTRY TEST: 01
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NEET CHEMISTRY TEST 2026 [TEST 01]
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1. Which of the following is the INCORRECT order for the melting points of d-block elements?
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2. When lanthanoid(Ln) is heated with carbon, the carbide which is not formed is:
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3. The freezing point of a 5g CH₃COOH in 100 g water solution is ﹣1·576 ᴼC, the degree of dissociation of CH₃COOH is:
[Kf for water is 1·86 Kkgmol⁻¹]
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4. The ratio of wavelengths of last line of Lyman series to that of second line of Balmer series in hydrogen spectrum is:
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5. For the reaction: 4 Fe(s) + 3 O₂(g) ➝ 2 Fe₂O₃(s), if ΔᵣS = ﹣550 JK⁻¹mol⁻¹ and ΔᵣHᴼ = ﹣1650 kJ mol⁻¹, then total entropy change for the reaction will be:
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6. X & Y in the given reaction sequence are respectively:
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7. Arrange the compounds in the order of boiling point:
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8. The volume of ethanol (d = 1·15 g/mL) that has to be added to prepare 100 mL of 0·5 M ethanol solution in water is:
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9. Which of the following is not true about brown ring test?
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10. For a chemical reaction at 127 ᴼC, the activation energy is 600R. The ratio of rate constant at 327 ᴼC to that at 127 ᴼC will be
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11. A sample of 0·50 g of an organic compound was treated according to Kjeldahl’s method. The ammonia evolved was absorbed in 50 ml of 0·5 M H₂SO₄. The residual acid required 60 mL of 0·5 M solution of NaOH for neutralisation. What is the % composition of nitrogen in the compound?
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12. tert-Butylmethyl ether [(CH₃)₃C-O-CH₃] cannot be prepared by:
(1) CH₃ONa + (CH₃)₃CBr
(2) (CH₃)₂C=CH₂ + CH₃OH + H⁺
(3) (CH₃)₃CONa + CH₃Br
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13. At 25 ᴼC, if the solubility of Ag₂CrO₄ in 0·01 M Na₂CrO₄ solution be 5× 10⁻⁶ M then Ksp of Ag₂CrO₄ will be
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14. One mole of an ideal gas at 300 K in thermal contact with surroundings expands isothermally from 1·0 L to 2·0 L against a constant pressure of 3·0 atm, the change in entropy of the system would be:
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15. What volume of O₂(g), measures at 0 ᴼC & 1 atm, is required to completely burn 2 L of butane gas under similar conditions?
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16. Consider the following reversible reaction in a closed container:
N₂O₄(g) ⇌ 2 NO₂(g)
The amounts of N₂O₄ & NO₂ present at equilibrium is found to be 7·64 g & 1·56 g respectively in a 3·0 L closed container. What will be the value of Kc?
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17. High spin and low spin complexes are not possible with the configuration:
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18. A(l) having boiling point 210 ᴼC and B(l) having boiling point 90 ᴼC form an azeotropic mixture at certain composition. What should be the boiling point of the azeotrope if solution of A & B shows negative deviation from ideal behaviour?
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19. The product (B) in the following reaction sequence is:
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20. Which of the following is not true about brown ring test?
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21. The correct order for O-O bond length in the species is:
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22. For a zero-order reaction, which of the following is correct?
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23. In the following two reaction sequences products Ⓒ and Ⓓ can be distinguished by:
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24. Correct order for molar conductivity at infinite dilution is:
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25. The hybridisations of the central atom in the chemical species, ClF₃, BrF₅ & [ICl₂]⁺, are respectively
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26. Identify the major product (Y):
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27. Which of the following is not correct?
(1) La(OH)₂ is less basic than Lu(OH)₃
(2) Europium (z=63) has largest atomic radii among Lanthanoids.
(3) Lanthanoids can form carbides Ln₃C, Ln₂C₃ and LnC₂ when heated with carbon.
