odadmin

NEET UG Chemistry Practice Paper – Part 12 (Solutions) is designed to strengthen one of the most formula-driven yet concept-oriented chapters of Physical Chemistry. Questions from the Solutions chapter appear regularly in NEET and are often considered easy scoring—but only when concepts like concentration terms, colligative properties, Raoult’s law, and abnormal molar mass are clearly understood. This practice paper brings together NEET-level MCQs inspired by previous years’ trends, helping students revise key formulas, apply concepts accurately, and avoid common mistakes. It is ideal for concept reinforcement, exam-oriented practice, and boosting confidence before full-length mock tests. NEET UG – Chemistry Practice Paper (Previous Years’ Questions) Part 12 | Topic: Solutions Total Questions: 30 | Total Marks: 120 Q1. Molarity is defined as: Moles of solute per kg solvent Moles of solute per litre solution Grams of solute per litre solution Equivalent per litre Molarity = moles of solute per litre of solution. Q2. Molality is independent of: Temperature Pressure Solvent mass Solute mass Molality depends on mass, not volume. Q3. Which is a colligative property? Surface tension Viscosity Osmotic pressure Density Depends only on number of particles. Q4. Raoult’s law applies best to: Ideal solutions Non-ideal solutions Electrolytes Colloids Valid for ideal solutions. Q5. Van’t Hoff factor (i) for NaCl is ideally: 1 2 3 0.5 NaCl dissociates into Na⁺ and Cl⁻. Q6. Which solution has highest osmotic pressure? 0.1 M glucose 0.1 M NaCl 0.1 M CaCl₂ 0.1 M urea CaCl₂ gives maximum particles. Q7. Which colligative property is used to determine molar mass? Elevation of boiling point Depression of freezing point Osmotic pressure All of these All can be used. Q8. Which solution shows negative deviation from Raoult’s law? Benzene + Toluene Ethanol + Acetone Chloroform + Acetone Hexane + Heptane Strong intermolecular interactions. Q9. Unit of osmotic pressure is: atm bar mmHg All of these Pressure units apply. Q10. Which property is independent of nature of solute? Osmotic pressure Vapour pressure lowering Elevation in boiling point All of these All are colligative properties. Q11. Henry’s law relates: Solubility and temperature Solubility and pressure Pressure and volume Concentration and temperature Gas solubility ∝ pressure. Q12. Ideal solution shows: ΔHmix ≠ 0 ΔVmix ≠ 0 ΔHmix = 0 Strong interactions No heat change on mixing. Q13. Which concentration unit changes with temperature? Molality Mole fraction Molarity Mass % Volume changes with temperature. Q14. Freezing point depression is given by: ΔTf = Kf m ΔTb = Kb m π = CRT p = x p° Freezing point depression formula. Q15. Which solution boils at highest temperature? 0.1 m glucose 0.1 m NaCl 0.1 m CaCl₂ 0.1 m urea More particles → higher ΔTb. Q16. Relative lowering of vapour pressure equals: Mole fraction of solvent Mole fraction of solute Molality Molarity Δp/p° = xsolute. Q17. Which solution shows positive deviation? Acetone + CS₂ Ethanol + Acetone Chloroform + Acetone Benzene + Toluene Weaker interactions. Q18. Colligative properties depend on: Nature of solute Number of particles Molecular mass Size of solute Only particle count matters. Q19. Van’t Hoff factor less than 1 indicates: Dissociation Association Ionisation Hydrolysis Association reduces particle count. Q20. Osmotic pressure method is best for: Low molar mass solutes Volatile solutes Polymers Electrolytes Used for high molar mass substances. Q21. Boiling point elevation constant depends on: Solute Solvent Concentration Pressure Kb is property of solvent. Q22. Which solution has lowest freezing point? 0.1 m glucose 0.1 m NaCl 0.1 m CaCl₂ 0.1 m urea Maximum ΔTf. Q23. Henry’s law constant is high when: Gas is highly soluble Gas is less soluble Temperature is low Pressure is low High KH → low solubility. Q24. Which is NOT a solution? Brass Sugar in water Milk Air Milk is a colloid. Q25. Vapour pressure of pure solvent is: Higher than solution Lower than solution Same as solution Zero Adding solute lowers vapour pressure. Q26. Which concentration unit is dimensionless? Molarity Molality Mole fraction Normality Ratio of moles. Q27. Osmotic pressure is directly proportional to: Temperature Concentration Both (a) and (b) Volume π = CRT. Q28. Which shows abnormal molar mass? NaCl Benzoic acid in benzene Glucose Urea Association due to H-bonding. Q29. Cryoscopic constant depends on: Solute Solvent Temperature Pressure Kf is solvent property. Q30. Which solution obeys Raoult’s law most closely? Benzene + Toluene Ethanol + Water Acetone + Water Chloroform + Acetone Similar intermolecular forces. Submit Paper Conclusion: Why Part 12 (Solutions) Is Extremely Valuable for NEET Aspirants The Solutions chapter plays a unique and crucial role in NEET Chemistry because it combines direct formula-based questions with deep conceptual understanding. Unlike some chapters where memorization dominates, Solutions rewards students who understand why formulas work and how different concentration terms and colligative properties are interconnected. NEET UG Chemistry Practice Paper – Part 12 is carefully structured to help students achieve exactly that level of clarity. One of the biggest advantages of Part 12 is its strong focus on core NEET scoring areas such as molarity, molality, mole fraction, Raoult’s law, Henry’s law, and colligative properties. These topics are tested almost every year in NEET, often through seemingly simple questions that can easily trap students who lack conceptual precision. By solving this paper, students learn to handle these frequently repeated question types with confidence and accuracy. Another major strength of Part 12 is its emphasis on colligative properties, a topic where many aspirants lose marks despite knowing the formulas. Concepts like elevation of boiling point, depression of freezing point, osmotic pressure, and relative lowering of vapour pressure are not difficult individually—but confusion often arises when electrolytes, Van’t Hoff factor, association, or dissociation come into play. This paper systematically exposes students to such scenarios, ensuring they understand how particle count directly affects observable properties. Part 12 also plays a vital role in building clarity around abnormal molar mass determination. Questions involving association (such as benzoic acid in benzene) or dissociation (electrolytes in aqueous solution) are classic NEET favourites. Practicing these questions helps students avoid one of the most common mistakes in the exam—blindly

