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Biology for Class 10 ICSE - Unit 1 Basic Biology - The Blueprint of Life

Biology for Class 10 ICSE – Unit 1: Basic Biology – The Blueprint of Life

ICSE Class 10 Biology / By

Biology for Class 10 ICSE (2025-26) Unit 1: Basic Biology – The Blueprint of Life A Comprehensive Lecture by Prof. Anil Tyagi, Ph.D. My dear students, the human body is a universe of roughly 37 trillion cells. Each of these cells knows its purpose, its function, and its lifespan. This incredible organization, the transmission of traits from one generation to the next, and the very differentiation of male and female—all of it is governed by the principles we will study today. We will delve into the cell’s life cycle, the architecture of genetic information, and the elegant rules of heredity laid down by a monk in a garden. This is where your journey into medicine truly begins. 1. The Cell Cycle and Cell Division: The Rhythm of Life Every living organism, from a single-celled amoeba to a complex human, grows and reproduces through cell division. It is a tightly regulated process, not a chaotic event. This ordered sequence of events is called the Cell Cycle. The cell cycle is divided into two primary phases: Interphase: The Busy Resting Period Do not be fooled by the old term “resting phase.” Interphase is a period of intense biochemical activity and preparation. It is the longest phase of the cell cycle and is subdivided into three distinct stages: M-Phase: The Phase of Division This is where the cell divides its already duplicated contents to form two daughter cells. M-phase consists of two processes: Mitosis (Equational Division) Mitosis is the process of nuclear division that ensures each daughter cell receives an exact copy of the parent cell’s genetic material. It is used for growth, repair, and asexual reproduction. It consists of four stages: The result of mitosis is two daughter cells, each genetically identical to the parent cell and to each other, with the same diploid number of chromosomes. Meiosis (Reductional Division) – A Basic Idea Meiosis is a specialized type of cell division that occurs only in the germ cells of the reproductive organs (ovaries and testes) to produce gametes (sperms and eggs). 2. Structure of Chromosome: The Packaging of Heredity How is meters-long DNA packed into a microscopic nucleus? The answer lies in the incredible packaging of chromosomes. Think of it like this: DNA is a long, intricate thread. Winding it around histones (nucleosomes) makes it manageable like a string of beads. Coiling this string further creates the thick, rod-like structures we see as chromosomes during cell division. This packaging is essential for the accurate segregation of genetic material. 3. Genetics: The Science of Heredity Genetics is the study of heredity and variation. It explains how traits are passed from parents to offspring. Mendel’s Laws: The Foundation Gregor Mendel, the father of genetics, discovered the fundamental principles of inheritance through his meticulous pea plant experiments. Monohybrid and Dihybrid Crosses Sex Determination This is the biological system that determines the development of sexual characteristics in an organism. In humans, it is chromosomal. Sex-linked Inheritance Genes located on the sex chromosomes (mostly the X-chromosome) show a specific pattern of inheritance called sex-linked inheritance. Professor Tyagi’s Key Takeaways for NEET Aspirants: This unit is the bedrock of modern biology and medicine. From understanding cancer (uncontrolled cell division) to genetic counseling and gene therapy, it all starts here. Internalize these concepts. Build your foundation strong. Your future patients are counting on the knowledge you build today. – Prof. Anil Tyagi