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28. If at 298K the bond energies of C–H, C–C, C=C and H – H bonds are respectively 414, 347, 615 and 435 kJ mol–1, then value of enthalpy change for the reaction,
H₂C=CH₂ + H₂(g) ➝ H₃C-CH₃(g)
at 298 K will be
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29. If Eᴼ for MnO₄⁻ ➝ Mn²⁺ is X₁ V and Eᴼ for MnO₄⁻ ➝ Mn⁴⁺ is X₂ V, then what will be Eᴼ for Mn⁴⁺ ➝ Mn²⁺?
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30. In the following reaction:
Mᴺ⁺ + MnO₄⁻ ➝ MO₃⁻ + Mn²⁺ + ½ O₂
If one mole of MnO₄⁻ oxidises 2·5 mole of Mᴺ⁺, then the value of N is:
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31. Number of mole of Cr₂O₇²⁻ required to oxidise 4 mole of ferrous oxalate in acidic medium is:
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32.
What is the configuration of the following compound?
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33. What should be the pH of 0.01M NaCl(aq) solution at 25ᴼC, if Kw for H₂O is 1·0 × 10⁻¹⁴ M²?
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34. Which one is INCORRECT order for the property indicated against it?
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35. If Kc = 3·92 × 10¹⁵, for the reaction:
Cu(s) + 2 Ag⁺(aq) ➝ Cu²⁺(aq) + 2 Ag(s).
What is the value of the Eᴼ for the reaction at 298 K?
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36. Which one of the following statements is INCORRECT?
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37. Choose the correct statement about K₂Cr₂O₇:
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38. In which of the following case osmotic pressure should be minimum?
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39. EMF of the cell
Zn(s) | Zn²⁺(0·01M) ‖ HCl(1M)| H₂(g, 1 atm)|Pt
At 298 K is 0·701 V. What is the minimum amount of NaOH required to neutralise the acid present in cathodic compartment completely? [Eᴼ(Zn²⁺➝ Zn) = 0·76 V]
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40. Which of the following is the Incorrect order for bond angle?
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41. Given:
NH₃(g) + 3 Cl₂ (g) ⇌ NCl₃(g) + 3 HCl(g); ΔH = ﹣X
N₂ (g) + 3 H₂ (g) ⇌ 2 NH₃(g); ΔH = ﹣Y
H₂ (g) + Cl₂ (g) ⇌ 2 HCl (g); ΔH = Z
The heat of formation of NCl₃ will be:
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42. The first four successive ionisation energy values for an element (A) are: x eV, 2x eV, 5x eV & 26x eV respectively. What should be the formula of its oxide?
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43. The major product ⓧ of the following reaction is:
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44. When 4 mole of A₂(g) and 2 mole of B₂(g) are taken in container of volume 1 L, following equilibriums established: A₂(g) + 2 B₂(g) ⇌ 3 C₂(g). If the mixture contains 1 mole of C₂(g) at equilibrium, then equilibrium constant will be:
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45. For which of the following conversion, there is no change in number of electronic exchange?
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FULL SYLLABUS CHEMISTRY TEST: 02
NEET CHEMISTRY TEST 2026 [TEST 02]
1. Identify the product (X) in the reaction:
2. Solution of A(l) [vp = 600 mmHg] and B(l) [vp = 800 mmHg] form ideal solution with certain composition. What should be the vapour pressure of the resulting solution?
3. Consider the following statements:
Choose the CORRECT statements:
4. Consider the following statements:
1. A chemical equilibrium is established when two exactly opposite reactions occur in the same container at the same time and with the same rates of reaction.
2. At equilibrium the concentrations of the chemical species become constant, but not necessarily equal.
3. Conjugate acid-base pairs differ only in a single H⁺; the one that has the extra H⁺ is the acid.
Choose the correct statements:
5. How many litres of water must be added to 1 L of an aqueous solution of HCl with pH of 1 to create an aqueous solution of pH of 3?
6. Choose the INCORRECT statement:
7. When 3-Iodo-2,2-dimethylbutane is treated with KOH in ethanol, three elimination products are formed, identify the major one:
8. How many stereogenic carbons are in the structure:
9. Number of phenols possible with molecular formula C₇H₈O is:
10. On increasing temperature from 27 ⁰C to 37 ⁰C, the rate of a chemical reaction becomes twice. What is the activation energy of the reaction?