Chemical & Ionic Equilibrium NEET UG Practice Paper NEET UG – Chemistry Practice Paper (Previous Years’ Questions) Part 11 | Topic: Chemical & Ionic Equilibrium Total Questions: 30 | Total Marks: 120 Q1. Chemical equilibrium is: Static Dynamic Irreversible Complete Forward and backward reactions occur simultaneously. Q2. The equilibrium constant depends on: Initial concentration Catalyst Temperature Pressure K depends only on temperature. Q3. For reaction aA + bB ⇌ cC + dD, Kc is: [A]ᵃ[B]ᵇ/[C]ᶜ[D]ᵈ [C]ᶜ[D]ᵈ/[A]ᵃ[B]ᵇ ([A]+[B])/([C]+[D]) Independent of concentration Products over reactants. Q4. Value of K >> 1 indicates: Reactants favored Products favored Reaction stops No reaction Equilibrium lies towards products. Q5. Le Chatelier’s principle applies when: System is at equilibrium Reaction is complete Catalyst is added Temperature is constant Applies only to equilibrium systems. Q6. Addition of catalyst: Changes equilibrium constant Shifts equilibrium Speeds up attainment of equilibrium Stops reaction Catalyst does not change position of equilibrium. Q7. For exothermic reaction, increase in temperature: Favours products Favours reactants No effect Stops equilibrium Heat acts as a product. Q8. Relationship between Kp and Kc is: Kp = KcRT Kp = Kc(RT)ⁿ Kp = Kc/RT Kp = Kc n = Δmoles of gaseous species. Q9. pH of pure water at 25°C is: 1 7 14 0 Neutral water has pH 7. Q10. Which is a strong acid? CH₃COOH H₂CO₃ HCl HF HCl ionises completely. Q11. Ionic product of water at 25°C is: 10⁻⁷ 10⁻¹⁴ 10⁻⁶ 1 Kw = 10⁻¹⁴. Q12. Buffer solution resists change in: Volume Pressure pH Temperature Buffer maintains pH. Q13. Which is an acidic buffer? NH₄OH + NH₄Cl NaOH + NaCl CH₃COOH + CH₃COONa HCl + NaCl Weak acid + its salt. Q14. Solubility product is applicable to: Soluble salts Sparingly soluble salts Gases Acids Applies to low-solubility salts. Q15. Precipitation occurs when: Q < Ksp Q = Ksp Q > Ksp Q = 0 Ionic product exceeds Ksp. Q16. pH of 10⁻³ M HCl is: 1 2 3 11 pH = −log[H⁺]. Q17. Common ion effect reduces: Solubility pH Pressure Volume Presence of common ion suppresses dissociation. Q18. Strong base among the following is: NH₄OH NaOH Al(OH)₃ Mg(OH)₂ NaOH dissociates completely. Q19. For weak acid, pH depends on: Ka only Concentration only Ka and concentration Temperature only pH = ½(pKa − log C). Q20. Which salt hydrolyses in water? NaCl KNO₃ NH₄Cl Na₂SO₄ Salt of weak base + strong acid. Q21. Equilibrium constant for reverse reaction is: Same Square Reciprocal Zero Kreverse = 1/Kforward. Q22. Increasing pressure favours side with: More moles of gas Less moles of gas No gas Equal moles Le Chatelier’s principle. Q23. pOH + pH equals: 7 10 14 1 At 25°C, pH + pOH = 14. Q24. Which is a weak electrolyte? HCl NaCl CH₃COOH KOH Partially ionises. Q25. Degree of dissociation increases with: Increase in concentration Decrease in dilution Increase in dilution Increase in pressure Ostwald’s dilution law. Q26. Which salt gives basic solution? NH₄Cl Na₂CO₃ NaCl KNO₃ Salt of strong base + weak acid. Q27. Equilibrium constant is dimensionless when: Kp used Activities used Concentrations used Pressures used Activities are unitless. Q28. Which salt will precipitate first? Lowest Ksp Highest Ksp Equal Ksp Depends on pH only Lower Ksp → earlier precipitation. Q29. pH of acidic buffer is: < 7 > 7 = 7 14 Acidic buffer has pH less than 7. Q30. Equilibrium shifts when: Concentration changes Pressure changes Temperature changes All of these Any stress shifts equilibrium. Submit Paper Conclusion: Why Part 11 (Chemical & Ionic Equilibrium) Is a Must-Master Section for NEET Aspirants NEET UG Chemistry Practice Paper – Part 11, focused on Chemical Equilibrium and Ionic Equilibrium, targets one of the most concept-sensitive and repeatedly tested areas of Physical Chemistry. This chapter plays a crucial role in NEET because it connects fundamental ideas of reversibility, reaction direction, acids–bases, buffers, solubility, and equilibrium shifts—all of which demand clarity rather than rote memorization. The biggest strength of Part 11 lies in its balanced integration of chemical equilibrium and ionic equilibrium concepts. NEET often mixes these ideas within the same paper, and students who treat them separately tend to struggle. This practice paper trains aspirants to smoothly move between equilibrium constants, Le Chatelier’s principle, pH calculations, buffers, common ion effect, and solubility product—exactly as required in the actual exam. Part 11 strongly reinforces core NEET scoring concepts such as the dependence of equilibrium constant on temperature, the effect of pressure and concentration changes, Kc–Kp relationships, and equilibrium direction prediction. On the ionic equilibrium side, it builds confidence in pH, pOH, Kw, Ka, Kb, buffer solutions, salt hydrolysis, and Ksp-based precipitation logic. These are high-frequency areas where NEET questions are often simple in appearance but unforgiving of weak fundamentals. Another key benefit of this paper is its focus on conceptual traps. Many students lose marks due to confusion between equilibrium shift and equilibrium constant, misunderstanding buffer action, or incorrect interpretation of common ion effect. By solving these carefully framed MCQs, students learn to avoid such mistakes and develop a sharper analytical approach. The instant explanation-based feedback ensures that errors are corrected immediately, preventing misconceptions from becoming habits. This is especially important in equilibrium-related topics, where a single wrong assumption can affect multiple questions. Part 11 also helps students build exam temperament by handling a full mixed set of equilibrium questions in one sitting. This improves time management, confidence, and decision-making under pressure—skills that directly impact NEET performance. In conclusion, Part 11 is not just a revision exercise; it is a concept-stabilizing and accuracy-building tool. It strengthens fundamentals, sharpens logical thinking, and prepares students to handle equilibrium-based NEET questions with confidence. For aspirants aiming to secure maximum marks in Physical Chemistry, mastering Chemical and Ionic Equilibrium through Part 11 is an essential step toward NEET success.