Top 20 Engineering Colleges in India – A Guide by Rahul C Sir

Top 20 Engineering Colleges in India – A Guide by Rahul C Sir

Engineering Colleges / By

Engineering continues to be one of the most sought-after career paths in India. Every year, lakhs of students appear for competitive examinations like JEE Main and JEE Advanced, aiming for admission into top institutions that promise world-class education, exposure, and career opportunities. As someone who has been guiding students in Mathematics for IIT-JEE for years, I often get questions such as: “Sir, which engineering colleges are considered the best in India?” This blog is my attempt to give you a clear and practical answer. Based on the National Institutional Ranking Framework (NIRF) 2025 rankings, reputation, placements, research output, and overall opportunities, here’s a detailed look at the Top 20 Engineering Colleges in India. 1. Indian Institute of Technology Madras (IIT Madras) – Chennai IIT Madras consistently tops the list of engineering colleges in India. With cutting-edge research facilities, excellent placements, and strong industry collaborations, it is often considered the dream destination for engineering aspirants. 2. Indian Institute of Technology Delhi (IIT Delhi) – New Delhi Known for its innovative research ecosystem and entrepreneurial culture, IIT Delhi is a top choice for students who wish to build strong academic foundations while exploring startups and global opportunities. 3. Indian Institute of Technology Bombay (IIT Bombay) – Mumbai Famous for its vibrant campus life and outstanding academic excellence, IIT Bombay offers not just engineering education but also exposure to arts, culture, and entrepreneurship. Its alumni network is one of the strongest in India. 4. Indian Institute of Technology Kanpur (IIT Kanpur) – Uttar Pradesh IIT Kanpur is well-known for its rigorous academic curriculum, focus on innovation, and research-driven environment. Students here often excel in both technical and managerial careers. 5. Indian Institute of Technology Kharagpur (IIT KGP) – West Bengal The first IIT to be established in India, IIT KGP carries a strong legacy. It offers a wide range of engineering courses and is especially renowned for civil, mechanical, and electronics engineering. 6. Indian Institute of Technology Roorkee (IIT Roorkee) – Uttarakhand IIT Roorkee, one of the oldest engineering institutions in Asia, has been a pioneer in civil and structural engineering. Its beautiful campus and research opportunities make it highly attractive for engineering aspirants. 7. Indian Institute of Technology Guwahati (IIT Guwahati) – Assam IIT Guwahati is gaining rapid recognition for its academic programs and research in advanced fields like nanotechnology, AI, and renewable energy. Its picturesque campus adds to the charm. 8. Indian Institute of Technology Hyderabad (IIT Hyderabad) – Telangana A relatively new IIT, IIT Hyderabad has already made a mark with its modern teaching methods, international tie-ups, and strong research focus, especially in AI, robotics, and data sciences. 9. National Institute of Technology Trichy (NIT Trichy) – Tamil Nadu Among the NITs, Trichy is considered the best. With strong placements, excellent faculty, and a dynamic campus environment, it competes closely with many IITs in terms of opportunities. 10. Indian Institute of Technology (Indian School of Mines), Dhanbad – Jharkhand Originally famous for mining and earth sciences, IIT (ISM) Dhanbad now offers diverse engineering disciplines and is becoming increasingly popular among JEE aspirants. 11. National Institute of Technology Karnataka (NITK Surathkal) – Karnataka With its strategic coastal location, NITK offers excellent research facilities and top-tier placements, especially in mechanical and computer science engineering. 12. Vellore Institute of Technology (VIT) – Tamil Nadu A leading private university, VIT has built a strong reputation for offering world-class facilities, good placement opportunities, and international exposure. Its VITEEE entrance exam attracts thousands of aspirants every year. 13. Birla Institute of Technology and Science (BITS Pilani) – Rajasthan BITS Pilani stands out as one of the best private institutions in India. Known for its flexible academic structure, strong alumni network, and research culture, BITS competes closely with some of the older IITs. 14. Indian Institute of Technology Indore (IIT Indore) – Madhya Pradesh IIT Indore has been steadily rising in reputation. It offers excellent academic programs, particularly in computer science, and has research partnerships with international institutions. 15. Indian Institute of Technology BHU (IIT BHU) – Varanasi With a blend of tradition and technology, IIT BHU is an excellent choice for students looking for strong academics along with the cultural vibrancy of Varanasi. 16. Amrita Vishwa Vidyapeetham – Coimbatore, Tamil Nadu Amrita University has built a strong reputation as one of the top private engineering colleges in India, with impressive placements and research output in areas like medical engineering and renewable energy. 17. Thapar Institute of Engineering & Technology – Patiala, Punjab Thapar Institute has long been recognized for quality education, strong industry ties, and excellent infrastructure, making it a top choice among private institutions. 18. SRM Institute of Science and Technology – Chennai SRMIST has a wide range of engineering courses and offers international collaborations, making it attractive for students aiming for global exposure along with engineering studies. 19. Manipal Institute of Technology (MIT Manipal) – Karnataka MIT Manipal is one of India’s oldest private engineering colleges with a strong legacy of academic excellence, entrepreneurship, and placements in reputed companies. 20. Delhi Technological University (DTU) – New Delhi Formerly known as Delhi College of Engineering (DCE), DTU is a top state university with a strong reputation for engineering programs, especially in mechanical and computer science. How to Choose the Right College for You While rankings provide a broad overview, the right engineering college for you depends on several factors: My Advice to Students Getting into one of these top 20 colleges requires consistent preparation, focus, and the right guidance. Mathematics, especially for IIT-JEE, can be a deciding factor in your performance. Many students struggle with problem-solving strategies, time management, and application of concepts. This is exactly where personalized guidance can make a huge difference. With years of teaching experience, I have seen students transform their confidence in Mathematics once they receive individual attention. If you are preparing for IIT-JEE or other engineering entrance exams, I am offering personalized online Maths coaching through Odtutor. Each student receives individual guidance, doubt-clearing sessions, and practice strategies tailored

