odadmin

IIT JEE Chemistry Practice Paper – Part 17: Solutions & Colligative Properties Topic: Solutions & Colligative Properties Type: Multiple Choice Questions (MCQs) Marks: +4 for each correct answer Negative Marking: 0 (Practice Mode) The molality of a solution containing 10 g of NaOH (M = 40 g/mol) dissolved in 250 g of water is: 0.5 m 1.0 m 2.0 m 3.0 m Which of the following is a colligative property? Surface tension Osmotic pressure Refractive index Viscosity Which law governs the lowering of vapour pressure for an ideal solution? Henry’s Law Raoult’s Law Dalton’s Law Boyle’s Law When a non-volatile solute is added to a solvent, the vapour pressure of the solvent: Increases Decreases Remains constant Becomes zero The osmotic pressure of a 0.1 M NaCl solution at 27°C (R = 0.0821 L·atm·K⁻¹·mol⁻¹) is approximately: 2.46 atm 4.92 atm 1.23 atm 0.82 atm Elevation of boiling point is directly proportional to: Molarity Molality Density Volume fraction Depression in freezing point (ΔTf) is given by: ΔTf = Kb·m ΔTf = Kf·m ΔTf = Kf/m ΔTf = Kb/m The van’t Hoff factor (i) accounts for: Solvent polarity Ionization or association of solute Solutions & Colligative Properties: Notes and Important Formulas A Strategic Guide for IIT-JEE Aspirants by Prof. Anil Tyagi My dear students, a solution is more than just a mixture; it is a homogeneous embodiment of molecular interactions. Understanding solutions is crucial, for it leads us to Colligative Properties—those properties that depend not on the identity of the solute particles, but solely on their number. This chapter is a hallmark of conceptual chemistry and a favorite for JEE problem-setters. Let’s build this concept from the ground up. 1. Core Definitions & Concentration Terms First, we must speak the language precisely. For JEE: Molality and Mole Fraction are preferred for colligative properties as they are independent of temperature. 2. The Foundation: Raoult’s Law For a volatile solvent in a solution containing a non-volatile solute, the governing principle is Raoult’s Law. 3. The Heart of the Chapter: Colligative Properties These are the properties that depend on the number of solute particles, not their nature. They are all consequences of the lowering of vapour pressure as stated by Raoult’s Law. For a non-volatile, non-electrolyte solute: 1. Relative Lowering of Vapour Pressure:This is the direct application of Raoult’s Law. (P⁰ – P) / P⁰ = x₂where x₂ is the mole fraction of the solute. For dilute solutions, it can be approximated as:(P⁰ – P) / P⁰ = (n₂ / n₁) ≈ (W₂ M₁) / (W₁ M₂) 2. Elevation of Boiling Point (ΔTb):Adding a solute lowers the vapour pressure, which means a higher temperature is needed to make the vapour pressure equal to the atmospheric pressure. 3. Depression of Freezing Point (ΔTf):The solute disrupts the solvent’s ability to form a solid lattice, thus freezing occurs at a lower temperature. 4. Osmotic Pressure (π):The pressure required to be applied on the solution to prevent the inward flow of pure solvent through a semi-permeable membrane. 4. The Crucial JEE Twist: The Van’t Hoff Factor (i) The formulas above are for non-electrolytes. For electrolytes that dissociate (or associate, like benzoic acid in benzene) in solution, we introduce the Van’t Hoff Factor (i). Professor Tyagi’s Key Takeaways & Problem-Solving Strategy: Internalize these principles. This chapter offers guaranteed marks if your concepts are clear and your calculations are systematic. Stay disciplined, stay focused. Your hard work will yield the ultimate colligative property—success. – Prof. Anil Tyagi

Instructions: Each question carries 4 marks. Select the correct answer and click Submit to view your score, correct answers, and explanations. Q1. The internal energy change (ΔU) for an isothermal process is: a) Positive b) Negative c) Zero d) Cannot be predicted Q2. The first law of thermodynamics is a statement of the law of conservation of: a) Mass b) Energy c) Momentum d) Entropy Q3. The enthalpy change (ΔH) and internal energy change (ΔU) are related by: a) ΔH = ΔU + ΔnRT b) ΔH = ΔU – ΔnRT c) ΔH = ΔU × ΔnRT d) ΔH = ΔU / ΔnRT Q4. The entropy of the universe in a spontaneous process: a) Decreases b) Increases c) Remains constant d) Becomes zero Q5. For an adiabatic process, which of the following is true? a) q = 0 b) ΔU = 0 c) w = 0 d) ΔH = 0 Q6. Which of the following thermodynamic quantities is a state function? a) Work b) Heat