FULL SYLLABUS CHEMISTRY TEST: 01
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NEET CHEMISTRY TEST 2026 [TEST 01]
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1. The hybridisations of the central atom in the chemical species, ClF₃, BrF₅ & [ICl₂]⁺, are respectively
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2. Which one of the following statements is INCORRECT?
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3.
Consider the structure of dimer of AlCl₃. The correct orders for bond parameters
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4. Among the following compounds, the one(s) that gives(give) effervescence with aq. NaHCO₃ solution is (are):
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5. 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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6. The functional group which is not present in the given structure is:
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7. Identify the major product (Y):
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8. What is the value of EMF of the cell at 298 K:
Pt|Fe²⁺(0·01 M), Fe³⁺(0·02 M) ‖ Ag⁺(1·0 M)|Ag(s)?
Given: E⁰(Ag⁺ ➝ Ag) = 0·80 V, and E⁰(Fe³⁺ ➝ Fe²⁺) = 0·77 V
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9. The major product ⓧ of the following reaction is:
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10. The bond dissociation enthalpies for the nitrogen–nitrogen bond in N₂ and [N₂]⁻ are respectively:
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11. 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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12. Which of the following is/are non reducing sugar(s)?
I. Fructose
II. Maltose
III. Sucrose
IV. Lactose
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13. Correct order for molar conductivity at infinite dilution is:
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14. For the equilibrium:
CaCO₃(s) ⇌ CaO (s) + CO₂(g); Kp = 1·64 atm at 1000 K. 50 g of CaCO₃ in a 10 L closed vessel is heated to 1000 K. Percentage of CaCO₃ that remains unreacted at equilibrium is [R = 0·082 L atm K⁻¹mol⁻¹]
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15. Which of the following is the composition of sucrose?
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16. In the following two reaction sequences products Ⓒ and Ⓓ can be distinguished by:
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17. A rocket fuel contains two liquids hydrazine (N₂H₄) and dinitrogen tetraoxide (N₂O₄) which ignite on contact to form N₂(g) and water vapour. How many grams of N₂(g) form when 1·00 × 10² g of N₂H₄ and N₂O₄ are mixed?
\(2 N_2 H_4 (l) + N_2O_4 (l) \longrightarrow 3 N_2(g) + 4 H_2O (g)\)
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18. Given equivalent conductivities at 298 K:
λᴼ for Ba(OH)₂ = 228·8 Ω⁻¹ cm² mol⁻¹
λᴼ for BaCl₂ = 120·3 Ω⁻¹ cm² mol⁻¹
λᴼ for NH₄Cl = 129·8 Ω⁻¹ cm² mol⁻¹
And equivalent conductivity of 0·2 N NH₄OH solution is 2·383 Ω⁻¹ cm² mol⁻¹, then the value of % degree of dissociation of NH₄OH will be nearly:
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19. High spin and low spin complexes are not possible with the configuration:
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20. What is the entropy change of 1 mole sample of perfect gas when it expands isothermally so that its volume doubles?
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21. The product (B) in the following reaction sequence is:
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22. Choose the correct statement about K₂Cr₂O₇:
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23. 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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24. 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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25. Choose the INCORRECT statement:
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26. For which of the following acid base titration no indicator is available?
For titration of weak acid and weak base there is no indicator.
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27. 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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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. For which of the following conversion, there is no change in number of electronic exchange?
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30. Arrange the compounds in the order of boiling point:
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31. Consider the formation of PCl₃:
P₄(s) + 6 Cl₂ (g) ➝ 4 PCl₃(l)
What is the maximum mass of PCl₃ that can be obtained from 125 g P₄ and 323 g Cl₂? [P = 31, Cl = 35·5]
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32. Which of the following is the Incorrect order for bond angle?
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33. 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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34. 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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35. 0·1568 g of Fe is converted to Fe²⁺(aq) and requires 26·24 mL of a KMnO₄(aq) solution for its titration in acidic medium. What is the molarity of the KmnO₄(aq) solution?
5 Fe²⁺(aq) + MnO₄⁻(aq) + 8 H⁺ ➝ 5 Fe³⁺ + Mn²⁺(aq) + 4 H₂O(l)
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36. X & Y in the given reaction sequence are respectively:
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37. When lanthanoid(Ln) is heated with carbon, the carbide which is not formed is:
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38. 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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39. 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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40. Number of mole of Cr₂O₇²⁻ required to oxidise 4 mole of ferrous oxalate in acidic medium is:
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41. 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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42. 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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43. The correct order for the wavelengths of absorption for the following is
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44. Which of the following is the INCORRECT order for the melting points of d-block elements?
