FULL SYLLABUS CHEMISTRY TEST: 01
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NEET CHEMISTRY TEST 2026 [TEST 01]
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1. The bond dissociation enthalpies for the nitrogen–nitrogen bond in N₂ and [N₂]⁻ are respectively:
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2. 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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3. 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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4. Identify the major product (Y):
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5. The functional group which is not present in the given structure is:
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6. 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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7. The correct order for the wavelengths of absorption for the following is
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8. 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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9. 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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10. Choose the INCORRECT statement:
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11. 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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12. 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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13. The coordination numbers of Au and Pt in the complexes formed when they are treated with aqua-regia are respectively:
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14. Which of the following is the Incorrect order for bond angle?
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15. Arrange the compounds in the order of boiling point:
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16. 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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17. 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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18. Which of the following is the INCORRECT order for the melting points of d-block elements?
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19. 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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20. When a catalyst is added to a reaction at 27 ⁰C, its rate becomes twice, what is the decrease in the activation energy of the reaction?
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21. Which of the following is/are non reducing sugar(s)?
I. Fructose
II. Maltose
III. Sucrose
IV. Lactose
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22. 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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23. In which of the following case osmotic pressure should be minimum?
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24. Correct order for molar conductivity at infinite dilution is:
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25. 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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26. 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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27. 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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28. The hybridisations of the central atom in the chemical species, ClF₃, BrF₅ & [ICl₂]⁺, are respectively
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29. The major product ⓧ of the following reaction is:
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30. The correct order for O-O bond length in the species is:
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31. The half-life period of a first order chemical reaction is 6·93 minutes. The time required for the completion of 99% of the chemical reaction will be
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32. Which one of the following statements is INCORRECT?
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33. 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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34. Among the following compounds, the one(s) that gives(give) effervescence with aq. NaHCO₃ solution is (are):
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35. Which one is INCORRECT order for the property indicated against it?
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36.
What is the configuration of the following compound?
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37. Arrange the compounds (A to E) in the order of solubility in hexane:
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38. 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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39. 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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40. When lanthanoid(Ln) is heated with carbon, the carbide which is not formed is:
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41. Which one of the following compounds can exhibit both geometrical and optical isomerism?
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42. 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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43. 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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44. The major product in the given reaction is:
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45. Identify the product (C) in the following sequence:
Your score is
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FULL SYLLABUS CHEMISTRY TEST: 02
NEET CHEMISTRY TEST 2026 [TEST 02]
1. 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)?
2. What is the relation between compounds A and B?
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. 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.
5. When 3-Iodo-2,2-dimethylbutane is treated with KOH in ethanol, three elimination products are formed, identify the major one:
6. Which of the following statements are correct about :C≡O: molecule?
7. 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
8. 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?
9. Bond order in CO and oxidation number of carbon in it, are respectively:
10. 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?
11. 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?
12. 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)
13. 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.
14. 1 g of graphite is burnt in a bomb calorimeter in excess of oxygen at 298 K and 1 atmospheric pressure according to the equation:
C (graphite) + O₂(g) ➝ CO₂(g)
During the reaction, temperature rises from 298 K to 299 K. If the heat capacity of the bomb calorimeter is 20·7 kJ K⁻¹g⁻¹, what is the enthalpy change for the above reaction at 298 K and 1 atm?
15. 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) ?
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. 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
18. Consider the following statements:
Choose the CORRECT statements:
19. In a qualitative analysis when H₂S is passed through the solution of a salt acidified with HCl, a black precipitate is obtained. On boiling the precipitate with dil. HNO₃, it forms a solution of blue colour. Addition of excess of aqueous solution of ammonia to this solution will give deep blue ________.
20. Based on CFT, which one of the following ions should be colourless?
21. Electron gain enthalpies (in kJ mol⁻¹) of Cl(g) and F(g) are respectively:
22. A hydrocarbon X is optically active. X upon hydrogenation gives an optically inactive alkane Y. X is
23. 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?
24. 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?
25. 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.
26. 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
27. 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
28. Choose the INCORRECT statement:
29. What is the average formal charge on each oxygen in [NO₃]⁻?
30. 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?
31. Identify the product (X) in the reaction:
32. 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:
33. Identify the pair of linear molecules:
34. 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]
35. 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?
36. Absolute value of which of the following thermodynamic property can be calculated?
37. If radius of second orbit of Be³⁺ is x Å, then what is the radius of 4ᵗʰ orbit of He⁺
38. 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
39. Which of the following pair of compounds are polar?
40. How many stereogenic carbons are in the structure:
41. Which of the following ion has zero spin only magnetic moment?
42. Consider the following statements for the complex [Ni(NH₃)₆]Cl₂:
1. It is an outer orbital octahedral complex 2. Hybridization of Ni is sp³d² 3. It is a paramagnetic complex 4. It is a diamagnetic complex
Which of the statements given above are correct?
43. 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?