Attempt this Chemical Kinetics NEET UG – Chemistry Practice Paper. Part 10 | Topic: Chemical Kinetics Total Questions: 30 | Total Marks: 120 Q1. Rate of a chemical reaction depends on: Thermodynamic stability Nature of reactants Enthalpy change Entropy change Reaction rate depends on nature and concentration of reactants. Q2. Unit of rate constant for first order reaction is: mol L⁻¹ s⁻¹ s⁻¹ L mol⁻¹ s⁻¹ mol⁻¹ L s⁻¹ First order rate constant has unit s⁻¹. Q3. Half-life of a first order reaction is: Directly proportional to concentration Independent of concentration Inversely proportional to concentration Dependent on pressure Half-life of first order reaction is constant. Q4. For zero order reaction, rate is: Proportional to concentration Inversely proportional to concentration Independent of concentration Dependent on pressure only Rate = k for zero order reaction. Q5. Which plot is linear for first order reaction? Concentration vs time log(concentration) vs time Rate vs concentration Pressure vs time log[A] vs time gives straight line. Q6. Which factor does NOT affect reaction rate? Temperature Catalyst Concentration Free energy Free energy affects spontaneity, not rate. Q7. Arrhenius equation relates rate constant with: Concentration Pressure Temperature Volume k = Ae⁻ᴱᵃ/RT. Q8. Activation energy is: Energy of products Energy of reactants Energy barrier for reaction Enthalpy change Minimum energy required for reaction. Q9. Catalyst works by: Increasing ΔH Decreasing ΔG Lowering activation energy Increasing entropy Catalyst lowers activation energy. Q10. Which reaction is first order? Decomposition of NH₃ Radioactive decay Esterification Neutralisation Radioactive decay follows first order kinetics. Q11. Unit of rate of reaction is: mol L⁻¹ s⁻¹ mol L⁻¹ s⁻¹ L mol⁻¹ Rate = change in concentration per unit time. Q12. Half-life of zero order reaction depends on: Rate constant only Initial concentration Temperature only Pressure t½ ∝ initial concentration. Q13. Molecularity of a reaction is: Always equal to order Can be fractional Number of reacting species Depends on catalyst Defined for elementary reactions only. Q14. Order of reaction can be: Zero Fractional Negative All of these Order can take any value. Q15. Which graph gives activation energy? log k vs 1/T k vs T concentration vs time rate vs concentration Slope = −Ea/2.303R. Q16. Pseudo first order reaction example is: Ester hydrolysis Saponification Neutralisation Combustion Water concentration remains constant. Q17. Rate law is determined by: Balanced equation Experimental data Stoichiometry Thermodynamics Order is experimentally determined. Q18. For first order reaction, time for 75% completion is: t½ 2t½ 3t½ 4t½ 75% = two half-lives. Q19. Increasing temperature increases rate because: ΔH changes More collisions exceed Ea Volume decreases Pressure increases More molecules cross activation energy. Q20. Slowest step in a reaction is: Initiation Rate determining step Termination Propagation Controls overall rate. Q21. Rate constant depends on: Concentration Temperature Pressure Volume k increases with temperature. Q22. Which reaction has constant half-life? Zero order First order Second order Third order Independent of concentration. Q23. Units of rate constant for zero order reaction: s⁻¹ L mol⁻¹ s⁻¹ mol L⁻¹ s⁻¹ Dimensionless Same as rate unit. Q24. Which increases reaction rate? Decrease temperature Increase surface area Decrease catalyst Decrease concentration More surface → more collisions. Q25. Collision theory applies best to: Solid reactions Gaseous reactions Ionic reactions Enzymatic reactions Assumes gaseous molecules. Q26. Which factor affects frequency factor A? Orientation Pressure Temperature Concentration Proper orientation increases A. Q27. Rate constant is independent of: Temperature Catalyst Concentration Nature of reaction k does not depend on concentration. Q28. Which reaction has negative order? Ester hydrolysis Ozone decomposition Enzyme inhibition Combustion Inhibitor reduces rate. Q29. Rate determining step has: Lowest activation energy Highest activation energy No activation energy No role Slowest step has highest Ea. Q30. Which statement is correct? Fast reactions are always spontaneous Slow reactions are non-spontaneous Rate and spontaneity are independent Catalyst changes ΔG Kinetics and thermodynamics are independent. Submit Paper Conclusion: Why this Chemical Kinetics NEET UG – Chemistry Practice Paper is good for NEET Aspirants. NEET UG Chemistry Practice Paper – Part 10, focused on Chemical Kinetics, addresses one of the most logic-driven and concept-testing chapters in Physical Chemistry. Unlike calculation-heavy topics, Chemical Kinetics rewards students who clearly understand reaction rates, orders, mechanisms, and the role of activation energy—making it a powerful scoring area when practiced correctly. Part 10 helps students clearly differentiate between rate of reaction and spontaneity, a common source of confusion in NEET. Through well-structured MCQs, aspirants learn that fast reactions are not necessarily spontaneous and slow reactions are not necessarily non-spontaneous. This conceptual clarity is crucial because NEET frequently tests such distinctions in indirect ways. The paper strongly reinforces core kinetics concepts such as rate laws, order and molecularity of reactions, half-life expressions, Arrhenius equation, activation energy, and the effect of temperature and catalysts. These are repeatedly asked themes in NEET, and regular practice ensures students can recall definitions, formulas, and graphs instantly under exam pressure. Another key benefit of Part 10 is its emphasis on graph-based and interpretation questions, such as identifying reaction order from plots or extracting activation