11. If radius of second orbit of Be³⁺ is x Å, then what is the radius of 4ᵗʰ orbit of He⁺
12. Absolute value of which of the following thermodynamic property can be calculated?
13. For the chemical reaction:
2 CIO₂ (aq) + 20H⁻ (aq) ➝ CIO₂⁻(aq) + CIO₃⁻(aq) + H₂O(l).
The initial concentrations and rates of three experiments are given in the table. What is the rate law for this reaction?
14. When lead storage cell is full charged, aqueous solution of H₂SO₄ in it is 40% by mass. If specific gravity of this solution is 1·30, then what is the mass of pure H₂SO₄ in 100 mL of the solution?
15. A certain reaction is non spontaneous under standard conditions but becomes spontaneous at lower temperatures. What conclusions may be drawn under standard conditions?
Non spontaneous means ΔG > O. For a reaction to become spontaneous at lower temperature (ΔG < 0) means ΔH < 0 and ΔS < 0.
16. Benzene is treated with excess of CH₃Cl + AlCl₃ to give salt of benzene derivative having formula C₁₃H₂₁AlCl₄. How many moles of CH₃Cl are consumed per mole of benzene?
17. A swimmer coming out from a pool is covered with a film of water weighing about 18g. How much heat must be used at constant volume to evaporate this water at 298 K? ΔvapHᴼ(H₂O) = 44·01 kJ mol⁻¹.
18. A black compound of manganese reacts with a halogen acid to give greenish yellow gas. When excess of this gas reacts with NH₃ an unstable trihalide is formed. In this process the oxidation state of nitrogen changes from
19. For the chemical reaction: A + B ➝ Product, the rate law is K [A]¹ × [B]¹. K = 5×10⁻³ L mol⁻¹s⁻¹, what is the concentration of ‘A’ remaining after 100 second if [A]₀ = 0·10 M & [B]₀ = 6 M? [log 20 = 1·3]
Since [B]₀ >> [A]₀
R = K’ [A], [K’ = K×[B]₀]
∴ K’ = (2·303/t) × log (C₁/C₂)
i.e., 5 × 10⁻³ × 6 = (2·303/100) × log(0·1/C₂)
On solving, C₂ = 5 × 10⁻³ M
20. Electron gain enthalpies (in kJ mol⁻¹) of Cl(g) and F(g) are respectively:
21. A 2·250 g sample of a dicarboxylic acid having molecular mass 174 u was burnt in an excess of oxygen and yielded 4·548 g of CO₂ and 1·629 g of H₂O. What should be the molecular formula of the compound?
22. When hydrated ferric chloride is dissolved in aqueous solution of oxalic acid containing KOH, green crystals is obtained having formula
FeCl₃ + 6 KOH + 3 H₂C₂O₄ ➝ K₃[Fe(C₂O₄)₃] + 3 KCl + 6 H₂O
23. If bond dissociation energies for H-H, O=O and O-H bonds are respectively: 436, 499 and 464 kJ/mol, then what will be the enthalpy change for the reaction:
2 H₂(g) + O₂(g) ➝ 2 H₂O(l) ?
24. An aqueous solution containing 3 g of a non volatile solute of molar mass 111.6 g/mol in 500 g of water freezes at - 0.125 °C. The mass of ice separated out in grams from the solution is (Kf = 1.86 K kg mol⁻¹)
25. An aromatic compound ‘A’ on treatment with aqueous ammonia and heating forms compound ‘B’ which on heating with Br₂ and KOH forms a compound ‘C’ of molecular formula C₆H₇N. What is the IUPAC name of B?