c) Internal Energy d) Both heat and work Q7. The Gibbs free energy change (ΔG) for a spontaneous process is: a) Positive b) Negative c) Zero d) Infinite Q8. Work done in an isothermal reversible expansion of an ideal gas is given by: a) w = nRT ln(V₂/V₁) b) w = –nRT ln(V₂/V₁) c) w = PΔV d) w = ΔU Q9. The condition for equilibrium in terms of Gibbs free energy is: a) ΔG > 0 b) ΔG = 0 c) ΔG < 0 d) ΔH = 0 Q10. Which of the following processes is endothermic? a) Condensation of steam b) Freezing of water c) Melting of ice d) Combustion of methane Submit IIT JEE Chemistry – Thermodynamics Summary & Formula Sheet Thermodynamics is the branch of physical chemistry that studies energy changes accompanying physical and chemical processes. It helps us understand the direction and feasibility of reactions — an essential part of IIT JEE Chemistry. 1. Basic Terms System: The part of the universe under study (e.g., reacting mixture). Surroundings: Everything outside the system. Types of Systems: Open – exchanges both matter and energy. Closed – exchanges energy but not matter. Isolated – exchanges neither energy nor matter. 2. Thermodynamic Processes Isothermal: Temperature constant (ΔT = 0). Adiabatic: No heat exchange (q = 0). Isobaric: Constant pressure. Isochoric: Constant volume. Reversible: Infinitely slow, equilibrium maintained. Irreversible: Rapid and spontaneous, not in equilibrium. 3. First Law of Thermodynamics Energy can neither be created nor destroyed; it can only be transformed. ΔU = q + w ΔU – Change in internal energy q – Heat absorbed by the system w – Work done on the system For ideal gas: w = –PextΔV At constant volume: qv = ΔU At constant pressure: qp = ΔH 4. Enthalpy (H) H = U + PV Change in enthalpy: ΔH = ΔU + PΔV For chemical reactions: ΔH = ΣHproducts – ΣHreactants Exothermic: ΔH < 0 Endothermic: ΔH > 0 5. Heat Capacities Cp – Cv = R For n moles of gas: ΔU = nCvΔT    and    ΔH = nCpΔT 6. Hess’s Law The total enthalpy change of a reaction is the same, irrespective of the path taken. ΔHoverall = ΣΔHindividual steps 7. Second Law of Thermodynamics The entropy (S) of an isolated system always increases in a spontaneous process. ΔSuniverse = ΔSsystem + ΔSsurroundings > 0 8. Gibbs Free Energy (G) G = H – TS Change in Gibbs energy: ΔG = ΔH – TΔS ΔG < 0 → Reaction is spontaneous ΔG = 0 → System at equilibrium ΔG > 0 → Non-spontaneous reaction 9. Key Relations ΔG° = –RT ln K (Relation between Gibbs energy and equilibrium constant) w = –nRT ln(V₂/V₁) (Reversible isothermal expansion of ideal gas) Conclusion Thermodynamics forms the backbone of physical chemistry, connecting energy, heat, and work with the spontaneity and equilibrium of reactions. By mastering concepts like internal energy (U), enthalpy (H), entropy (S), and Gibbs free energy (G), IIT JEE aspirants can predict the feasibility and direction of any chemical process — making it one of the most scoring topics in the exam.

Instructions: Each question carries 4 marks. Select the correct answer and click Submit to view your score, correct answers, and explanations. Q1. The standard electrode potential of Zn2+/Zn is –0.76 V and that of Cu2+/Cu is +0.34 V. The EMF of the cell Zn | Zn2+ || Cu2+ | Cu is: a) 0.42 V b) 1.10 V c) 0.76 V d) –1.10 V Q2. The unit of molar conductivity is: a) S m2 mol–1 b) S mol–1 c) ohm–1 d) S m mol–1 Q3. Which of the following electrolytes shows the highest molar conductivity at infinite dilution? a) NaCl b) HCl c) NH4OH d) CH3COOH Q4. In the electrolysis of molten NaCl, the product at the cathode is: a) Na b) Cl2 c) NaOH d) H2 Q5. According to Kohlrausch’s Law, the molar conductivity of an electrolyte at infinite dilution is equal to: a) Sum of equivalent conductivities of cation and anion at infinite dilution b) Product of ionic mobilities c) Square of ionic mobilities d) None of these Q6. The slope of a graph between log([oxidised]/[reduced]) and electrode potential (E) is related to: a) Faraday’s constant b) Nernst equation c) Gibbs free energy d) Cell constant Q7. The conductance of a solution depends upon: a) Nature of ions only b) Concentration of ions only c) Nature and concentration of ions, and temperature d) Electrode potential Q8. In a galvanic cell, the flow of electrons occurs from: a) Cathode to anode b) Anode to cathode c) Salt bridge to anode d) Salt bridge to cathode Q9. During electrolysis, the amount of substance deposited on an electrode is proportional to: a) Charge passed b) Voltage applied c) Temperature d) Pressure Q10. The relation between free energy change (ΔG) and EMF of the cell (E) is: a) ΔG = –nFE b) ΔG = nFE c) ΔG = –RT lnK d) ΔG = E/RT Submit Here are notes on Electrochemistry chapter by Prof. Anil Tyagi : https://odtutor.com/electrochemistry-the-science-of-chemical-energy-electrical-power/

