FULL SYLLABUS CHEMISTRY TEST: 01
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NEET CHEMISTRY TEST 2026 [TEST 01]
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1. 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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2. The major product ⓧ of the following reaction is:
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3. In which one of the following molecules, all the bond lengths are equal?
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4. The major product in the given reaction is:
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5. Which one of the following statements is INCORRECT?
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6. Identify the major product (Y):
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7. 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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8. 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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9. 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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10. Identify the product (C) in the following sequence:
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11. The correct order for O-O bond length in the species is:
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12. Which of the following is the composition of sucrose?
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13. 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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14. When lanthanoid(Ln) is heated with carbon, the carbide which is not formed is:
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15. 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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16. The bond dissociation enthalpies for the nitrogen–nitrogen bond in N₂ and [N₂]⁻ are respectively:
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17. 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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18. Among the following compounds, the one(s) that gives(give) effervescence with aq. NaHCO₃ solution is (are):
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19. 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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20. In the following two reaction sequences products Ⓒ and Ⓓ can be distinguished by:
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21. In which of the following case osmotic pressure should be minimum?
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22. Which of the following is the Incorrect order for bond angle?
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23. The hybridisations of the central atom in the chemical species, ClF₃, BrF₅ & [ICl₂]⁺, are respectively
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24. 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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25. High spin and low spin complexes are not possible with the configuration:
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26. 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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27. 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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28. Choose the correct statement about K₂Cr₂O₇:
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29. Arrange the compounds in the order of boiling point:
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30. 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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31. For a zero-order reaction, which of the following is correct?
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32. 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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33. 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
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34. Number of mole of Cr₂O₇²⁻ required to oxidise 4 mole of ferrous oxalate in acidic medium is:
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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. The coordination numbers of Au and Pt in the complexes formed when they are treated with aqua-regia are respectively:
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37. 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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38. 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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39. 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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40. For which of the following conversion, there is no change in number of electronic exchange?
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41. 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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42.
What is the configuration of the following compound?
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43. The product (B) in the following reaction sequence is:
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44. 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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45. Which of the following is the INCORRECT order for the melting points of d-block elements?
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FULL SYLLABUS CHEMISTRY TEST: 02
NEET CHEMISTRY TEST 2026 [TEST 02]
1. The incorrect order among the following is:
2. 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?
3. The carbocation in which rearrangement is not feasible?
4. 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.
5. Choose the INCORRECT statement:
6. 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?
7. 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
8. 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.]
9. Bond order in CO and oxidation number of carbon in it, are respectively:
10. 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:
11. 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?
12. Identify the pair of linear molecules:
13. If radius of second orbit of Be³⁺ is x Å, then what is the radius of 4ᵗʰ orbit of He⁺
14. 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
15. What is the relation between compounds A and B?
16. When the Intermediate complex of Balz-Schiemann reaction heated in NaNO₂ with Cu forms
17. A hydrocarbon X is optically active. X upon hydrogenation gives an optically inactive alkane Y. X is
18. Which of the following pair of chemical species are NOT iso-structural as well as isoelectronic?
19. 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?
20. Consider the following statements about plot of Intensity versus wavelength during black body radiation at various temperatures:
Choose the CORRECT statement
21. What is the average formal charge on each oxygen in [NO₃]⁻?
22. 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) ?
23. 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?
24. Consider the following statements:
Choose the CORRECT statements:
25. 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?
26. Consider the following statements:
27. 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
28. 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.
29. 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)?
30. 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)?
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. When 3-Iodo-2,2-dimethylbutane is treated with KOH in ethanol, three elimination products are formed, identify the major one:
33. How many stereogenic carbons are in the structure:
34. For the redox reaction:
x MnO₄⁻ + y C₂O₄²⁻ + z H⁺ ➝ Mn²⁺ + CO₂ + H₂O, x, y and z for the balanced reaction are
35. 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
36. 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
37. 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.
