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 coordination numbers of Au and Pt in the complexes formed when they are treated with aqua-regia are respectively:
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3. Number of mole of Cr₂O₇²⁻ required to oxidise 4 mole of ferrous oxalate in acidic medium is:
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4. The hybridisations of the central atom in the chemical species, ClF₃, BrF₅ & [ICl₂]⁺, are respectively
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5. Arrange the compounds (A to E) in the order of solubility in hexane:
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6. 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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7. 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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8. The number of σ bonds in the structure 卐 is
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9. The product (B) in the following reaction sequence is:
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10. 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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11. In which of the following case osmotic pressure should be minimum?
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12. 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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13. Among the following compounds, the one(s) that gives(give) effervescence with aq. NaHCO₃ solution is (are):
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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
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15. Which one of the following statements is INCORRECT?
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16. 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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17. In which one of the following molecules, all the bond lengths are equal?
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18. 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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19. Which of the following is the INCORRECT order for the melting points of d-block elements?
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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. Identify the product (C) in the following sequence:
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22. 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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23. 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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24. The correct order for O-O bond length in the species is:
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25. Which one of the following compounds can exhibit both geometrical and optical isomerism?
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26. 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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27. The bond dissociation enthalpies for the nitrogen–nitrogen bond in N₂ and [N₂]⁻ are respectively:
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28. 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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29. 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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30. 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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31. 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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32. 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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33.
What is the configuration of the following compound?
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34. Which of the following is/are non reducing sugar(s)?
I. Fructose
II. Maltose
III. Sucrose
IV. Lactose
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35. 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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36. The correct order for the wavelengths of absorption for the following is
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37. Choose the correct statement about K₂Cr₂O₇:
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38. In the following two reaction sequences products Ⓒ and Ⓓ can be distinguished by:
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39. For which of the following conversion, there is no change in number of electronic exchange?
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40. High spin and low spin complexes are not possible with the configuration:
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41. 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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42. Which of the following is the composition of sucrose?
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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
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44. Which of the following is not true about brown ring test?
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45. Correct order for molar conductivity at infinite dilution is:
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FULL SYLLABUS CHEMISTRY TEST: 02
NEET CHEMISTRY TEST 2026 [TEST 02]
1. Consider the following statements about plot of Intensity versus wavelength during black body radiation at various temperatures:
Choose the CORRECT statement
2. Number of phenols possible with molecular formula C₇H₈O is:
3. 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?
4. What is the average formal charge on each oxygen in [NO₃]⁻?
5. Which of the following tests are given positive by both aldehydes and ketones?
6. 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)
7. The carbocation in which rearrangement is not feasible?
8. 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?
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:
2 H₂(g) + O₂(g) ➝ 2 H₂O(l) ?
10. 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)?
11. When the Intermediate complex of Balz-Schiemann reaction heated in NaNO₂ with Cu forms
12. 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.
13. 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
14. Choose the INCORRECT statement:
15. Electron gain enthalpies (in kJ mol⁻¹) of Cl(g) and F(g) are respectively:
16. 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)?
17. Identify the pair of linear molecules:
18. If radius of second orbit of Be³⁺ is x Å, then what is the radius of 4ᵗʰ orbit of He⁺
19. The incorrect order among the following is:
20. 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
21. What is the relation between compounds A and B?
22. 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?
23. Which of the following statements are correct about :C≡O: molecule?
24. 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 ________.
25. 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?
26. 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
27. 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?
28. Consider the following statements:
Choose the CORRECT statements:
29. Consider the following statements:
30. Which of the following pair of chemical species are NOT iso-structural as well as isoelectronic?
31. Bond order in CO and oxidation number of carbon in it, are respectively:
32. Consider the following statements:
33. 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.
34. 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
35. 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?
36. A hydrocarbon X is optically active. X upon hydrogenation gives an optically inactive alkane Y. X is
37. When glucose is treated with bromine water and concentrated nitric acid separately, is converted respectively into:
38. 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.
39. 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:
40. Which of the following pair of compounds are polar?
41. The chemical species having two π-bonds and ½ σ-bond is:
42. Which of the following ion has zero spin only magnetic moment?
43. What is the correct IUPAC name of the structure given?
44. 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.]
45. 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?
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. In H-atom if electron absorbs a photon of 1·89 eV, then transition of electron is from
3. 25 g of an unknown hydrocarbon upon burning produces 88 g of CO₂ and 9 g of H₂O. This unknown hydrocarbon contains.
4. 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
5. 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
6. 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
7. The correct order of the following compounds towards addition of HCN is:
8. Which of the following metal will exhibit photoelectric effect with photon having longest wavelength?
9. 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
10. 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:
11. Energy of electron in 2ⁿᵈ orbit of Be³⁺ is ﹣x eV atom⁻¹, what is the energy of electron in 4ᵗʰ orbit of He⁺?
12. Increasing order of reactivity of the following compounds for SN1 substitution is:
13. 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
14. 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?
15. 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?
16. 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
17. 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:
18. 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
19. 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
20. The process in which an ideal gas undergoes change from X to Y as shown in the following diagram is
21. Consider the following reaction:
[CoCl₂(NH₃)₄]⁺ + Cl⁻ ➝ [CoCl₃(NH₃)₃] + NH₃.
Which of the following statements are correct:
22. 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
23. What is the product of following reaction?
24. 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.
25. 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.