Strategic Notes for IIT-JEE and NEET Aspirants by Prof. Anil Tyagi Future innovators, welcome. Electrochemistry is not merely a chapter; it is the bridge between the world of chemical reactions and the tangible power of electricity. It explains how your batteries work, how metals corrode, and how life itself maintains electrical potentials across cell membranes. For IIT-JEE, this topic is a high-yield area, blending conceptual clarity with numerical application. Our mission is to master both. 1. The Foundation: Conductors and Redox Revisited First, we must distinguish between two paths of current flow: At its heart, electrochemistry is the systematic study of redox reactions. Recall: 2. The Electrochemical Cell: Converting Chemical Energy to Electrical Work The Galvanic or Voltaic Cell is the archetype. Think of a Daniel Cell (Zn | Zn²⁺ || Cu²⁺ | Cu). 3. The Driving Force: Standard Electrode Potential (E°) Why does zinc lose electrons to copper? The answer lies in the intrinsic tendency of an electrode to lose or gain electrons, measured as the Standard Electrode Potential (E°). 4. The Nernst Equation: Accounting for Real-World Conditions The standard potential is for 1 M concentration and 1 atm pressure at 298 K. The real cell potential under non-standard conditions is given by the Nernst Equation, a cornerstone for JEE problems. Ecell = E°cell – (RT/nF) ln Q For simplicity at 298 K: Ecell = E°cell – (0.059/n) log Q Where: 5. Electrolytic Cells: Using Electricity to Drive Chemistry This is the reverse of a galvanic cell. Here, electrical energy is used to force a non-spontaneous redox reaction (E°cell is negative). 6. Conductivity: Measuring the Ease of Ion Flow Professor Tyagi’s Key Takeaways for JEE Success: Master these principles, and you will not only solve JEE problems but also understand the technology powering our world. Stay focused, and let your potential drive your success. – Prof. Anil Tyagi

Instructions: Each question carries 4 marks. Select the correct option and click Submit to check your score, answers, and explanations. Q1. The coordination number of Co in [Co(NH3)6]Cl3 is: a) 3 b) 4 c) 5 d) 6 Q2. The IUPAC name of [Pt(NH3)2Cl2] is: a) Dichlorodiamineplatinum(II) b) Diamminedichloroplatinum(II) c) Platinum diamine dichloride d) Dichloroplatinum diamine Q3. Which of the following shows linkage isomerism? a) [Co(NH3)6]Cl3 b) [Co(NO2)(NH3)5]Cl2 c) [CoCl(NH3)5]Cl2 d) [Cu(NH3)4]SO4 Q4. The hybridization of central metal ion in [Ni(CO)4] is: a) dsp2 b) sp3 c) d2sp3 d) sp2d Q5. Which of the following is a chelating ligand? a) NH3 b) Cl– c) EDTA4- d) CN– Q6. The complex [Fe(CN)6]4- is: a) High spin, paramagnetic b) Low spin, diamagnetic c) High spin, diamagnetic d) Low spin, paramagnetic Q7. The effective atomic number (EAN) of Fe in [Fe(CO)5] is: a) 36 b) 34 c) 35 d) 32 Q8. In [Cr(NH3)4Cl2]Cl, the primary valency of Cr is: a) 2 b) 3 c) 4 d) 6 Q9. Which one among the following is an inner orbital complex? a) [CoF6]3- b) [Ni(CO)4] c) [Fe(CN)6]4- d) [MnO4]– Q10. Which of the following complexes exhibits geometrical isomerism? a) [Co(NH3)6]3+ b) [Pt(NH3)2Cl2] c) [Fe(CN)6]3- d) [Mn(H2O)6]2+ Submit Coordination Compounds: The Architectural Marvels of Inorganic Chemistry A Strategic Introduction for IIT-JEE Aspirants by Prof. Anil Tyagi Future engineers and scientists, welcome. As we venture beyond simple salts and molecules, we enter the elegant and complex world of Coordination Compounds. Think of this not as another chapter, but as the study of chemical architecture where a central metal ion acts as a cornerstone, and surrounding molecules or ions, called ligands, form the intricate pillars and walls. This topic is not just crucial for IIT-JEE; it is fundamental to understanding biological systems (like haemoglobin), industrial catalysts, and modern materials. Our goal is to build a conceptual framework that is both deep and exam-ready. 