Class 10 ICSE - Unit 1. Periodic Table, Periodic Properties & Variations Early classification (Dobereiner, Newlands, Mendeleev)

Class 10 ICSE – Unit 1. Periodic Table, Periodic Properties & Variations Early classification (Dobereiner, Newlands, Mendeleev)

ICSE Class 10 Chemistry / By

Unit 1: Periodic Table, Periodic Properties & Variations A Comprehensive Lecture by Prof. Anil Tyagi, Ph.D. My dear students, future custodians of health and scientific inquiry, welcome. Before we can comprehend the complex biochemistry of the human body, the pharmacology of drugs, or the diagnosis of diseases, we must first become fluent in the language of matter itself. That language is written in the elements, and its grammar is defined by the Periodic Table. This is not merely a chart to be memorized; it is a profound reflection of the inherent order in the universe, a map that reveals the deepest relationships between the building blocks of everything we see, touch, and are. Consider this unit the most important chapter in your chemical education. Let’s begin. 1. The Early Classification: A Quest for Order The 19th century was a time of rapid chemical discovery. New elements were being isolated regularly, and scientists, like detectives, were desperately looking for patterns to make sense of the chaos. They were trying to group elements based on their properties, much like a librarian organizes books. a) Dobereiner’s Triads (1829): The First Hint of a Pattern Johann Wolfgang Dobereiner, a German chemist, was the first to notice a tangible numerical relationship between elements and their properties. b) Newlands’ Law of Octaves (1864): The Musical Analogy Inspired by Dobereiner’s work, the English chemist John Newlands took a more ambitious approach. He arranged all the known elements (about 56 at the time) in the strict order of increasing atomic masses. c) Mendeleev’s Periodic Table (1869): The Masterstroke Then came Dmitri Ivanovich Mendeleev, a Russian chemist of unparalleled vision. His approach was both brilliant and bold. 2. The Modern Periodic Table: The Final Key The year 1913 was a turning point. The English physicist Henry Moseley, while working with X-rays, discovered a fundamental property of the atom: its atomic number (Z). 3. Periodic Properties: The Heart of the Matter Why do elements behave the way they do? The answer lies in periodic trends. These trends are logical and can be understood by considering three key factors: Let’s analyze the trends in detail: Property & Definition Trend Across a Period (Left to Right) Trend Down a Group (Top to Bottom) Underlying Reason Atomic RadiusDistance from nucleus to outermost electron Decreases Increases Across: Increased nuclear charge pulls the electron cloud closer with greater force, shrinking the atom.Down: A new electron shell is added with each period, increasing the size despite the increased nuclear charge. Metallic CharacterTendency to lose electrons and form positive ions Decreases Increases Across: Increased nuclear charge holds onto valence electrons more tightly, making them harder to lose.Down: Increased atomic size and shielding effect mean valence electrons are farther from the nucleus and are held less tightly, making them easier to lose. Non-Metallic CharacterTendency to gain electrons and form negative ions Increases Decreases This is the exact opposite of metallic character. It increases as the effective nuclear charge increases and the atomic size decreases, making it easier to attract electrons. Ionisation Energy (IE)Minimum energy required to remove the most loosely bound electron from an isolated gaseous atom Increases Decreases Across: Increasing nuclear charge and decreasing atomic size make it harder to remove an electron (more energy needed).Down: Increased atomic size and shielding effect make it easier to remove an electron (less energy needed). Electron Affinity (EA)Energy change when an electron is added to a neutral gaseous atom Increases Decreases Across: Smaller atomic size and high nuclear charge facilitate easier addition of an electron, releasing more energy.Down: Larger atomic size means the incoming electron is less attracted by the nucleus, so less energy is released. Electronegativity (EN)The relative tendency of an atom to attract the shared pair of electrons towards itself in a covalent bond Increases Decreases Across: High nuclear charge and small size allow an atom to attract shared electrons strongly.Down: Larger size and increased shielding reduce the atom’s ability to attract shared electrons. Note on Noble Gases: They often are exceptions to trends like Electron Affinity and Electronegativity as they have a stable octet and little tendency to gain or attract electrons. 4. Core Concepts: Valency, Atomic Number, Mass Number These are the fundamental identifiers and descriptors of an element. Professor Tyagi’s Final Words for NEET Aspirants: My young scholars, internalize this unit. Do not rote-learn it. This chapter is the alphabet of chemistry. Master it, and you will be able to read the entire language of science with ease. Your journey to AIIMS and other top medical colleges begins with a strong command of such fundamental concepts. Work hard, stay curious, and never stop questioning. I am here to guide you every step of the way. – Prof. Anil Tyagi