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45. Arrange the compounds (A to E) in the order of solubility in hexane:
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FULL SYLLABUS CHEMISTRY TEST: 02
NEET CHEMISTRY TEST 2026 [TEST 02]
1. 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
2. Choose the INCORRECT statement:
3. 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
4. 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
5. Absolute value of which of the following thermodynamic property can be calculated?
6. 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]
7. A microscope using suitable photons is employed to locate an electron in an atom within a distance of 0·1 Å. What is the uncertainty involved in the measurement of its velocity?
8. Choose CORRECT Statement:
I. In graphite distance between two layers is 340pm.
II. Graphite conducts electricity between layers.
III. Graphite is very soft and slippery.
9. The chemical species having two π-bonds and ½ σ-bond is:
10. When 3-Iodo-2,2-dimethylbutane is treated with KOH in ethanol, three elimination products are formed, identify the major one:
11. A hydrocarbon X is optically active. X upon hydrogenation gives an optically inactive alkane Y. X is
12. 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?
13. 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)
14. 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) ?
15. Consider the following statements:
16. 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?
17. What is the correct IUPAC name of the structure given?
18. What is the relation between compounds A and B?
19. 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
20. 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?
21. Identify the pair of linear molecules:
22. When the Intermediate complex of Balz-Schiemann reaction heated in NaNO₂ with Cu forms
23. The incorrect order among the following is:
24. 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.
25. Consider the following statements:
Choose the CORRECT statements:
26. 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?
27. Which of the following ion has zero spin only magnetic moment?
28. Identify the product (X) in the reaction:
29. What is the minimum volume of water required to dissolve 1 g of CaSO₄ at 298 K? [Ksp(CaSO₄) at 298 K = 9 × 10⁻⁶]
S = 3 × 10⁻³ mol/L = 136 × 3 × 10⁻³ g/L = 0·408 g/L
∴ For 1 g CaSO₄ to be dissolved, 2·45 L of water will be required.
30. Consider the following statements:
31. If 1 g NaOH is added to 200 mL of 2·5 M solution of NaOH(aq), then what is the molarity of the resulting solution?
32. Number of phenols possible with molecular formula C₇H₈O is:
33. Sample solutions of each of the three acids (given in figure) were titrated with 0.10 M NaOH(aq). Each of the acid solutions had a concentration of 0.10 M. Which of the acid titrations had the highest pH at the endpoint?
The weakest acid (smallest Kₐ) will have the highest pH at the endpoint.
34. 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?
35. What is the average formal charge on each oxygen in [NO₃]⁻?
36. Electron gain enthalpies (in kJ mol⁻¹) of Cl(g) and F(g) are respectively:
37. If a solution of diethyl ether, (C₂H₅)₂O, in ethanol, C₂H₅OH, is treated as an ideal solution, what is the mole fraction of diethyl ether in the vapour over an equimolar solution of these two liquids at 20 ⁰C?
[P⁰(diethyl ether) = 480 mm Hg & P⁰(ethanol) = 50 mm Hg at 20⁰C.]
38. 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?
39. 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?
40. 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?
41. Which of the following pair of compounds are polar?
42. Which of the following tests are given positive by both aldehydes and ketones?
43. 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.
44. How many stereogenic carbons are in the structure:
45. The carbocation in which rearrangement is not feasible?
The average score is 6%
FULL SYLLABUS CHEMISTRY TEST: 03
NEET CHEMISTRY TEST 2026 [TEST 03]
1. The process in which an ideal gas undergoes change from X to Y as shown in the following diagram is
2. 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.
3. 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:
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. Consider the following reaction:
[CoCl₂(NH₃)₄]⁺ + Cl⁻ ➝ [CoCl₃(NH₃)₃] + NH₃.
Which of the following statements are correct:
6. Increasing order of reactivity of the following compounds for SN1 substitution is:
7. If azimuthal quantum number (l) of an electron in an orbital is 2, the shape of the orbital should be
8. The emf of a cell corresponding to the following reaction is 0·199 V at 298 K.
Zn(s) + 2 H⁺ (aq) ➝ Zn²⁺(0·1 M) + H₂(g); (E⁰(Zn/Zn²⁺) = 0·76 V)
The approximate pH of the solution at the electrode where hydrogen is being produced is
9. 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
10. The correct order of the following compounds towards addition of HCN is:
11. 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.
12. 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
13. 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]
14. 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
15. A chemical reaction is carried out at two different temperatures T₁ and T₂ (T₂ > T₁) and also with and without a catalyst.