energy from Arrhenius graphs. These question types often intimidate students, but consistent exposure builds confidence and speed, reducing hesitation during the actual exam. Part 10 also sharpens analytical thinking by including questions on pseudo-first-order reactions, rate-determining steps, collision theory, and frequency factors. These topics require understanding rather than memorization, and mastering them helps students tackle twisted or application-based NEET questions with ease. The instant explanation-based feedback ensures that every incorrect attempt becomes a learning opportunity. Misconceptions about half-life, units of rate constants, or factors affecting reaction rate are corrected immediately, leading to stronger long-term retention and fewer repeated mistakes. Overall, Part 10 functions as a precision-building practice tool. It improves conceptual clarity, enhances speed and accuracy, strengthens graph interpretation skills, and builds confidence in one of NEET’s most reliable scoring chapters. For aspirants aiming to maximize marks in Physical Chemistry, mastering Chemical Kinetics through Part 10 is a smart and essential step toward NEET success. Learn more about Chemical Kinetics: https://en.wikipedia.org/wiki/Chemical_kinetics Attempt More NEET Chemistry Papers Here: https://odtutor.com/category/neet-practice-papers/

NEET UG Electrochemistry PYQs practice paper helps aspirants strengthen concepts and exam readiness. Topic-wise previous year questions provide clarity, accuracy, and confidence. This focused resource ensures effective preparation for Chemistry, guiding students toward success in competitive exams with structured problem-solving.Total Questions: 30 | Marks: 120📌 One of the most scoring Physical Chemistry chapters in NEET NEET UG – Chemistry Practice Paper (Previous Years’ Questions) Part 9 | Topic: Electrochemistry Total Questions: 30 | Total Marks: 120 Q1. The unit of electrical conductivity is: ohm ohm⁻¹ cm⁻¹ volt ampere Conductivity is measured in ohm⁻¹ cm⁻¹. Q2. Which cell converts chemical energy into electrical energy? Electrolytic cell Galvanic cell Fuel cell Both (b) and (c) Both galvanic and fuel cells generate electricity. Q3. EMF of a cell is: Always negative Potential at cathode Difference between electrode potentials Same as current EMF = E°cathode − E°anode. Q4. Which ion has the highest molar conductivity? Na⁺ K⁺ H⁺ Li⁺ H⁺ moves by Grotthuss mechanism. Q5. Which factor increases the conductivity of an electrolyte? Decrease in temperature Increase in dilution Increase in viscosity Decrease in ionization More ion mobility at higher dilution. Q6. Standard electrode potential of hydrogen is: 1 V −1 V 0 V 0.5 V SHE is assigned zero potential. Q7. Which metal is most easily oxidised? Cu Ag Zn Au Zn has most negative reduction potential. Q8. Which law relates mass deposited to charge passed? Ohm’s law Kohlrausch’s law Faraday’s first law Hess’s law Faraday’s first law of electrolysis. Q9. In a galvanic cell, oxidation occurs at: Cathode Anode Salt bridge Electrolyte Oxidation always occurs at anode. Q10. Role of salt bridge is to: Increase EMF Maintain electrical neutrality Increase current Stop oxidation It balances charge in half-cells. Q11. Which cell has highest efficiency? Dry cell Fuel cell Lead storage cell Mercury cell Fuel cells have very high efficiency. Q12. Which equation relates EMF with equilibrium constant? Arrhenius equation Nernst equation Van’t Hoff equation Gibbs equation Nernst equation connects E and K. Q13. Which solution shows highest molar conductivity at infinite dilution? NaCl KCl HCl CH₃COOH H⁺ and Cl⁻ have high mobility. Q14. Which reaction occurs at cathode? Oxidation Reduction Neutralisation Displacement Reduction occurs at cathode. Q15. Which metal is protected by cathodic protection? Magnesium Zinc Iron Aluminium Iron structures are protected using Zn/Mg. Q16. Corrosion of iron is an example of: Oxidation Reduction Redox reaction Neutralisation Both oxidation and reduction occur. Q17. Unit of EMF is: Ohm Volt Ampere Coulomb EMF is measured in volts. Q18. Which battery is rechargeable? Dry cell Mercury cell Lead storage cell Fuel cell Lead storage battery is rechargeable. Q19. Which ion migrates fastest in solution? Na⁺ K⁺ H⁺ NH₄⁺ H⁺ shows proton hopping. Q20. Which law states conductivity is sum of ionic contributions? Ohm’s law Faraday’s law Kohlrausch’s law Nernst law Kohlrausch’s law of independent migration. Q21. Which metal acts as sacrificial anode? Copper Silver Zinc Gold Zinc protects iron by oxidising itself. Q22. Electrolysis of molten NaCl gives: Na at cathode Cl₂ at anode Both (a) and (b) NaCl remains unchanged Na and Cl₂ are liberated. Q23. Which factor does NOT affect EMF? Nature of electrodes Concentration Temperature Size of electrodes Electrode size does not affect EMF. Q24. Standard conditions mean: 1 atm, 298 K 1 bar, 298 K 1 bar, 273 K 1 atm, 273 K Standard state uses 1 bar. Q25. Which equation gives relation between ΔG° and EMF? ΔG° = −nFE° ΔG° = nFE° ΔG° = RT ln K ΔG° = q + w ΔG° = −nFE°. Q26. Which electrolyte is weakest? HCl NaOH CH₃COOH KOH Weak acid partially ionises. Q27. Which gas is evolved at anode during electrolysis of water? Hydrogen Oxygen Chlorine Nitrogen Oxidation gives oxygen at anode. Q28. Which metal has highest standard reduction potential? Zn Cu Ag Fe Ag is least reactive metal here. Q29. Which battery is used in automobiles? Dry cell Mercury cell Lead storage battery Fuel cell Lead storage battery is used in cars. Q30. Which process prevents rusting? Oxidation Galvanization Corrosion Reduction Zinc coating prevents corrosion. Submit Paper Conclusion: Why Part 9 (Electrochemistry) Is a Must-Solve Section for NEET Aspirants NEET UG Chemistry Practice Paper – Part 9, focused