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Q. What is the electronic configuration of oxygen?
  • A. 1s2 2s2 2p4
  • B. 1s2 2s2 2p6
  • C. 1s2 2s2 2p2
  • D. 1s2 2s2 2p5
Q. What is the electronic configuration of the chloride ion (Cl-)?
  • A. 1s2 2s2 2p6 3s2 3p5
  • B. 1s2 2s2 2p6 3s2 3p6
  • C. 1s2 2s2 2p6 3s2 3p4
  • D. 1s2 2s2 2p6 3s2 3p3
Q. What is the electronic configuration of the element with atomic number 12?
  • A. [Ne] 3s2
  • B. [He] 2s2 2p6
  • C. [Ne] 3s1
  • D. [Ar] 4s2
Q. What is the electronic configuration of the element with atomic number 15?
  • A. [Ne] 3s2 3p3
  • B. [Ne] 3s2 3p4
  • C. [Ne] 3s2 3p5
  • D. [Ne] 3s2 3p2
Q. What is the electronic configuration of the element with atomic number 17?
  • A. 1s2 2s2 2p6 3s2 3p5
  • B. 1s2 2s2 2p6 3s2 3p4
  • C. 1s2 2s2 2p6 3s2 3p6
  • D. 1s2 2s2 2p6 3s2 3p3
Q. What is the electronic configuration of the element with atomic number 20?
  • A. [Ne] 3s2 3p6
  • B. [Ar] 4s2
  • C. [He] 2s2 2p6 3s2 3p6
  • D. [Ne] 3s2 3p4
Q. What is the electronic configuration of the element with atomic number 26?
  • A. [Ar] 4s2 3d6
  • B. [Ar] 4s2 3d5
  • C. [Kr] 5s2 4d6
  • D. [Ar] 4s1 3d7
Q. What is the electronic configuration of the element with atomic number 29?
  • A. [Ar] 4s2 3d9
  • B. [Ar] 4s2 3d10
  • C. [Kr] 5s1 4d10
  • D. [Ne] 3s2 3p6
Q. What is the electronic configuration of the iron (Fe) atom?
  • A. [Ar] 4s2 3d6
  • B. [Ar] 4s2 3d5
  • C. [Ar] 4s1 3d7
  • D. [Ar] 4s2 3d4
Q. What is the electronic configuration of the nitrogen atom?
  • A. 1s2 2s2 2p3
  • B. 1s2 2s2 2p4
  • C. 1s2 2s2 2p2
  • D. 1s2 2s2 2p5
Q. What is the electronic configuration of the potassium ion (K+)?
  • A. 1s2 2s2 2p6 3s2
  • B. 1s2 2s2 2p6
  • C. 1s2 2s2 2p6 3s1
  • D. 1s2 2s2 2p6 3s2 3p1
Q. What is the electronic configuration of the sodium ion (Na+)?
  • A. 1s2 2s2 2p6
  • B. 1s2 2s2 2p5
  • C. 1s2 2s2 2p4
  • D. 1s2 2s2 2p3
Q. What is the empirical formula of a compound containing 40% carbon, 6.7% hydrogen, and 53.3% oxygen?
  • A. CH2O
  • B. C2H4O2
  • C. C3H6O3
  • D. C4H8O4
Q. What is the empirical formula of a compound containing 40% carbon, 6.7% hydrogen, and 53.3% oxygen by mass?
  • A. CH2O
  • B. C2H4O2
  • C. C3H6O3
  • D. C4H8O4
Q. What is the empirical formula of C6H12O6?
  • A. C2H4O2
  • B. CH2O
  • C. C3H6O3
  • D. C6H12O6
Q. What is the empirical formula of glucose (C6H12O6)?
  • A. C6H12O6
  • B. CH2O
  • C. C3H6O3
  • D. C2H4O2
Q. What is the enthalpy change for the formation of 1 mole of CO2 from its elements in their standard states?
  • A. -393.5 kJ/mol
  • B. -285.8 kJ/mol
  • C. 0 kJ/mol
  • D. 100 kJ/mol
Q. What is the enthalpy change for the formation of water from hydrogen and oxygen?
  • A. It is positive.
  • B. It is negative.
  • C. It is zero.
  • D. It is undefined.
Q. What is the enthalpy change for the reaction 2Na + Cl2 → 2NaCl?
  • A. -411 kJ
  • B. -240 kJ
  • C. 0 kJ
  • D. 411 kJ
Q. What is the enthalpy change for the reaction at constant pressure?
  • A. ΔH = ΔU + PΔV
  • B. ΔH = ΔU - PΔV
  • C. ΔH = ΔU + VΔP
  • D. ΔH = ΔU - VΔP
Q. What is the enthalpy change for the reaction N2(g) + 3H2(g) → 2NH3(g) at standard conditions?
  • A. -92.4 kJ
  • B. -45.9 kJ
  • C. 0 kJ
  • D. 0.5 kJ
Q. What is the enthalpy change for the reaction: 2H2(g) + O2(g) → 2H2O(g)?
  • A. It is positive.
  • B. It is negative.
  • C. It is zero.
  • D. It is dependent on temperature.
Q. What is the enthalpy change for the reaction: 2H2(g) + O2(g) → 2H2O(l)?
  • A. -571.6 kJ
  • B. -285.8 kJ
  • C. 0 kJ
  • D. 285.8 kJ
Q. What is the enthalpy change for the reaction: C(s) + O2(g) -> CO2(g)?
  • A. -393.5 kJ/mol
  • B. -241.8 kJ/mol
  • C. 0 kJ/mol
  • D. 285.8 kJ/mol
Q. What is the enthalpy change for the reaction: C(s) + O2(g) → CO2(g)?
  • A. -393.5 kJ/mol
  • B. -241.8 kJ/mol
  • C. 0 kJ/mol
  • D. 285.8 kJ/mol
Q. What is the enthalpy change for the reaction: CaCO3(s) → CaO(s) + CO2(g)?
  • A. It is an endothermic reaction.
  • B. It is an exothermic reaction.
  • C. It has no enthalpy change.
  • D. It is spontaneous at all temperatures.
Q. What is the enthalpy change for the reaction: H2(g) + 1/2 O2(g) → H2O(l)?
  • A. -285.8 kJ/mol
  • B. 0 kJ/mol
  • C. -241.8 kJ/mol
  • D. -572 kJ/mol
Q. What is the enthalpy change for the reaction: N2(g) + 3H2(g) → 2NH3(g)?
  • A. It is always positive.
  • B. It is always negative.
  • C. It can be either positive or negative depending on conditions.
  • D. It is zero.
Q. What is the enthalpy change when 1 mole of NaCl is dissolved in water?
  • A. -3.87 kJ
  • B. 0 kJ
  • C. +3.87 kJ
  • D. -7.0 kJ
Q. What is the enthalpy change when 1 mole of water vapor condenses to liquid water?
  • A. It is positive.
  • B. It is negative.
  • C. It is zero.
  • D. It is dependent on pressure.
Showing 601 to 630 of 1494 (50 Pages)