The statement that is correct among the following is
16. For the reaction 2A + B ➝ C, the values of initial rate at different reactant concentrations are given in the table below: The rate law for the reaction is:
17. The hydrocarbon that cannot be prepared effectively by Wurtz reaction is
18. The ammonia(NH₃) released on quantitative reaction of 0.6 g urea (NH₂CONH₂) with sodium hydroxide(NaOH) can be neutralized by
19. Energy of electron in 2ⁿᵈ orbit of Be³⁺ is ﹣x eV atom⁻¹, what is the energy of electron in 4ᵗʰ orbit of He⁺?
20. The order of electron gain enthalpy in kJ/mol of fluorine, chlorine, bromine and iodine, respectively are
21. Which of the following metal will exhibit photoelectric effect with photon having longest wavelength?
22. Among the following maximum number of resonating structures are possible for
23. 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:
24. The quantum number of four electrons are given below:
I. n = 4, l = 2, m = 2, s = ﹣½
II. n = 3, l = 2, m = 1, s = + ½
III. n = 4, l = 1, m = 0, s = + ½
IV. n = 3, l = 1, m = 1, s = ﹣½
The correct order of their increasing energies will be:
25. What would be the molality of 20% (mass/mass) aqueous solution of KI? (molar mass of KI = 166 g mol⁻¹)
26. In H-atom if electron absorbs a photon of 1·89 eV, then transition of electron is from
27. The best sequence of reactions for the following conversion is
28. A₂(g) + 4 B₂(g) ⇌ 2 AB₄(g), ΔH < 0
Product formation is favoured by
29. 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 :
30. O₂(g) is paramagnetic in nature because it has
31. Identify the chemical species having maximum number of lone pair of electrons on the central atom, in its most stable structure:
32. 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:
33. 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
34. HF has highest boiling point among hydrogen halides, because it has:
35. p-Hydroxybenzophenone upon reaction with bromine in carbon tetrachloride gives:
36. 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
37. 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
38. 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
39. 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:
40. 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]
41. 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
42. 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
43. 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?
44. If Ni²⁺ ion is replaced with Pt²⁺ ion in complex [NiCl₂Br₂], which of the following would change:
45. 25 g of an unknown hydrocarbon upon burning produces 88 g of CO₂ and 9 g of H₂O. This unknown hydrocarbon contains.
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FULL SYLLABUS CHEMISTRY TEST: 04
NEET CHEMISTRY TEST 2026 [TEST 04]
1. Which of the following best explains why salt is spread on icy roads in winter?
2. Incorrect statement among the following :
3. For the chemical reaction:
I⁻ + ClO₃⁻ + H₂SO₄ ➝ Cl⁻ + HSO₄⁻ + I₂,
Choose the Incorrect statement for the balanced equation:
4. Elevation in boiling point for 1·5 molal solution of glucose in water is 4 K. The depression in freezing point of 4.5 molal solution of glucose in water is 4 K. The ratio of molal elevation constant to molal depression constant (Kb/Kf) is
5. 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
6. Identify the INCORRECT IUPAC Name of an Organic Compound:
I. 2, 3-Diethylbutane
II. 1-Aminomethanal
III. 3-Oxopropanal
7. 2·44 g of benzoic acid (C₆H₅COOH, Molar Mass = 122·00) dissolved in 25 g of benzene shows a depression in freezing point equal to 2·45 K. Molal depression constant for benzene is 4.9 K kg mol⁻¹. What is the percentage association of acid if it forms dimer in solution?
8. Which one of the following reagents react differently with HCHO(methanal), CH₃CHO(ethanal) and CH₃COCH₃ (propanone)?
9. What should be the correct order for bond dissociation energy?
10. At -20 °C and 1 atm pressure, a cylinder is filled with equal number of H₂, I₂ and HI molecules for the reaction,
H₂(g) + I₂(g) ⇌ 2HI (g), the Kp for the process is: z × 10⁻¹. Then z is equal to
[Given: R = 0.082 L atm K⁻¹ mol⁻¹]
11. For the following oxyacid formula HClOₓ (x lies between 1 to 4 ), which of the following is INCORRECT if value of x increases?
12. The IUPAC name of the given structure is:
13. Number of lone pairs of electrons in the central atom of SCl₂, O₃, ClF₃ and SF₆ respectively, are:
14. Which of the following is INCORRECT statement?
15. What is the hybridization state of the circled nitrogens, respectively?
16. For a first-order reaction, the time required to reduce the concentration from 1.0 M to 0.5 M is 20 min. Time required to reduce it from 2.0 M to 1.0 M is:
17. A non-volatile solute is added to a pure liquid solvent. Which of the following changes occurs?
18. Boiling point of a 2% aqueous solution of a non-volatile solute 1 is equal to the boiling point of 8% aqueous solution of a non volatile solute 2. The relation between molecular weight 1 and 2 is:
19. The periodicity in properties is a result primarily of
20. Consider the following statements regarding magnetism of two complexes:
I. [CoF₆]³⁻is a paramagnetic and high spin complex II. [Co(NH₃)₆]³⁺ is a diamagnetic and low spin complex
Which of the statements given above is/are correct?