on Electrochemistry, targets one of the most high-scoring yet concept-sensitive chapters in Physical Chemistry. Electrochemistry has a consistent presence in NEET, and questions from this chapter often decide whether a student moves from an average Chemistry score to an excellent one. The biggest strength of Part 9 is its balanced coverage of theory, application, and logic-based questions. NEET does not test Electrochemistry only through numerical problems; it also evaluates conceptual understanding of galvanic cells, electrolytic cells, electrode potentials, corrosion, batteries, fuel cells, and conductivity. This paper reflects that exact pattern, ensuring students are prepared for every possible question type. By solving Part 9, students develop clarity in core electrochemical concepts such as oxidation and reduction, anode and cathode behavior, EMF calculation, standard electrode potentials, and the role of salt bridges. These are areas where many aspirants make avoidable mistakes due to sign confusion or weak conceptual foundations. Repeated exposure through well-structured MCQs helps eliminate such errors permanently. Another major advantage of this paper is its focus on high-yield NEET formulas and relationships, including the Nernst equation, Faraday’s laws of electrolysis, Kohlrausch’s law, and the relationship between Gibbs free energy and EMF. Practicing these questions improves a student’s ability to recall formulas instantly and apply them correctly under time pressure—an essential exam-day skill. Part 9 also strengthens real-world application understanding, especially through questions on corrosion, galvanization, batteries, fuel cells, and industrial electrolysis. NEET increasingly includes application-based questions, and this paper prepares students to handle them confidently without rote learning. The instant explanation-based feedback after submission ensures that every mistake becomes a learning opportunity. Instead of repeating the same errors across multiple tests, students can immediately correct misconceptions related to electrode reactions, ion mobility, or conductivity trends. This significantly improves long-term retention and accuracy. Equally important is the exam temperament built through this paper. Solving

Total Questions: 30 | Marks: 120📌 One of the most frequently tested Physical Chemistry topics in NEET NEET UG – Chemistry Practice Paper (Previous Years’ Questions) Part 8 | Topic: Thermodynamics & Thermochemistry Total Questions: 30 | Total Marks: 120 Q1. Which thermodynamic quantity determines spontaneity of a reaction? ΔH ΔS ΔG Heat A reaction is spontaneous if ΔG is negative. Q2. The unit of entropy is: J mol⁻¹ J K⁻¹ J mol⁻¹ K⁻¹ kJ mol⁻¹ Entropy is energy per mole per kelvin. Q3. Which process is always spontaneous? Endothermic reaction Exothermic reaction Increase in entropy of universe Decrease in entropy Second law: entropy of universe increases. Q4. For an exothermic reaction, ΔH is: Positive Negative Zero Infinite Heat is released, so ΔH is negative. Q5. Enthalpy change of a reaction depends on: Path Catalyst Initial and final states Temperature only Enthalpy is a state function. Q6. Which law states that energy can neither be created nor destroyed? Zeroth law First law Second law Third law First law of thermodynamics. Q7. ΔG = 0 indicates: Spontaneous reaction Non-spontaneous reaction Equilibrium Endothermic reaction ΔG = 0 at equilibrium. Q8. Which has maximum entropy? Solid Liquid Gas Plasma Gas has maximum randomness. Q9. Standard enthalpy of formation is defined for: 1 mole of compound Elements in standard state Both None Formation of 1 mole of compound. Q10. Which is a state function? Heat Work Internal energy Path length Internal energy depends only on state. Q11. Unit of work in thermodynamics is: Joule Pascal Newton Watt Work is measured in joules. Q12. Which process is endothermic? Freezing Condensation Vaporization Crystallisation Heat is absorbed during vaporization. Q13. Which thermodynamic function is always positive? ΔG ΔH ΔS(universe) Work Entropy of universe always increases. Q14. At absolute zero, entropy of a perfect crystal is: Maximum Zero Infinite Constant Third law of thermodynamics. Q15. Which condition favours spontaneity? ΔH +, ΔS − ΔH −, ΔS + ΔH +, ΔS + ΔH −, ΔS − Always spontaneous at all temperatures. Q16. Heat absorbed at constant pressure equals: ΔU ΔH Work ΔS ΔH = qp. Q17. Which is an extensive property? Temperature Density Volume Pressure Depends on amount of substance. Q18. Which process results in maximum increase in entropy? Solid → Liquid Liquid → Gas Solid → Gas Gas → Liquid Direct solid to gas gives maximum disorder. Q19. Hess’s law is based on: First law Second law Third law Zeroth law Energy conservation principle. Q20. For an isolated system, which remains constant? Energy Entropy Volume Temperature No exchange of energy with surroundings. Q21. Work done during free expansion of gas is: Maximum Minimum Zero Infinite No opposing pressure. Q22. Which quantity is path dependent? Enthalpy Entropy Internal energy Work Work depends on process path. Q23. If ΔH = 0 and ΔS > 0, reaction is spontaneous: At low temperature At high temperature At all temperatures Never ΔG = −TΔS is always negative. Q24. Which term measures randomness? Enthalpy Entropy Free energy Heat Entropy measures disorder. Q25. Which condition gives ΔG < 0? ΔH − TΔS < 0 ΔH + TΔS < 0 ΔH − ΔS < 0 ΔS − TΔH < 0 ΔG = ΔH − TΔS. Q26. Which law explains equilibrium between systems? Zeroth law First law Second law Third law Zeroth law defines thermal equilibrium. Q27. Which process occurs at constant enthalpy? Free expansion Joule–Thomson expansion Isothermal expansion Adiabatic compression Joule–Thomson process is isenthalpic. Q28. Which reaction has ΔG > 