1. The Core Concept: What Are Coordination Compounds? A coordination compound is characterized by a central metal atom or ion surrounded by a set of molecules or anions known as ligands. The key differentiator from a double salt is that coordination compounds retain their identity in solution. The bond between the metal and the ligand is a special covalent bond where the ligand donates a pair of electrons to the metal. This is called a coordinate covalent bond. 2. Fundamental Terminology: The Building Blocks To master this chapter, you must be fluent in its language. 3. Werner’s Coordination Theory: The Historical Breakthrough Alfred Werner’s theory (1893) was revolutionary. He proposed: 4. Modern Bonding Theories: The “Why” Behind the Structure For IIT-JEE, you must have a clear understanding of two key theories: Professor’s Final Advice: Focus on CFT. Master the spectrochemical series. Practice numerical problems on magnetic moments and crystal field stabilization energy (CFSE). This chapter is highly scoring if your concepts are clear. Visualize the structures, understand the splitting, and you will conquer it. – Prof. Anil Tyagi

Instructions: Each question carries 4 marks. Select the best answer and submit to view your score, correct answers, and explanations. Q1. The rate constant of a first-order reaction has units: a) mol L-1 s-1 b) s-1 c) mol s-1 d) L mol-1 s-1 Q2. In the Arrhenius equation, k = A·e-Ea/RT, the slope of ln k vs 1/T plot is: a) -Ea/R b) Ea/R c) -R/Ea d) 1/Ea Q3. A zero-order reaction has a half-life that: a) Depends on initial concentration b) Is independent of concentration c) Is infinite d) Does not exist Q4. If doubling concentration doubles the rate, the order of reaction is: a) Zero b) One c) Two d) Fractional Q5. In a reaction A → Products, if the rate law is Rate = k[A]^2, then doubling [A] will increase rate by: a) 2 times b) 4 times c) 8 times d) No change Q6. Which one of the following reactions is generally zero order? a) H2 + Cl2 → 2HCl (in sunlight) b) Hydrolysis of ester c) Decomposition of N2O5 d) Radioactive decay Q7. For a first-order reaction, the half-life (t1/2) is given by: a) 1/k b) 0.693/k c) ln2·k d) k/2 Q8. Catalyst increases rate of reaction by: a) Increasing equilibrium constant b) Lowering activation energy c) Increasing activation energy d) Increasing ΔG Q9. The rate constant doubles when temperature is raised from 300K to 310K. The activation energy (Ea) is approximately: a) 54 kJ/mol b) 5.4 kJ/mol c) 540 kJ/mol d) 2.7 kJ/mol Q10. A reaction with rate law Rate = k[A]^0[B]^1 is: a) First order in A b) First order overall c) Zero order overall d) Second order overall Submit Introduction to IIT JEE Chemistry – Chemical Kinetics The Chemical Kinetics chapter holds a very significant place in Physical Chemistry and is frequently tested in the IIT JEE Main and Advanced examinations. While Thermodynamics tells us whether a reaction is feasible or not, Chemical Kinetics focuses on how fast the reaction occurs and what factors influence the rate. For aspirants, mastering this topic ensures a strong foundation for solving numerical problems and conceptual questions that often appear in competitive exams. What is Chemical Kinetics? Chemical Kinetics is the branch of chemistry that deals with the speed (rate) of chemical reactions, the mechanisms by which they proceed, and the factors influencing the rate. For example, while burning of paper in air is very slow at room temperature, it becomes very fast when ignited with a flame. This difference is explained by kinetics, not thermodynamics. Importance in IIT JEE In JEE Main and Advanced, questions from this chapter range from basic definitions and order of reaction concepts to numerical problems on half-life, integrated rate laws, Arrhenius equation, and activation energy. Understanding this chapter not only helps in direct scoring but also supports other concepts like equilibrium, electrochemistry, and surface chemistry. On average, 2–3 questions are asked every year in JEE Main from this topic. Key Concepts Students Must Master Application-Based Questions in JEE Students must expect questions like: Tips for JEE Preparation Why This Practice Paper Will Help This Part 13 Practice Paper on Chemical Kinetics is designed to test students on both theoretical understanding and problem-solving skills. The multiple-choice format reflects the exact pattern of JEE, and each question includes explanations to aid in quick revision. By attempting this quiz, aspirants can identify weak areas, strengthen concepts, and improve speed and accuracy—two essential qualities for cracking JEE.