21. Correct order for molar conductivity at infinite dilution is:
22. When 2-methylbut-3-en-2-ol is treated with concentrated hydrochloric acid, 1-chloro-3-methylbut-2-ene is produced, as shown in the above figure. Choose the INCORRECT statement about the reaction:
23. If 0.1 M solution of glucose and 0.1 M solution of urea are placed on two sides of the semipermeable membrane to equal heights, then it will be correct to say that
24. At 27°C one mole of an ideal gas is compressed isothermally and reversibly from a pressure of 2 atm to 10 atm. The values of U and q are respectively (R = 2 cal K-1 mol-1)
25. Resistance of 0.2 M solution of an electrolyte is 50 Ω. The specific conductance of the solution is 1.4 Sm⁻¹. The resistance of 0.5 M solution of the same electrolyte is 280 Ω. The molar conductivity of 0.5 M solution of the electrolyte in Sm²/mol will be
26. CₐHₓNₑ + CuO ➝ CO₂ + H₂O + N₂ + Cu. In the balanced chemical reaction for 1 mole of CₐHₓNₑ, number of moles of Cu produced would be:
27. In estimation of sulphur, 0.314 g of an organic compound gave 0.9626 g of barium sulphate (BaSO₄ = 233 g mol⁻¹). What is the percentage of sulphur in the compound?
28. In a reaction A → Products, doubling the concentration of A increases the rate by 8 times. The order of the reaction is:
29. What is the free energy change per mole when liquid water boils against 1 atm pressure? (ΔHvap = 2.0723 kJ/g)
30. The species having bond order different from that in CO is
31. A compound ( C₄H₈O) which gives 2,4-DNP derivative and negative iodoform test is
32. For the given reaction, choose the correct expression of Kc from the following :
\(Fe^{3+}(aq)\ +\ SCN^-(aq) \rightleftharpoons [FeSCN]^{2+}(aq)\)
33. At constant temperature, the equilibrium constant (K,) for the decomposition reaction N₂O₄ ⇌ 2NO₂, is expressed by Kp = (4x²P) /(1 - x²), where P = pressure, x = extent of decomposition. Which one of the following statements is true?
34. Enthalpies of combustion of CH₃OH, C, and H₂ are respectively: ﹣676, ﹣394 and ﹣242 kJ mol⁻¹, respectively. What would be the enthalpy of formation of CH₃OH?
35. The reduction potential values of A, B and C are +1.46 V, −1.01 V and −2.13 V respectively. Which of the following is the correct order of reducing power?
36. HF reacts with SiF₄ to give H₂[SiF₆], this is possible because
I. the number of valence orbitals of silicon is greater than four, and part of them are not occupied by valence electrons;
II. the number of valence electrons of silicon is four;
III. Having smaller size and basic nature of F⁻, favoured the formation of octahedral compound with Si.
Choose the correct statement(s):
37. For the structures given above, choose the correct statement
38. 2 Mn²⁺ + 5 S₂O₈²⁻ + 8 H₂O ➝ 2 MnO₄⁻ + 10 SO₄²⁻ + 16 H⁺, In this reaction the element undergoing decrease in oxidation number is:
39. The amount of charge in (faraday) required to obtain one mole of iron from Fe₃O₄ is
40. A hydrocarbon X is optically active. X upon hydrogenation gives an optically inactive alkane Y. X is
41. In case of XeO₂F₂ and XeF₆, Xe is with
42. The number of structural and configurational isomers of a bromo compound , C₅H₉Br, formed by the addition of HBr to pent-2-yne respectively are
43. An orange solid on heating gives a colourless gas and a green solid which can be reduced to metal by aluminium powder. Orange and green solids are respectively,
44. Which of the following element does not undergo disproportionation Reaction?
45. Which of the following is true about Fuel Cell
NEET CHEMISTRY TEST 2026 [TEST 05]
1. Given equivalent conductivities at 298 K:
2. 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?
3. Which of the following statements are correct about :C≡O: molecule?
4. The number of σ bonds in the structure 卐 is
5. Which of the following reactions will yield propan-2-ol?
6. What should be the pH of 0.01M NaCl(aq) solution at 25ᴼC, if Kw for H₂O is 1·0 × 10⁻¹⁴ M²?
7. Choose CORRECT Statement:
8. 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?