Physical Chemistry MCQ & Objective Questions

Physical Chemistry is a crucial branch of chemistry that combines principles of physics and chemistry to explain how matter behaves. Mastering this subject is essential for students preparing for school exams and competitive tests. Practicing MCQs and objective questions in Physical Chemistry not only enhances conceptual clarity but also boosts your chances of scoring better in exams. Engaging with practice questions helps identify important topics and reinforces learning.

What You Will Practise Here

  • Thermodynamics: Laws, concepts, and applications
  • Kinetics: Rate laws, reaction mechanisms, and factors affecting reaction rates
  • Equilibrium: Chemical equilibrium, Le Chatelier's principle, and equilibrium constants
  • Quantum Chemistry: Basic principles and applications in atomic structure
  • Electrochemistry: Redox reactions, electrochemical cells, and Nernst equation
  • Solutions: Colligative properties and their calculations
  • Acids and Bases: pH calculations, buffer solutions, and titration curves

Exam Relevance

Physical Chemistry is a significant part of the syllabus for CBSE, State Boards, NEET, and JEE. Questions often focus on theoretical concepts, numerical problems, and application-based scenarios. Common patterns include direct questions on laws of thermodynamics, calculations involving reaction rates, and conceptual questions on equilibrium. Familiarity with these patterns can greatly enhance your exam preparation.

Common Mistakes Students Make

  • Misunderstanding the application of thermodynamic laws in different scenarios
  • Confusing reaction rates with equilibrium constants
  • Overlooking the significance of units in calculations
  • Neglecting to practice numerical problems, leading to poor time management during exams

FAQs

Question: What are the key topics to focus on in Physical Chemistry for exams?
Answer: Focus on thermodynamics, kinetics, equilibrium, and electrochemistry as these are frequently tested.

Question: How can I improve my performance in Physical Chemistry MCQs?
Answer: Regular practice of MCQs and understanding the underlying concepts will significantly improve your performance.

Now is the time to enhance your understanding of Physical Chemistry! Dive into our practice MCQs and test your knowledge to excel in your exams. Your success starts with practice!

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