26. What is the correct IUPAC name of the structure given?
27. Consider the following statements about plot of Intensity versus wavelength during black body radiation at various temperatures:
Choose the CORRECT statement
28. Based on CFT, which one of the following ions should be colourless?
29. What is the EMF of the cell: Al(s) | Al³⁺(0.01 M) || Fe²⁺(0.1 M) | Fe(s)? [Given Eᵒ(Al³⁺/Al) = -1.66 V and Eᵒ(Fe²⁺/Fe) = -0.45 V]
30. Which of the following reactions will yield propan-2-ol?
I. Acid catalysed hydration of propene.
II. Reaction of ethanal with CH₃MgI followed by hydrolysis
III. Reaction of methanal with C₂H₅MgI followed by hydrolysis
IV. Oxidation of propene with neutral KMnO₄
31. Organic Compound A C₈H₈O gives 2,4-DNP and Iodoform test but does not reduce Tollens and Fehlings reagent neither decolorises Baeyer's reagent. On drastic Oxidation with H₂CrO₄ it gives B (C₇H₆O₂). A and B are respectively
32. What will be the work done in isothermal reversible compression of a gas having initial pressure & volume (10 atm & 20 L) to final pressure & volume (20 atm & 10 L)?
33. Bond order in CO and oxidation number of carbon in it, are respectively:
34. At 518 °C, the rate of decomposition of a sample of gaseous acetaldehyde, initially at a pressure of 363 Torr, was 1.00 Torr/s when 5% had reacted and 0.5 Torr/s when 33% had reacted. The order of the reaction is
35. For the redox reaction:
x MnO₄⁻ + y C₂O₄²⁻ + z H⁺ ➝ Mn²⁺ + CO₂ + H₂O, x, y and z for the balanced reaction are
36. When 50·0 mL of 0·10 M Fe(NO₃)₂ solution is mixed with 50·0 mL of 0·10 M KOH, a green precipitate is formed and the concentration of hydroxide ion becomes very small. Which of the following is the correct order of the concentrations of the remaining ions in the solution?
The hydroxide is low because it combined with some of the iron, so Fe²⁺ will be low. There is no other ion that the hydroxide ion could combine with to form a precipitate. The nitrate is double the potassium because there are two moles of nitrate per mole of iron(II) nitrate instead of one ion per mole, as in potassium hydroxide.
37. Which of the following ion has zero spin only magnetic moment?
38. Which of the following statements are correct about :C≡O: molecule?
39. Identify the pair of linear molecules:
40. The chemical species having two π-bonds and ½ σ-bond is:
41. A hydrocarbon X is optically active. X upon hydrogenation gives an optically inactive alkane Y. X is
42. When the Intermediate complex of Balz-Schiemann reaction heated in NaNO₂ with Cu forms
43. The incorrect order among the following is:
44. Consider the following statements:
45. What is the relation between compounds A and B?
The average score is 6%
FULL SYLLABUS CHEMISTRY TEST: 03
NEET CHEMISTRY TEST 2026 [TEST 03]
1. Increasing order of reactivity of the following compounds for SN1 substitution is:
2. A bottle of H₃PO₄ solution contains 70%(w/w) acid. If the density of the solution is 1·54 g cm⁻³, the volume of the H₃PO₄ solution required to prepare 1 L of I N solution is
3. 2 g of a metal oxide MxOy reduced to 0·99 g of the metal. If the atomic mass of the metal is 55 g mol⁻¹, x and y are respectively:
4. The reaction aA(g) ⇌ bB(g) + cC(g) was carried out at a certain temperature with an initial pressure of A = 30 bar. Initially ‘B’ and ‘C’ were not present. If the equilibrium partial pressures of ‘A’, ‘B’ and ‘C’ are 20, 5 and 10 bar respectively, then a:b:c is
5. An electron present in the third excited state of a H atom returns of the first excited state and then to the ground state. If λ₁ and λ₂ are the wavelengths of light emitted in these two transitions respectively, λ₁:λ₂ is