44. Consider the following statements about plot of Intensity versus wavelength during black body radiation at various temperatures:
Choose the CORRECT statement
45. 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.
The average score is 6%
FULL SYLLABUS CHEMISTRY TEST: 03
NEET CHEMISTRY TEST 2026 [TEST 03]
1. 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
2. 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:
3. 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 :
4. 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:
5. 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
6. If Ni²⁺ ion is replaced with Pt²⁺ ion in complex [NiCl₂Br₂], which of the following would change:
7. 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:
8. 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
9. 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
10. 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
11. 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
12. 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
13. 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:
14. 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
15. The order of electron gain enthalpy in kJ/mol of fluorine, chlorine, bromine and iodine, respectively are
16. What would be the molality of 20% (mass/mass) aqueous solution of KI? (molar mass of KI = 166 g mol⁻¹)
17. The theory that can completely/properly explain the nature of bonding in [Ni(CO)₄] is
18. Energy of electron in 2ⁿᵈ orbit of Be³⁺ is ﹣x eV atom⁻¹, what is the energy of electron in 4ᵗʰ orbit of He⁺?
19. A solution of Ni(NO₃)₂ is electrolysed between platinum electrodes using 0.1 faraday electricity. How many mole of Ni will be deposited at the cathode?
20. 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)
21. 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
22. 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
23. A cricket ball is moving with a kinetic energy of 5 J. The wavelength of the ball will be [h = 6.626 × 10⁻³⁴ Js]
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. If azimuthal quantum number (l) of an electron in an orbital is 2, the shape of the orbital should be
26. 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
27. Among the following maximum number of resonating structures are possible for
28. 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:
29. 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)
30. Increasing order of reactivity of the following compounds for SN1 substitution is:
31. HF has highest boiling point among hydrogen halides, because it has:
32. A₂(g) + 4 B₂(g) ⇌ 2 AB₄(g), ΔH < 0
Product formation is favoured by
33. Consider the following reaction:
[CoCl₂(NH₃)₄]⁺ + Cl⁻ ➝ [CoCl₃(NH₃)₃] + NH₃.
Which of the following statements are correct:
34. 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:
35. 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?
36. 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.
37. Which of the following metal will exhibit photoelectric effect with photon having longest wavelength?
38. 25 g of an unknown hydrocarbon upon burning produces 88 g of CO₂ and 9 g of H₂O. This unknown hydrocarbon contains.
39. 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
40. The process in which an ideal gas undergoes change from X to Y as shown in the following diagram is
41. The C–C bond length is maximum in
42. 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
43. The reaction of 2, 4-hexadiene with one equivalent of bromine at 0⁰ C gives a mixture of two compounds ‘X’ and ‘Y’. If ‘X’ is 4, 5-dibromohex-2-ene, ‘Y’ is
44. The correct order of the following compounds towards addition of HCN is:
45. The ammonia(NH₃) released on quantitative reaction of 0.6 g urea (NH₂CONH₂) with sodium hydroxide(NaOH) can be neutralized by
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FULL SYLLABUS CHEMISTRY TEST: 04
NEET CHEMISTRY TEST 2026 [TEST 04]
1. 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:
2. CₐHₓNₑ + CuO ➝ CO₂ + H₂O + N₂ + Cu. In the balanced chemical reaction for 1 mole of CₐHₓNₑ, number of moles of Cu produced would be:
3. 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:
4. For the following oxyacid formula HClOₓ (x lies between 1 to 4 ), which of the following is INCORRECT if value of x increases?
5. 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.
6. What is the free energy change per mole when liquid water boils against 1 atm pressure? (ΔHvap = 2.0723 kJ/g)
7. Which of the following element does not undergo disproportionation Reaction?
8. For the structures given above, choose the correct statement
9. The enthalpy of vapourisation of a liquid is 30 kJ mol–1 and entropy of vapourisation is 75 mol–1 K. The boiling point of the liquid at 1 atm is
10. Which of the following pair of molecules contain odd electron molecule and an expanded octet molecule?
11. Which of the following is INCORRECT statement?
12. 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?
13. 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]
14. The species having bond order different from that in CO is
15. Which one of the following reagents react differently with HCHO(methanal), CH₃CHO(ethanal) and CH₃COCH₃ (propanone)?
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. What should be the correct order for bond dissociation energy?
18. 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?
19. For the chemical reaction:
I⁻ + ClO₃⁻ + H₂SO₄ ➝ Cl⁻ + HSO₄⁻ + I₂,
Choose the Incorrect statement for the balanced equation:
20. 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
21. In case of XeO₂F₂ and XeF₆, Xe is with
22. 2 Mn²⁺ + 5 S₂O₈²⁻ + 8 H₂O ➝ 2 MnO₄⁻ + 10 SO₄²⁻ + 16 H⁺, In this reaction the element undergoing decrease in oxidation number is:
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. In an experiment 0.22 g of magnesium pyrophosphate was produced from 0.1 g of an organic compound. Percentage of phosphorus in the compound is
25. 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,
26. 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:
27. Consider a reaction with the following data:
What is the rate law?