0? Spontaneous Non-spontaneous At equilibrium Exothermic Positive ΔG means non-spontaneous. Q29. Which quantity is conserved in chemical reactions? Mass Energy Both None Both mass and energy are conserved. Q30. Entropy change is maximum when: Order increases Disorder increases Energy decreases Temperature decreases Entropy increases with disorder. Submit Paper Conclusion: Why Part 8 (Thermodynamics & Thermochemistry) Is Crucial for NEET Chemistry Mastery NEET UG Chemistry Practice Paper – Part 8, focused on Thermodynamics and Thermochemistry, targets one of the most conceptually important and frequently tested areas of Physical Chemistry in NEET. This chapter is not just about formulas—it is about understanding how and why chemical reactions occur, which makes it a core decision-making topic in the exam. The primary strength of Part 8 lies in its emphasis on fundamental thermodynamic principles such as the first, second, and third laws of thermodynamics, Gibbs free energy, entropy, enthalpy, and spontaneity. NEET often frames questions that appear simple but test deep clarity—such as identifying conditions for spontaneity, interpreting ΔG values, or understanding entropy changes during phase transitions. Practicing these questions helps students develop conceptual precision, which is essential for avoiding careless errors. Part 8 also strengthens a student’s ability to analyze reactions beyond heat change. Many students wrongly associate exothermic reactions with spontaneity, but this paper reinforces the correct understanding that spontaneity depends on both enthalpy and entropy. This clarity is critical, as NEET frequently includes trap-based questions that exploit such misconceptions. Another major advantage of this practice set is its focus on real NEET-style logic questions—covering state functions vs. path functions, entropy trends, equilibrium conditions (ΔG = 0), Hess’s law, and thermodynamic processes like free expansion and Joule–Thomson expansion. These questions train students to think conceptually rather than memorize, which significantly improves performance in unfamiliar or twisted MCQs. Part 8 also plays an important role in building calculation confidence without overwhelming students. The balance between theory-based and numerically light questions helps aspirants strengthen understanding while maintaining speed—an essential factor in a time-bound exam like NEET. The inclusion of instant explanations after submission ensures that mistakes are corrected immediately. This prevents long-term conceptual gaps and improves retention, especially in abstract topics like entropy and free energy, which students often find difficult. In conclusion, Part 8 acts as a concept-strengthening and clarity-building tool. It helps students master the logic behind chemical reactions, improves accuracy in Physical Chemistry, and builds confidence in one of NEET’s most scoring yet misunderstood chapters. For aspirants aiming to secure every possible mark in Chemistry, thorough practice of Thermodynamics through Part 8 is not optional—it is

Part 7 | Topic: Chemical Bonding & Molecular Structure Total Questions: 30 | Total Marks: 120 Q1. Which bond is the strongest? Single bond Double bond Triple bond Hydrogen bond Triple bond has maximum bond energy. Q2. Which molecule has zero dipole moment? NH₃ H₂O CO₂ SO₂ Linear CO₂ cancels dipole moments. Q3. Hybridisation of carbon in methane is: sp sp² sp³ dsp² Methane has tetrahedral geometry. Q4. Which molecule is trigonal planar? NH₃ BF₃ H₂O PCl₃ BF₃ is sp² hybridised. Q5. Which orbital has maximum penetration power? s p d f s-orbital penetrates closest to nucleus. Q6. Which species is paramagnetic? N₂ O₂ CO₂ H₂ O₂ has unpaired electrons. Q7. Bond order of O₂⁺ is: 1 1.5 2 2.5 Removal of electron increases bond order. Q8. Which compound shows hydrogen bonding? H₂S NH₃ PH₃ HCl NH₃ has N–H bonds. Q9. Which has highest bond angle? CH₄ NH₃ H₂O CO₂ Linear CO₂ has 180° bond angle. Q10. Which bond is most polar? C–H N–H O–H F–H Maximum electronegativity difference. Q11. Shape of SF₆ is: Tetrahedral Trigonal bipyramidal Octahedral Square planar Six bond pairs around sulphur. Q12. Which molecule is bent in shape? CO₂ SO₂ BF₃ BeCl₂ Lone pair causes bending. Q13. Which compound has sp hybridisation? Ethene Ethyne Ethane Benzene Ethyne has linear geometry. Q14. Which ion is isoelectronic with neon? Na⁺ Mg²⁺ F⁻ All of these All have 10 electrons. Q15. Which interaction is weakest? Covalent bond Ionic bond Hydrogen bond Van der Waals force Van der Waals forces are weakest. Q16. Which molecule has square planar geometry? XeF₄ SF₆ PCl₅ NH₃ XeF₄ has two lone pairs. Q17. Which has maximum lattice energy? NaCl KCl MgO CsCl Higher charge and smaller size. Q18. Which molecule is linear? H₂O NH₃ CO₂ SO₂ CO₂ has sp hybridisation. Q19. Which compound shows resonance? Ethane Ethene Benzene Methane Delocalized π electrons. Q20. Which has highest bond dissociation energy? F–F Cl–Cl O=O N≡N Triple bond in nitrogen is strongest. Q21. Which bond is present in interhalogen compounds? Ionic Covalent Hydrogen Metallic Interhalogens are covalent. Q22. Which molecule is pyramidal? BF₃ NH₃ CO₂ BeCl₂ Lone pair on nitrogen. Q23. Which species is diamagnetic? O₂ NO N₂ NO₂ All electrons are paired. Q24. Which compound has highest polarity? CCl₄ CO₂ NH₃ BF₃ Asymmetric pyramidal structure. Q25. Which hybridisation gives linear geometry? sp sp² sp³ dsp² sp hybridisation → 180°. Q26. Which molecule has tetrahedral geometry? NH₃ CH₄ H₂O SO₂ CH₄ is sp³ hybridised. Q27. Which bond angle is smallest? CH₄ NH₃ H₂O CO₂ Two lone pairs reduce angle most. Q28. Which species has maximum bond order? O₂ O₂⁺ O₂⁻ O₂²⁻ Removal of antibonding electron. Q29. Which interaction is responsible for boiling of liquids?