6. O₂(g) is paramagnetic in nature because it has
7. Carbon suboxide (C₃O₂), has a linear structure. Which of the following is correct about C₃O₂?
I. Oxidation state of all three C atoms is +2.
II. Oxidation state of the central C atom is zero.
III. The molecule contains 4 σ and 4 π bonds.
IV. Hybridization of the central carbon atom is sp²
8. Three elements X, Y and Z are in the 3rd period of the periodic table. The oxides of X, Y and Z, respectively, are basic, amphoteric and acidic. The correct order of the atomic numbers of X, Y and Z is:
9. The process in which an ideal gas undergoes change from X to Y as shown in the following diagram is
10. The mass ratio of steam and hydrogen is found to be 1:1·5 at equilibrium in the following reaction:
3 Fe(s) + 4 H₂O (g) ⇌ Fe₃O₄(s) + 4 H₂(g)
The value of the equilibrium constant (Kc) of the above reaction is
11. Among the following maximum number of resonating structures are possible for
12. NO₂ required for a reaction is produced by the decomposition of N₂O₅ in CCl₄ as per the equation:
2 N₂O₅ (g) ➝ 4 NO₂ (g) + O₂ (g)
The initial concentration of N₂O₅ is 3.00 mol L⁻¹ and it is 2.75 mol L⁻¹ after 30 minutes.
The rate of formation of NO₂ is :
13. Energy of electron in 2ⁿᵈ orbit of Be³⁺ is ﹣x eV atom⁻¹, what is the energy of electron in 4ᵗʰ orbit of He⁺?
14. A solution is prepared by dissolving 0·6 g of urea (molar mass = 60 g mol⁻¹) and 1.8 g of glucose (molar mass = 180 g mol⁻¹) in 100 mL of water at 27 ⁰C. The osmotic pressure of the solution is :
(R = 0.08206 L atm K⁻¹ mol⁻¹)
15. 25 g of an unknown hydrocarbon upon burning produces 88 g of CO₂ and 9 g of H₂O. This unknown hydrocarbon contains.
16. When 1 L of 0·1 M H₂SO₄ solution is allowed to react with 1 L of 0·1 M sodium hydroxide solution, the amount of Na₂SO₄ (anhydrous) that can be obtained from the solution formed and the concentration of H+ in the solution respectively are
17. Among the statements (a - d), the incorrect ones are:
(a) Octahedral Co(III) complexes with strong field ligands have very high magnetic moments
(b) When Δ₀ < P, the d-electron configuration of Co(III) in an octahedral complex is (t₂g)⁴(eg)²
(c) Wavelength of light absorbed by [Co(en)₃]³⁺ is lower than that of [CoF₆]³⁻
(d) If the Δₒ for an octahedral complex of Co(III) is 18,000cm⁻¹, the Δt for its tetrahedral complex with the same ligand will be 16,000 cm⁻¹.
18. A current of 5.0 A flows for 4.0 h through an electrolytic cell containing a molten salt of metal M. This results in deposition of 0.25 mol of the metal M at the cathode. The oxidation state of M in the molten salt is (1 Faraday = 96485 C mol⁻¹)
19. A sample of a gas was analysed and found to contain 2·34 g of nitrogen and 5·34 g of oxygen. The vapour density of the gas was found to be about 45·9. What is the molecular formulas of this gas?
20. Gas phase reactions (i) and (ii) are of first and second order respectively
2N₂O₅ (g) ➝ 4NO₂ (g) + O₂ (g) ...................... (i)
2NO(g) + O₂(g) ➝ 2NO₂(g). ....................... (ii)
Under certain conditions, the rate constants (k₁, k₂) of (i) and (ii) respectively, have the same numerical value, when the concentrations of the reactants are expressed in mol/dm³.
If the concentrations are expressed in mol/mL, the correct relationship between k₁ and k₂ is
21. Among the following, the correct statement/s about ‘p’ block elements is/are
I. The valence shell electronic configuration of all of them is ns²np¹⁻⁶, where n=1,2,3. . .
II. Only in p block, metals, nonmetals and metalloids are present.
III. Halogens have the lowest negative electron gain enthalpy in the respective periods.
IV. Noble gases have no tendency to accept an electron and hence they have large negative values of electron gain enthalpy.