38. The chemical species having two π-bonds and ½ σ-bond is:
39. Which of the following ion has zero spin only magnetic moment?
40. Absolute value of which of the following thermodynamic property can be calculated?
41. Consider the following statements:
42. 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?
43. 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
44. 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?
45. 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?
The average score is 6%
FULL SYLLABUS CHEMISTRY TEST: 03
NEET CHEMISTRY TEST 2026 [TEST 03]
1. 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
2. HF has highest boiling point among hydrogen halides, because it has:
3. 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
4. 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:
5. 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
6. 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:
7. 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?
8. The process in which an ideal gas undergoes change from X to Y as shown in the following diagram is
9. 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:
10. 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
11. 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
12. If azimuthal quantum number (l) of an electron in an orbital is 2, the shape of the orbital should be
13. The order of electron gain enthalpy in kJ/mol of fluorine, chlorine, bromine and iodine, respectively are
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. If Ni²⁺ ion is replaced with Pt²⁺ ion in complex [NiCl₂Br₂], which of the following would change:
16. 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:
17. p-Hydroxybenzophenone upon reaction with bromine in carbon tetrachloride gives:
18. 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:
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 correct order of the following compounds towards addition of HCN is:
21. The hydrocarbon that cannot be prepared effectively by Wurtz reaction is
22. The theory that can completely/properly explain the nature of bonding in [Ni(CO)₄] is
23. 25 g of an unknown hydrocarbon upon burning produces 88 g of CO₂ and 9 g of H₂O. This unknown hydrocarbon contains.
24. 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
25. 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.
26. 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:
27. 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]
28. The C–C bond length is maximum in
29. 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
30. In H-atom if electron absorbs a photon of 1·89 eV, then transition of electron is from
31. 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
32. 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:
33. 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]
34. 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
35. 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.
36. What would be the molality of 20% (mass/mass) aqueous solution of KI? (molar mass of KI = 166 g mol⁻¹)
37. 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)
38. 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
39. Among the following maximum number of resonating structures are possible for
40. Increasing order of reactivity of the following compounds for SN1 substitution is:
41. 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
42. The ammonia(NH₃) released on quantitative reaction of 0.6 g urea (NH₂CONH₂) with sodium hydroxide(NaOH) can be neutralized by
43. 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 :
44. 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
45. What is the product of following reaction?
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FULL SYLLABUS CHEMISTRY TEST: 04
NEET CHEMISTRY TEST 2026 [TEST 04]
1. 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:
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. Correct order for molar conductivity at infinite dilution is:
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. 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)
6. What is the free energy change per mole when liquid water boils against 1 atm pressure? (ΔHvap = 2.0723 kJ/g)
7. A compound ( C₄H₈O) which gives 2,4-DNP derivative and negative iodoform test is
8. Incorrect statement among the following :
9. The periodicity in properties is a result primarily of
10. Which of the following statements is correct about a first-order reaction?
11. Which of the following is INCORRECT statement?
12. 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
13. The IUPAC name of the given structure is:
14. What is the hybridization state of the circled nitrogens, respectively?
15. 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:
16. A non-volatile solute is added to a pure liquid solvent. Which of the following changes occurs?
17. The IUPAC name of the given structure is:
18. If the half-life of a first-order reaction is 10 min, how long will it take for 75% of the substance to decompose?
19. 2 Mn²⁺ + 5 S₂O₈²⁻ + 8 H₂O ➝ 2 MnO₄⁻ + 10 SO₄²⁻ + 16 H⁺, In this reaction the element undergoing decrease in oxidation number is:
20. 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.
21. Which of the following element does not undergo disproportionation Reaction?
22. For the given reaction, choose the correct expression of Kc from the following :
\(Fe^{3+}(aq)\ +\ SCN^-(aq) \rightleftharpoons [FeSCN]^{2+}(aq)\)
23. What should be the correct order for bond dissociation energy?
24. 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?