9. 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:
10. The chemical species having two π-bonds and ½ σ-bond is:
11. Consider the following statement(s):
I. Cyclohexanone forms cyanohydrin in good yield but 2,2,6-trimethylcyclo- hexanone does not.
II. There are two –NH₂ groups in semicarbazide. However, only one is involvedin the formation of semicarbazones III. Although phenoxide ion has more number of resonating structures than carboxylate ion, carboxylic acid is a stronger acid than phenol
The correct statements is/are:
12. Consider the following statements:
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
14. 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
15. 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?
16. At constant temperature, the equilibrium constant (K,) for the decomposition reaction N₂O₄ ⇌ 2NO₂, is expressed by Kp = (4x²P) /(1 - x²), where P = pressure, x = extent of decomposition. Which one of the following statements is true?
17. Choose the INCORRECT statement:
18. E⁰ for: [MnO₄]⁻ (aq) + 8 H⁺ (aq) + 5 e⁻ ⇌ Mn²⁺(aq) + 4 H₂O(l), is +1·51 V, what is the reduction potential in aqueous solution of pH = 2·5 having the ratio [Mn²⁺]:[MnO₄⁻] = 1 : 100?
pH = -log[H⁺]
[H⁺] = 10⁻²·⁵
Now apply the Nernst equation:
E = E⁰﹣(0·06)/(5) × log([Mn²⁺])/[MnO₄⁻][H⁺]⁸
E = 1·51 ﹣0·216 = + 1·294 V
19. The IUPAC name of the given structure is:
20. Sample solutions of each of the three acids (given in figure) were titrated with 0.10 M NaOH(aq). Each of the acid solutions had a concentration of 0.10 M. Which of the acid titrations had the highest pH at the endpoint?
21. Which one of the following compounds can exhibit both geometrical and optical isomerism?
22. 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
23. Resistance of 0.2 M solution of an electrolyte is 50 Ω. The specific conductance of the solution is 1.4 Sm⁻¹. The resistance of 0.5 M solution of the same electrolyte is 280 Ω. The molar conductivity of 0.5 M solution of the electrolyte in Sm²/mol will be
24. The best reagent for converting 2-phenylpropanamide into 2- phenylpropanamine is
25. For which of the following conversion, there is no change in number of electronic exchange?
26. 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
27. Choose the INCORRECT statement:
28. A sample of 1·0 g of an organic compound was treated according to Kjeldahl’s method. The ammonia evolved was absorbed in 100 mL of 0·5 M H₂SO₄. The residual acid required 50 mL of 1·0 M NaOH for neutralisation. What is the % of nitrogen in the organic compound?
29. 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
30. The hybridisations of the central atom in the chemical species, ClF₃, BrF₅ & [ICl₂]⁺, are respectively
31. CₐHₓNₑ + CuO ➝ CO₂ + H₂O + N₂ + Cu. In the balanced chemical reaction for 1 mole of CₐHₓNₑ, number of moles of Cu produced would be:
32. 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?
33. 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
34. 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?
35. Cis but-2-ene and trans but-2-ene are
36. In which of the following case osmotic pressure should be minimum?
37. 2 Mn²⁺ + 5 S₂O₈²⁻ + 8 H₂O ➝ 2 MnO₄⁻ + 10 SO₄²⁻ + 16 H⁺, In this reaction the element undergoing decrease in oxidation number is:
38. The orbital angular momentum of a d-electron is given as:
39. Boiling point of a 2% aqueous solution of a non-volatile solute 1 is equal to the boiling point of 8% aqueous solution of a non volatile solute 2. The relation between molecular weight 1 and 2 is:
40. How many mole of Au will be deposited on the cathode when 0·60 F of electricity is passed through 1 L solution of 0·10 M Au³⁺(aq)?
41. Absolute value of which of the following thermodynamic property can be calculated?
42. What is the entropy change of 1 mole sample of perfect gas when it expands isothermally so that its volume doubles?
43. The following reaction occurs in the Blast furnace where iron ore is reduced to iron metal :
\(Fe_2 O_3(s) \ + \ 3CO(g) \rightleftharpoons Fe(l)\ +\ 3CO_2(g)\)
Using the Le-Chateler's principle, predict which one of the following will not disturb the equilibrium.
44. The periodicity in properties is a result primarily of
45. At -20 °C and 1 atm pressure, a cylinder is filled with equal number of H₂, I₂ and HI molecules for the reaction,