22. If Ni²⁺ ion is replaced with Pt²⁺ ion in complex [NiCl₂Br₂], which of the following would change:
23. The correct statements among I to III are:
I. Valence bond theory cannot explain the color exhibited by transition metal complexes
II. Valence bond theory can predict quantitatively the magnetic properties of transition metal complexes
III. Valence bond theory cannot distinguish ligands as weak and strong field ones
24. The kinetic energy of the photoelectrons ejected by a metal surface increased from 0.6 eV to 0.9 eV when the energy of the incident photons was increased by 20%. The work function of the metal is
25. The ammonia(NH₃) released on quantitative reaction of 0.6 g urea (NH₂CONH₂) with sodium hydroxide(NaOH) can be neutralized by
26. The C–C bond length is maximum in
27. The theory that can completely/properly explain the nature of bonding in [Ni(CO)₄] is
28. The correct order of the following compounds towards addition of HCN is:
29. Two solutions A and B, each of 100 L was made by dissolution of 4g of NaOH and 9.8 g of H₂SO₄ in water, respectively. The pH of the resultant solution obtained from mixing 40 L of solution A and 10 L of solution B is
30. An organic compound 'A' (C4H10) when treated with conc. HI undergoes, cleavage yield compound 'B' and C'. ‘B' gives yellow precipitate with AgNO₃ where as tautomerizes to 'D'. 'D' gives positive iodoform test. 'A' could be:
31. A balance having a precision of 0.001 g was used to measure a mass of a sample of about 15g. The number of significant figures to be reported in this measurement is
32. HF has highest boiling point among hydrogen halides, because it has:
33. The qualitative plots given represent the yield of the product, [XY], at equilibrium in the reaction X(g) + Y(g) ⇌ XY(g), as a function of temperature, at total pressures P₁ and P₂. The reaction is
34. The solubility products (Ksp) for three salts MX, MY₂ and MZ₃ are 1 × 10⁻⁸, 4 × 10⁻⁹ and 27 × 10⁻⁸, respectively. The correct order for solubilities of these salts is
35. The order of electron gain enthalpy in kJ/mol of fluorine, chlorine, bromine and iodine, respectively are
36. If azimuthal quantum number (l) of an electron in an orbital is 2, the shape of the orbital should be
37. The vapour pressures of pure liquids A and B are 400 and 600 mm Hg, respectively at 298 K. On mixing the two liquids, the sum of their initial volumes is equal to the volume of the final mixture. The mole fraction of liquid B is 0.5 in the mixture. The vapour pressure of the final solution, the mole fractions of components A and B in vapour phase, respectively are:
38. The vapour pressure of benzene is 53.3 kPa at 60.6 ∞C, but it fall to 51.5 kPa when 19 g of a nonvolatile organic compound is dissolved in 500 g benzene. The molar mass of the nonvolatile compound is [assume dilute solution]
39. In order to oxidize a mixture of one mole of each of FeC₂O₄, Fe₂(C₂O₄)₃, FeSO₄ and Fe₂(SO₄)₃ in acidic medium, the number of moles of KMnO₄ required is:
40. The decreasing order of electrical conductivity of the following aqueous solutions is:
1. 0.1 M Formic acid
2. 0.1 M Acetic acid
3. 0.1 M Benzoic acid
41. What would be the molality of 20% (mass/mass) aqueous solution of KI? (molar mass of KI = 166 g mol⁻¹)
42. What is the product of following reaction?
43. A₂(g) + 4 B₂(g) ⇌ 2 AB₄(g), ΔH < 0
Product formation is favoured by
44. The ratio of the mass percentages of 'C & H' and 'C & O' of a saturated acyclic organic compound 'X' are 4 : 1 and 3 : 4 respectively. Then, the moles of oxygen gas required for complete combustion of two moles of organic compound 'X' is
45. The number of possible optical isomers for the complexes MA₂B₂ with sp³ and dsp² hybridized metal atom, respectively is:
[Note: A and B are uni-dentate neutral and uni-dentate mono-anionic ligands, respectively]
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