IIT JEE Chemistry Practice Paper – Part 13 - (Chemical Kinetics)

IIT JEE Chemistry Practice Paper – Part 13 (Chemical Kinetics)

IIT - JEE Chemistry / By

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.

IIT JEE Chemistry Practice Paper – Part 12 - Solutions

IIT JEE Chemistry Practice Paper – Part 12 (Solutions)

IIT - JEE Chemistry / By

IIT JEE Chemistry Practice Paper – Part 12 covers the topic of Solutions, an important unit of Physical Chemistry. This section focuses on concentration terms, Raoult’s Law, vapor pressure, colligative properties (relative lowering of vapor pressure, elevation of boiling point, depression of freezing point, osmotic pressure), and Henry’s Law. These concepts are frequently tested in JEE Main and Advanced exams. By solving these questions, students can strengthen numerical ability, avoid common mistakes, and gain confidence in handling real exam problems. Q1. Which of the following is not a colligative property? (a) Relative lowering of vapor pressure (b) Elevation of boiling point (c) Depression of freezing point (d) Heat of vaporization Q2. Raoult’s law is applicable to: (a) Ideal solutions (b) Non-ideal solutions (c) Super-saturated solutions (d) Colloidal solutions Q3. The unit of molality is: (a) mol L–1 (b) mol kg–1 (c) g L–1 (d) g mol–1 Q4. Henry’s law relates solubility of a gas with: (a) Temperature (b) Pressure (c) Nature of solvent (d) Osmotic pressure Q5. Which colligative property is used to calculate molar masses of polymers? (a) Relative lowering of vapor pressure (b) Osmotic pressure (c) Elevation of boiling point (d) Depression of freezing point Q6. An azeotropic mixture shows: (a) Positive deviation from Raoult’s law only (b) Negative deviation from Raoult’s law only (c) Either positive or negative deviation (d) Ideal behavior Q7. The freezing point of 1 molal NaCl solution (assuming complete dissociation) compared to 1 molal glucose solution is: (a) Same (b) Lower (c) Higher (d) Unaffected Q8. Which concentration term is temperature independent? (a) Molarity (b) Molality (c) Normality (d) Mole fraction Q9. Osmotic pressure of a dilute solution is proportional to: (a) Molarity (b) Molality (c) Temperature only (d) Pressure Q10. Colligative properties depend on: (a) Nature of solute (b) Number of solute particles (c) Nature of solvent (d) Temperature only Submit Answers Solutions – IIT JEE Chemistry Notes The chapter Solutions is an important topic in Physical Chemistry for IIT JEE as it combines concepts of thermodynamics, equilibrium, and practical chemistry. A solution is a homogeneous mixture of two or more components, with the component present in larger quantity called the solvent, and the smaller one(s) called solute(s). Types of Solutions Depending on concentration, solutions can be dilute, concentrated, saturated, or supersaturated. Concentration Terms Students must master different ways of expressing concentration: Solubility Solubility depends on temperature, pressure, and nature of solute/solvent. Vapour Pressure & Raoult’s Law Colligative Properties These properties depend only on the number of solute particles: Colligative properties are also used to calculate molar mass of solutes, a favorite JEE question type. Key JEE Tips ✅ With solid conceptual clarity and practice of numericals, the Solutions chapter can help students secure crucial marks in IIT JEE.