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. If Ni²⁺ ion is replaced with Pt²⁺ ion in complex [NiCl₂Br₂], which of the following would change:
28. 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]
29. 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:
30. 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)
31. The best sequence of reactions for the following conversion is
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 C–C bond length is maximum in
34. 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
35. The ammonia(NH₃) released on quantitative reaction of 0.6 g urea (NH₂CONH₂) with sodium hydroxide(NaOH) can be neutralized by
36. 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
37. 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
38. 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
39. 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
40. 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
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. p-Hydroxybenzophenone upon reaction with bromine in carbon tetrachloride gives:
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. The hydrocarbon that cannot be prepared effectively by Wurtz reaction is
45. 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:
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FULL SYLLABUS CHEMISTRY TEST: 04
NEET CHEMISTRY TEST 2026 [TEST 04]
1. Correct order for molar conductivity at infinite dilution is:
2. Consider a reaction with the following data:
What is the rate law?
3. The number of structural and configurational isomers of a bromo compound , C₅H₉Br, formed by the addition of HBr to pent-2-yne respectively are
4. For the chemical reaction:
I⁻ + ClO₃⁻ + H₂SO₄ ➝ Cl⁻ + HSO₄⁻ + I₂,
Choose the Incorrect statement for the balanced equation:
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. In case of XeO₂F₂ and XeF₆, Xe is with
7. If the half-life of a first-order reaction is 10 min, how long will it take for 75% of the substance to decompose?
8. For the following oxyacid formula HClOₓ (x lies between 1 to 4 ), which of the following is INCORRECT if value of x increases?
9. 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)
10. For the structures given above, choose the correct statement
11. Which of the following best explains why salt is spread on icy roads in winter?
12. Which of the following element does not undergo disproportionation Reaction?
13. Which of the following statements is correct about a first-order reaction?
14. In a reaction A → Products, doubling the concentration of A increases the rate by 8 times. The order of the reaction is:
15. CₐHₓNₑ + CuO ➝ CO₂ + H₂O + N₂ + Cu. In the balanced chemical reaction for 1 mole of CₐHₓNₑ, number of moles of Cu produced would be:
16. The IUPAC name of the given structure is:
17. What is the hybridization state of the circled nitrogens, respectively?
18. 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):
19. Which of the following is INCORRECT statement?
20. What is the free energy change per mole when liquid water boils against 1 atm pressure? (ΔHvap = 2.0723 kJ/g)
21. 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
22. 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:
23. 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?
24. 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:
25. 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:
26. 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?
27. A hydrocarbon X is optically active. X upon hydrogenation gives an optically inactive alkane Y. X 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. 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,
30. The amount of charge in (faraday) required to obtain one mole of iron from Fe₃O₄ is
31. 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:
32. Incorrect statement among the following :
33. 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
34. The IUPAC name of the given structure is:
35. 2 Mn²⁺ + 5 S₂O₈²⁻ + 8 H₂O ➝ 2 MnO₄⁻ + 10 SO₄²⁻ + 16 H⁺, In this reaction the element undergoing decrease in oxidation number is:
36. The species having bond order different from that in CO is
37. 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?
38. 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
39. Cis but-2-ene and trans but-2-ene are
40. 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
41. 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?
42. 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:
43. What should be the correct order for bond dissociation energy?
44. Identify the INCORRECT IUPAC Name of an Organic Compound:
I. 2, 3-Diethylbutane
II. 1-Aminomethanal
III. 3-Oxopropanal
45. 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]
NEET CHEMISTRY TEST 2026 [TEST 05]
1. The number of σ bonds in the structure 卐 is
2. 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
3. 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,
4. Absolute value of which of the following thermodynamic property can be calculated?
5. Which of the following ion has zero spin only magnetic moment?
6. 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:
7. At -20 °C and 1 atm pressure, a cylinder is filled with equal number of H₂, I₂ and HI molecules for the reaction,
8. The chemical species having two π-bonds and ½ σ-bond is:
9. When the Intermediate complex of Balz-Schiemann reaction heated in NaNO₂ with Cu forms
10. 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)
11. 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
12. Arrange the compounds (A to E) in the order of solubility in hexane:
13. Which of the following statements are correct about :C≡O: molecule?
14. For the following oxyacid formula HClOₓ (x lies between 1 to 4 ), which of the following is INCORRECT if value of x increases?
15. 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?
16. The orbital angular momentum of a d-electron is given as:
17. Bond order in CO and oxidation number of carbon in it, are respectively:
18. A hydrocarbon X is optically active. X upon hydrogenation gives an optically inactive alkane Y. X is
19. 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:
20. The ratio of wavelengths of last line of Lyman series to that of second line of Balmer series in hydrogen spectrum is:
21. For the given hypothetical reactions, the equilibrium constants are as follows:
22. 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?
23. 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
24. Which of the following pair of molecules contain odd electron molecule and an expanded octet molecule?
25. Which of the following is the INCORRECT order for the melting points of d-block elements?
26. 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
27. Consider the formation of PCl₃:
28. O₂(g) is paramagnetic in nature because it has
29. The process in which an ideal gas undergoes change from X to Y as shown in the following diagram is
30. The IUPAC name of the given structure is:
31. Which of the following is/are non reducing sugar(s)?
32. The correct order for the wavelengths of absorption for the following is
33. Identify the chemical species having maximum number of lone pair of electrons on the central atom, in its most stable structure:
34. High spin and low spin complexes are not possible with the configuration:
35. 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)
36. Consider the following statements about plot of Intensity versus wavelength during black body radiation at various temperatures:
37. Of the following sets which one does NOT contain isoelectronic species?
38. Which of the following element does not undergo disproportionation Reaction?
39. 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
40. Consider the following reversible reaction in a closed container:
41. 10+20
42. 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
43. 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
44. Number of lone pairs of electrons in the central atom of SCl₂, O₃, ClF₃ and SF₆ respectively, are:
45. The hydrocarbon that cannot be prepared effectively by Wurtz reaction is