28. The IUPAC name of the given structure is:
29. A compound ( C₄H₈O) which gives 2,4-DNP derivative and negative iodoform test is
30. Identify the INCORRECT IUPAC Name of an Organic Compound:
I. 2, 3-Diethylbutane
II. 1-Aminomethanal
III. 3-Oxopropanal
31. 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)
32. In a reaction A → Products, doubling the concentration of A increases the rate by 8 times. The order of the reaction is:
33. 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
34. Cis but-2-ene and trans but-2-ene are
35. The number of structural and configurational isomers of a bromo compound , C₅H₉Br, formed by the addition of HBr to pent-2-yne respectively are
36. Which of the following best explains why salt is spread on icy roads in winter?
37. 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
38. A non-volatile solute is added to a pure liquid solvent. Which of the following changes occurs?
39. For the given hypothetical reactions, the equilibrium constants are as follows:
X ⇌ Y; K₁= 1.0
Y ⇌ Z; K₂ = 2.0
Z ⇌ W; K₃ = 4.0
The equilibrium constant for the reaction, X ⇌ W is
40. Correct order for molar conductivity at infinite dilution is:
41. Which of the following statements is correct about a first-order reaction?
42. 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:
43. The IUPAC name of the given structure is:
44. The amount of charge in (faraday) required to obtain one mole of iron from Fe₃O₄ is
45. 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):
NEET CHEMISTRY TEST 2026 [TEST 05]
1. 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?
2. 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
3. The stepwise stability constants, at 303 K, of [Ni(OH₂)₆₋ₓ (NH₃)ₓ]²⁺,(x = 1 to 6) as: log K₁ = 2·79, log K₂ = 2·26, log K₃ = 1·69, log K₄ = 1·25, log K₅ = 0·74 and log K₆ = 0·03. What should be the β₆ for [Ni(NH₃)₆]²⁺?
Β₆ = K₁ × K₂ × K₃ × K₄ × K₅ × K₆
log Β₆ = log K₁ + log K₂ + log K₃ + log K₄ + log K₅ + log K₆
= 2.79 + 2.26 + 1.68 + 1.25 + 0.74 + 0.03
= 8.76
∴ β₆ = 5.75 × 10⁸
4. 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:
5. Which of the following is the Incorrect order for bond angle?
6. 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?
7. The best reagent for converting 2-phenylpropanamide into 2- phenylpropanamine is
8. A non-volatile solute is added to a pure liquid solvent. Which of the following changes occurs?
9. Number of phenols possible with molecular formula C₇H₈O is:
10. For the given hypothetical reactions, the equilibrium constants are as follows:
11. The ratio of wavelengths of last line of Lyman series to that of second line of Balmer series in hydrogen spectrum is:
12. Consider the following statements:
13. The incorrect order among the following is:
14. 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?
15. Which of the following is the INCORRECT order for the melting points of d-block elements?
16. 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:
17. What is the average formal charge on each oxygen in [NO₃]⁻?
18. Which of the following pair of chemical species are NOT iso-structural as well as isoelectronic?
19. Consider the following statement(s):
20. 150/3
21. 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?
22. 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
23. 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]
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]
25. Gas phase reactions (i) and (ii) are of first and second order respectively
26. 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?
27. The correct order for O-O bond length in the species is:
28. In case of XeO₂F₂ and XeF₆, Xe is with
29. What is the free energy change per mole when liquid water boils against 1 atm pressure? (ΔHvap = 2.0723 kJ/g)
30. 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,
31. The set A = {x : x ∈ R, x² = 16 and 2x = 6} equals
x² = 16, i.e., x = ± 4,
2x = 6, i.e., x = 3
There is no value of x which satisfies both the above equations. Thus, A = φ
32. The correct order for the wavelengths of absorption for the following is
33. What is the hybridization state of the circled nitrogens, respectively?
34. The hydrocarbon that cannot be prepared effectively by Wurtz reaction is
35. Arrange the compounds in the order of boiling point:
36. For the redox reaction:
x MnO₄⁻ + y C₂O₄²⁻ + z H⁺ ➝ Mn²⁺ + CO₂ + H₂O, x, y and z for the balanced reaction are
37. Identify the pair of linear molecules:
38. The mass ratio of steam and hydrogen is found to be 1:1·5 at equilibrium in the following reaction:
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. 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
41. A certain reaction is non spontaneous under standard conditions but becomes spontaneous at lower temperatures. What conclusions may be drawn under standard conditions?
42. 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]
43. In an experiment 0.22 g of magnesium pyrophosphate was produced from 0.1 g of an organic compound. Percentage of phosphorus in the compound is
44. Carbon suboxide (C₃O₂), has a linear structure. Which of the following is correct about C₃O₂?
45. Which of the following ion has zero spin only magnetic moment?