Part 11 – IIT JEE Chemistry Practice Paper (Surface Chemistry)

Part 11 – IIT JEE Chemistry Practice Paper (Surface Chemistry)

IIT - JEE Chemistry / By

IIT JEE Chemistry Practice Paper – Part 11 (Surface Chemistry) Instructions: This practice paper contains 10 multiple-choice questions from the topic Surface Chemistry. Each correct answer gives 4 marks. Attempt all and then click “Submit” to view your score, answers, and explanations. Q1. The process of accumulation of molecules at the surface rather than in the bulk is called: Absorption Adsorption Desorption Sorption Q2. Which of the following is an example of chemisorption? Adsorption of O₂ on charcoal Adsorption of H₂ on finely divided Ni Adsorption of NH₃ on silica gel Adsorption of iodine on starch Q3. Freundlich adsorption isotherm is represented as: x/m = kP x/m = kP^1/n x/m = k + P x/m = k/P Q4. Which of the following is used as a positive catalyst in the manufacture of NH₃ by Haber’s process? V₂O₅ Ni Fe Pt Q5. Which type of colloid is milk? Solid in gas Liquid in liquid Liquid in solid Gas in liquid Q6. Gold sol is prepared by: Reduction Oxidation Hydrolysis Peptization Q7. Which of the following is an example of lyophobic colloid? Gum Starch Gold sol Gelatin Q8. Which of the following is used to coagulate negatively charged colloids like arsenic sulphide sol? Cl⁻ ions OH⁻ ions Ba²⁺ ions SO₄²⁻ ions Q9. Tyndall effect is due to: Reflection of light Scattering of light Refraction of light Absorption of light Q10. Which type of catalysis is observed in the conversion of SO₂ to SO₃ in contact process? Homogeneous catalysis Heterogeneous catalysis Autocatalysis Enzyme catalysis