Total Questions: 30 | Total Marks: 120 Q1. Which thermodynamic parameter predicts spontaneity of a reaction? ΔH ΔS ΔG Heat Negative Gibbs free energy indicates spontaneity. Q2. Which orbital has maximum penetration power? s p d f s-orbitals penetrate closest to nucleus. Q3. Which of the following is an extensive property? Temperature Pressure Density Volume Volume depends on amount of substance. Q4. Which species is diamagnetic? O₂ NO N₂ NO₂ All electrons in N₂ are paired. Q5. Which solution will show maximum lowering of vapour pressure? 0.1M glucose 0.1M urea 0.1M NaCl 0.1M CaCl₂ CaCl₂ gives maximum number of particles. Q6. Which element shows maximum atomic radius? Na K Rb Cs Atomic size increases down the group. Q7. Which gas deviates least from ideal behavior? NH₃ CO₂ He SO₂ Helium has negligible intermolecular forces. Q8. Which compound shows strongest hydrogen bonding? NH₃ H₂O HF CH₃OH Water forms extensive hydrogen-bonded network. Q9. Which compound undergoes SN1 reaction most easily? CH₃Cl C₂H₅Cl (CH₃)₃CCl C₆H₅Cl Tertiary carbocation is most stable. Q10. Which reaction shows zero-order kinetics? Radioactive decay Photochemical reaction Ester hydrolysis SN2 reaction Rate depends only on light intensity. Q11. Which metal is strongest reducing agent in aqueous solution? Na K Li Cs Highest hydration energy of Li⁺. Q12. Which compound shows resonance stabilization? Ethane Ethene Benzene Propane π-electron delocalization in benzene. Q13. Which salt undergoes hydrolysis? NaCl KNO₃ NH₄Cl Na₂SO₄ Salt of weak base and strong acid. Q14. Which metal is extracted by leaching? Iron Aluminium Gold Zinc Gold extraction uses cyanide leaching. Q15. Which compound acts as local anesthetic? Chloroform Ether Lidocaine Aspirin Lidocaine is a local anesthetic. Q16. Which compound has highest boiling point? CH₄ NH₃ H₂O HF Strong hydrogen bonding in water. Q17. Which element has highest electron affinity? F Cl Br I Chlorine has highest electron affinity. Q18. Which compound gives iodoform test? Ethanol Methanol Propanol Phenol Ethanol forms CH₃CO– group on oxidation. Q19. Which oxide is amphoteric? Na₂O MgO Al₂O₃ SO₃ Al₂O₃ reacts with acids and bases. Q20. Which gas is known as producer gas? CO + H₂ CO + N₂ CH₄ + H₂ CO₂ + N₂ Producer gas = CO + N₂. Q21. Which compound has linear geometry? CO₂ SO₂ NH₃ H₂O CO₂ is linear. Q22. Which process decreases entropy? Melting Vaporisation Condensation Dissolution Gas to liquid reduces disorder. Q23. Which electrolyte has highest molar conductivity at infinite dilution? NaCl HCl CH₃COOH NH₄OH H⁺ has very high ionic mobility. Q24. Which compound is used as antacid? NaOH Mg(OH)₂ HCl NH₄OH Milk of magnesia neutralizes excess acid. Q25. Which compound shows optical isomerism? 2-bromopropane 2-butanol Ethanol Propane Has chiral carbon atom. Q26. Which compound is strongest oxidising agent? KMnO₄ K₂Cr₂O₇ H₂O₂ O₃ Ozone is a very strong oxidising agent. Q27. Which metal is liquid near room temperature? Cs Ga Hg All of these Cs, Ga, and Hg melt near room temperature. Q28. Which compound causes temporary hardness of water? CaCl₂ MgSO₄ Ca(HCO₃)₂ Na₂CO₃ Bicarbonates cause temporary hardness. Q29. Which polymer is used for non-stick cookware? PVC Bakelite Teflon Nylon Teflon is chemically inert and non-stick. Q30. Which process leads to maximum increase in entropy? Solid → Liquid Liquid → Gas Solid → Gas Gas → Liquid Solid to gas shows maximum disorder. Submit Paper Conclusion: Why Part 5 Practice Strengthens NEET Chemistry Performance NEET UG Chemistry Practice Paper – Part 5 (Miscellaneous) is designed to push students one step closer to real NEET readiness by reinforcing concept integration, accuracy, and exam confidence. By the time aspirants reach Part 5, the goal is no longer just understanding concepts—but mastering their application under mixed and unpredictable conditions, exactly as required in the actual NEET examination. The greatest strength of Part 5 lies in its advanced consolidation approach. The questions compel students to recall ideas from Physical, Organic, and Inorganic Chemistry simultaneously, encouraging them to connect concepts rather than treat chapters as isolated units. This integrated practice significantly improves concept retention, which is crucial during long exams when mental fatigue can cause even well-prepared students to make mistakes. Part 5 also focuses heavily on high-yield NEET themes such as thermodynamics, chemical equilibrium, colligative properties, electrochemistry, bonding trends, reaction mechanisms, stereochemistry, environmental chemistry, and real-life chemical applications. These areas consistently appear in NEET, and repeated exposure through well-structured questions ensures students are prepared for both direct and twisted versions of such problems. Another key benefit of solving Part 5 is the development of decision-making speed. NEET Chemistry often provides options that are closely related, where hesitation can cost valuable seconds. Practicing these questions helps students learn how to identify the key concept quickly, eliminate incorrect options confidently, and arrive at the correct answer without overthinking. The inclusion of clear explanations after each question transforms mistakes into learning opportunities. Instead of simply knowing whether an answer is right or wrong, students understand why it is so. This prevents the repetition of conceptual errors and strengthens long-term understanding—an essential requirement for consistent scoring across multiple mock tests and the final exam. Part 5 also plays a critical role in building exam temperament. Attempting a full 30-question mixed set in one sitting improves focus, stamina, and mental discipline. Students become comfortable handling pressure, managing time effectively, and maintaining accuracy even in the later stages of a practice session—skills that directly translate to better performance on NEET exam day. In essence, Part 5 serves as a bridge between practice and performance. It sharpens conceptual clarity, enhances speed and accuracy, reinforces high-frequency NEET topics, and builds the confidence needed to tackle Chemistry as a scoring subject. For students aiming for top ranks, consistent practice with Part 5 ensures they are not just prepared—but exam-ready.