25. For the structures given above, choose the correct statement
26. A hydrocarbon X is optically active. X upon hydrogenation gives an optically inactive alkane Y. X is
27. In a reaction A → Products, doubling the concentration of A increases the rate by 8 times. The order of the reaction is:
28. 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
29. Which of the following best explains why salt is spread on icy roads in winter?
30. 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]
31. 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
32. 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:
33. 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?
34. 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
35. For the chemical reaction:
I⁻ + ClO₃⁻ + H₂SO₄ ➝ Cl⁻ + HSO₄⁻ + I₂,
Choose the Incorrect statement for the balanced equation:
36. Cis but-2-ene and trans but-2-ene are
37. Consider a reaction with the following data:
What is the rate law?
38. Which of the following pair of molecules contain odd electron molecule and an expanded octet molecule?
39. 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?
40. Which of the following is true about Fuel Cell
41. 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:
42. Number of lone pairs of electrons in the central atom of SCl₂, O₃, ClF₃ and SF₆ respectively, are:
43. Which one of the following reagents react differently with HCHO(methanal), CH₃CHO(ethanal) and CH₃COCH₃ (propanone)?
44. The correct order of the spin only magnetic moment of metal ions in the following low spin complexes, [V(CN)₆)⁴⁻, [Fe(CN)₆]⁴⁻, [Ru(NH₃)₆]³⁺, [Cr(NH₃)₆], and [Cr(NH₃)₆]²⁺ is:
45. 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?
NEET CHEMISTRY TEST 2026 [TEST 05]
1. Choose the correct statement about K₂Cr₂O₇:
2. 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.
3. Which of the following tests are given positive by both aldehydes and ketones?
4. Two finite sets have m and n elements. The total number of subsets of the first set is 56 more than the total number of subsets of the second set. The values of m and n are
\[ 2^m-2^n=56=8\times7=2^3\times 7 \]
\[ 2^n(2^{m-n}-1)=2\times 7 \]
\[ ∴ n=3 \text{ and } 2^{m-n}=2^3 \]
\[ m-n=3,\ \text{ i.e., } m = 6 \]
5. 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?
6. 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?
7. 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
8. The coordination numbers of Au and Pt in the complexes formed when they are treated with aqua-regia are respectively:
9. EMF of the cell
10. 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
11. 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,
12. High spin and low spin complexes are not possible with the configuration:
13. If Ni²⁺ ion is replaced with Pt²⁺ ion in complex [NiCl₂Br₂], which of the following would change:
14. The following reaction occurs in the Blast furnace where iron ore is reduced to iron metal :
15. Which of the following is INCORRECT statement?
16. At -20 °C and 1 atm pressure, a cylinder is filled with equal number of H₂, I₂ and HI molecules for the reaction,
17. 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
18. The amount of charge in (faraday) required to obtain one mole of iron from Fe₃O₄ is
19. 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):
20. 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
21. Among the following maximum number of resonating structures are possible for
22. Identify the pair of linear molecules:
23. 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:
24. 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]
25. 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
26. The product (B) in the following reaction sequence is:
27. In the following reaction:
28. 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.
29. In case of XeO₂F₂ and XeF₆, Xe is with
30. 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?
32. Incorrect statement among the following :
33. 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
34. If Eᴼ for MnO₄⁻ ➝ Mn²⁺ is X₁ V and Eᴼ for MnO₄⁻ ➝ Mn⁴⁺ is X₂ V, then what will be Eᴼ for Mn⁴⁺ ➝ Mn²⁺?
35. The number of σ bonds in the structure 卐 is
36. 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?
37. Cis but-2-ene and trans but-2-ene are
38. 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?
39. Identify the product (X) in the reaction:
40. The IUPAC name of the given structure is:
41. 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?
42. If Kc = 3·92 × 10¹⁵, for the reaction:
43. 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
44. What is the relation between compounds A and B?
45. The best sequence of reactions for the following conversion is