_IIT JEE Chemistry Practice Paper (Electrochemistry) with 10 MCQs - Part 10

IIT JEE Chemistry Practice Paper (Electrochemistry) with 10 MCQs – Part 10

IIT - JEE Chemistry / By

IIT JEE Chemistry Practice Paper – Part 10 (Electrochemistry) Instructions: This practice paper includes 10 multiple-choice questions from the topic Electrochemistry. Each correct answer gives you 4 marks. Attempt all and then click “Submit” to check your score, answers, and explanations. Q1. 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: 0.10 V 1.10 V –1.10 V 0.76 V Q2. Which law states that the amount of substance deposited during electrolysis is proportional to the quantity of electricity passed? Ohm’s Law Faraday’s First Law Faraday’s Second Law Kohlrausch’s Law Q3. Molar conductivity of a strong electrolyte: Increases with dilution Decreases with dilution Remains constant First increases then decreases Q4. The unit of molar conductivity is: S m⁻¹ Ω m S cm² mol⁻¹ C mol⁻¹ Q5. For the reaction: Cu²⁺ + Zn → Cu + Zn²⁺, the reducing agent is: Cu²⁺ Cu Zn Zn²⁺ Q6. The slope of the graph of molar conductivity vs √C (for strong electrolyte) is related to: Kohlrausch’s Law Faraday’s Law Ohm’s Law Raoult’s Law Q7. The quantity of electricity required to deposit 1 mole of Al (Atomic mass = 27) from Al³⁺ ion is: 1 F 2 F 3 F 6 F Q8. The Nernst equation relates electrode potential with: Temperature only Pressure only Concentration of ions Heat of reaction Q9. In a Daniel cell, which of the following occurs? Cu is oxidised, Zn is reduced Zn is oxidised, Cu²⁺ is reduced Both Cu and Zn are oxidised Both Cu and Zn are reduced Q10. The electrochemical equivalent depends upon: Nature of electrolyte Nature of electrode Nature of substance deposited Quantity of electricity

IIT JEE Chemistry Practice Paper on Topic - Solid State -Part 9 - PYQs

IIT JEE Chemistry Practice Paper on Topic – Solid State -Part 9 – PYQs

IIT - JEE Chemistry / By

IIT JEE Chemistry Practice Paper – Part 9 covers the topic of Solid State, a fundamental concept in Physical Chemistry. This section focuses on crystal lattices, unit cells, packing efficiency, defects in solids, and electrical properties. Many tricky and conceptual questions are asked from this topic in JEE Main and Advanced. In this practice paper, you will find 10 carefully selected multiple-choice questions inspired by previous years’ exams. Each question comes with detailed solutions and explanations to help you clear concepts, avoid common mistakes, and build the confidence needed to tackle Solid State questions in the actual exam. IIT JEE Chemistry Practice Paper – Part 9 (Solid State) Instructions: Attempt all 10 questions. Each correct answer carries 4 marks. No negative marking here. After submitting, you’ll see your score, number of correct/wrong answers, and explanations. Q1. Which of the following is an example of ionic solid? Diamond Sodium chloride Graphite Ice Q2. In body-centered cubic (bcc) arrangement, the coordination number of each atom is: 4 6 8 12 Q3. The packing efficiency in a face-centered cubic (fcc) lattice is: 52.4% 68.0% 74.0% 60.0% Q4. Schottky defect is observed in: KCl ZnS AgCl FeO Q5. Which type of solid shows electrical conductivity in solid as well as molten state? Covalent solids Ionic solids Metallic solids Molecular solids Q6. The number of atoms per unit cell in a simple cubic structure is: 1 2 4 6 Q7. Frenkel defect is usually observed in: NaCl KCl AgBr CsCl Q8. The edge length of a unit cell is 400 pm. If it is fcc, the radius of the atom is approximately: 141 pm 200 pm 282 pm 173 pm Q9. Which of the following is not a crystalline solid? Quartz Glass Sodium chloride Diamond Q10. In hexagonal close packing (hcp), the percentage of empty space is: 26% 32% 40% 20%