Total Questions: 30 | Total Marks: 120 Q1. Which law explains the distribution of solute between two immiscible solvents? Henry’s law Raoult’s law Nernst distribution law Dalton’s law Nernst distribution law governs solute distribution. Q2. Which quantum number determines the orientation of an orbital? n l m s Magnetic quantum number determines orientation. Q3. Which of the following is an intensive property? Volume Mass Temperature Enthalpy Temperature does not depend on amount. Q4. Which species has highest bond order? N₂ N₂⁺ N₂⁻ N₂²⁻ Removal of electron increases bond order. Q5. Which compound will show maximum ionisation in water? CH₃COOH NH₄OH HCl H₂CO₃ HCl is a strong acid. Q6. Which compound has maximum lattice energy? NaF NaCl KCl CsCl

Part 1 | Topic: Miscellaneous Total Questions: 30 | Total Marks: 120 Q1. Which of the following is a state function? Heat Work Enthalpy Path length Enthalpy depends only on initial and final states. Q2. SI unit of entropy is: J J mol⁻¹ J K⁻¹ mol⁻¹ K J⁻¹ Entropy is measured per mole per Kelvin. Q3. Shape of an orbital depends on: Principal quantum number Azimuthal quantum number Magnetic quantum number Spin quantum number Azimuthal quantum number determines shape. Q4. Maximum deviation from ideal gas behavior is shown by: He H₂ NH₃ Ne NH₃ has strong intermolecular forces. Q5. Pseudo first order reaction is: Ester hydrolysis N₂O₅ decomposition Radioactive decay Combination reaction Water in excess makes it pseudo-first order. Q6. Highest lattice energy is shown by: NaCl KCl CsCl MgO Higher charge and smaller ions give higher lattice energy. Q7. Paramagnetic species is: N₂ O₂ CO NO⁺ O₂ has two unpaired electrons. Q8. Hybridization of BF₃ is: sp² sp³ sp dsp² BF₃ is trigonal planar. Q9. Which is strongest acid? HF HCl HBr HI Acid strength increases down the group. Q10. Order of reaction is equal to: Stoichiometric coefficients Molecularity Concentration Sum of powers of concentration terms Order is experimentally determined. Q11. Which colligative property depends on number of particles? Osmotic pressure Viscosity Surface tension Density Osmotic pressure depends only on particle number. Q12. Which metal has highest electrical conductivity? Cu Ag Fe Al Silver has highest conductivity. Q13. Which is not a buffer solution? CH₃COOH + CH₃COONa NH₄OH + NH₄Cl HCl + NaCl H₂CO₃ + NaHCO₃ Strong acid + salt does not form buffer. Q14. Which shows hydrogen bonding? H₂S PH₃ HCl HF HF has strong hydrogen bonding. Q15. Which catalyst is used in Haber process? Pt Fe Ni V₂O₅ Iron catalyst with promoters. Q16. Which compound shows maximum boiling point? H₂O NH₃ H₂S PH₃ Strong hydrogen bonding in water. Q17. Which law relates pressure and volume? Charles law Gay Lussac law Boyle’s law Avogadro law Boyle’s law: P ∝ 1/V. Q18. Which has highest bond order? O₂ O₂⁺ O₂⁻ O₂²⁻ Removal of electron increases bond order. Q19. Which is strongest oxidizing agent? F₂ Cl₂ Br₂ I₂ Fluorine has highest electronegativity. Q20. Which compound shows resonance? Benzene Methane Ethane Propane Benzene has delocalized π electrons. Q21. Which is amphoteric oxide? Na₂O MgO Al₂O₃ SO₂ Al₂O₃ reacts with acids and bases. Q22. Which solution has highest boiling point? 0.1M glucose 0.1M NaCl 0.1M urea 0.1M CaCl₂ More particles → higher elevation. Q23. Which is not a greenhouse gas? CO₂ CH₄ O₂ N₂O Oxygen is not a greenhouse gas. Q24. Which is strongest base? NaOH NH₄OH Al(OH)₃ Mg(OH)₂ NaOH is a strong base. Q25. Which has highest pH? 0.1M HCl 0.1M NaCl 0.1M NaOH 0.1M NH₄Cl Strong base gives highest pH. Q26. Which metal is liquid at room temperature? Na Ga Cs Hg Mercury is liquid at room temperature. Q27. Which compound has zero dipole moment? NH₃ CO₂ H₂O SO₂ Linear CO₂ cancels dipoles. Q28. Which gas is used in balloons? He H₂ N₂ O₂ Helium is non-flammable. Q29. Which shows maximum covalent character? NaCl KCl AlCl₃ MgCl₂ Al³⁺ has high polarizing power. Q30. Which vitamin is water soluble? Vitamin A Vitamin D Vitamin E Vitamin C Vitamin C is water soluble. Submit Paper Conclusion: Why This NEET UG Chemistry Practice Paper Is Truly Helpful This NEET UG Chemistry Practice Paper (Part 1 – Miscellaneous) has been carefully designed to serve as a high-impact revision and self-assessment tool for aspirants targeting a strong NEET score. Unlike random question sets, the questions in this paper are previous-year inspired, concept-driven, and aligned with the actual NEET examination pattern, making it highly relevant for real exam preparation. One of the biggest advantages of this paper is its “Miscellaneous” nature. NEET Chemistry often tests a student’s ability to switch quickly between Physical, Organic, and Inorganic concepts within the same section. This paper intentionally mirrors that challenge. By practicing such mixed questions, students develop mental flexibility, reduce confusion during the actual exam, and improve time management under pressure. Each question in this paper targets a foundational concept—such as thermodynamics, chemical bonding, solutions, electrochemistry, acids and bases, periodic trends, or basic organic principles. These are areas from which direct or indirect questions are repeatedly asked in NEET. Practicing these ensures that students are not just memorizing facts but understanding why an option is correct or incorrect, which is critical for tackling tricky NEET MCQs. Another key strength of this practice paper is the instant feedback mechanism. After submission, students can immediately see: This instant analysis helps in identifying weak areas quickly, reinforcing correct concepts, and preventing the repetition of common mistakes. Such immediate learning loops are far more effective than passive reading or delayed evaluation. The NEET-accurate marking scheme (4 marks per correct answer) also allows students to realistically assess their performance. This helps them track progress over time, set score benchmarks, and build confidence before attempting full-length mock tests. Importantly, this paper is also ideal for last-minute revision. Since it covers a wide range of topics in a compact format, students can use it during the final weeks or even days before the exam to quickly refresh key concepts without feeling overwhelmed. In summary, this practice paper is not just a set of questions—it is a strategic learning tool. It strengthens conceptual clarity, improves exam temperament, enhances accuracy, and builds confidence. Regular practice with such well-structured PYQ-based papers can make a significant difference between an average attempt and a high-scoring NEET Chemistry performance.