IIT JEE Chemistry Practice Paper – Part 8 - Electrochemistry - PYQ

IIT JEE Chemistry Practice Paper – Part 8 – Electrochemistry – PYQ

Uncategorized / By

IIT JEE Chemistry Practice Paper – Previous Years’ Questions Part 8: Electrochemistry 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) 0.58 V b) 1.10 V c) 1.50 V d) 0.42 V In the electrolysis of aqueous NaCl solution, the gas liberated at the cathode is: a) Oxygen b) Hydrogen c) Chlorine d) Nitrogen The equivalent conductance of a strong electrolyte at infinite dilution is denoted as: a) Λm0 b) λm c) Km d) Λc The electrochemical equivalent of an element is directly proportional to: a) Equivalent weight b) Atomic weight c) Valency d) Density Faraday’s first law of electrolysis states that: a) Mass deposited is independent of electricity passed b) Mass deposited ∝ Quantity of electricity passed c) Mass deposited ∝ Voltage applied d) Mass deposited depends only on temperature Conductivity of a solution decreases with: a) Increase in dilution b) Increase in concentration c) Increase in temperature d) None of these The unit of molar conductivity is: a) S m2 mol-1 b) Ω-1 cm2 mol-1 c) Both a and b d) J mol-1 The product formed at the anode during electrolysis of molten NaCl is: a) Sodium b) Chlorine c) Oxygen d) Hydrogen The standard electrode potential of hydrogen electrode is: a) +1.00 V b) 0.00 V c) -1.00 V d) +0.76 V Kohlrausch’s law is useful in determining: a) Equivalent conductivity of weak electrolytes b) Solubility product c) Degree of dissociation d) All of the above

IT JEE Chemistry Practice Paper - PYQs SET 7 - Redox Reactions

IIT JEE Chemistry Practice Paper – Part 7 – Redox Reactions – PYQs

IIT - JEE Chemistry / By

IIT JEE Chemistry Practice Paper – Previous Years’ Questions Part 7: Redox Reactions Q1. In the reaction: Zn + CuSO₄ → ZnSO₄ + Cu, which element is oxidized? a) Cu b) Zn c) S d) O Q2. In which of the following reactions is H₂O₂ acting as an oxidizing agent? a) 2H₂O₂ → 2H₂O + O₂ b) H₂O₂ + 2KI + H₂SO₄ → I₂ + 2H₂O + K₂SO₄ c) H₂O₂ + Na₂SO₃ → Na₂SO₄ + H₂O d) H₂O₂ + Cl₂ → 2HCl + O₂ Q3. The oxidation number of Cr in K₂Cr₂O₇ is: a) +2 b) +3 c) +6 d) +7 Q4. Which of the following is a disproportionation reaction? a) Cl₂ + 2OH⁻ → Cl⁻ + ClO⁻ + H₂O b) Zn + Cu²⁺ → Zn²⁺ + Cu c) Fe²⁺ + MnO₄⁻ → Fe³⁺ + Mn²⁺ d) Cu + 2AgNO₃ → Cu(NO₃)₂ + 2Ag Q5. Which of the following statements about oxidizing agents is correct? a) They undergo reduction b) They undergo oxidation c) They always contain oxygen d) They always contain halogens Q6. The change in oxidation number of Mn in KMnO₄ when it acts as an oxidizing agent in acidic medium is: a) +7 to +2 b) +7 to +4 c) +7 to +6 d) +7 to +5 Q7. In the reaction: 2FeCl₃ + SnCl₂ → 2FeCl₂ + SnCl₄, the reducing agent is: a) FeCl₃ b) SnCl₂ c) FeCl₂ d) SnCl₄ Q8. Which of the following reactions is NOT a redox reaction? a) CaCO₃ → CaO + CO₂ b) 2Mg + O₂ → 2MgO c) Zn + 2HCl → ZnCl₂ + H₂ d) Fe²⁺ + Cl₂ → Fe³⁺ + 2Cl⁻ Q9. In acidic medium, MnO₂ acts as an oxidizing agent and changes into: a) Mn²⁺ b) Mn³⁺ c) MnO₄⁻ d) Mn Q10. In which of the following is the oxidation number of nitrogen highest? a) NH₃ b) NO₂ c) HNO₃ d) N₂ Submit These IIT JEE Chemistry practice quizzes are highly useful for students as they provide structured, exam-oriented preparation. Each quiz is topic-specific, allowing aspirants to revise one concept at a time and strengthen their weak areas. The format follows the real JEE exam pattern, with multiple-choice questions and negative marking awareness, which helps students build accuracy and time management skills. Detailed explanations after every question enhance conceptual clarity and prevent repetitive mistakes. Since the quizzes are self-evaluating, students can measure progress instantly and adapt their study strategy accordingly, ensuring consistent improvement and confidence for IIT JEE success.

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