Zeroth Law of Thermodynamics states that when two bodies are in thermal equilibrium with another third body than the two bodies are also in thermal equilibrium with each other. Ralph H.
Fowler developed this law in the 1930s, many years after the first, second, and third laws of thermodynamics had achieved widespread acceptance.
Here Thermal Equilibrium implies that when two systems are in contact with a barrier permeable only to heat, so there will be no change or transfer of heat.
Table of Contents
What is Zeroth Law of Thermodynamics?
Consider two systems A and B, separated by a wall that does not allow any exchange of energy between them. Such a wall is known as an insulating wall or adiabatic wall. The third system C is separated from systems A and B by a conducting or diathermic wall as shown in the figure.
Since energy can be exchanged between systems A and C, both A and C are in thermal equilibrium. Similarly, energy can be exchanged between the systems B and C, so both B and C are also in thermal equilibrium. In other words, both systems A and B are in thermal equilibrium with the third system C separately.
When the adiabatic wall between systems A and B is removed, no transfer of energy takes place between them.
This shows that systems A and B are also in thermal equilibrium with each other. This observation leads to an important law known as Zeroth’s law of thermodynamics which is stated as follows:
Zeroth Law of Thermodynamics states that when two bodies are in thermal equilibrium with another third body then the two bodies are also in thermal equilibrium with each other.
According to Zeroth’s law of thermodynamics, if system A is in thermal equilibrium with system C, then
Temperature of System A = Temperature of System C
Similarly, if system B is in thermal equilibrium with system C, then
Temperature of System B =Temperature of System C
Now, from the above relation, we have
Temperature of System A = Temperature of System B
Thermal Equilibrium
The zeroth law of thermodynamics recognizes that temperature is a valuable measurement since it predicts whether or not heat will flow between things. Regardless matter how the items interact, this is true. Heat can move between two things even if they are not physically interacting, as per the radiation method of heat transmission.
The zeroth law of thermodynamics says that no heat flow will occur if the systems are in thermal equilibrium.
Thermodynamics is distinguished from other studies by temperature. This trait is capable of distinguishing between hot and cold. When two or more bodies of different temperatures come into touch, they eventually reach a similar temperature and are said to be in thermal equilibrium.
Zeroth Law of Thermodynamics Example
Zeroth Law of Thermodynamics states that heat energy flows between two bodies when they are kept in contact with each other.
For example, if we take three bodies P, Q, and R at different temperatures which are in contact with each other than the heat transfers among the three bodies till they reach thermal equilibrium, in this case, they reach the constant temperature.
Thermal equilibrium can also be achieved even when the temperature of the bodies is different.
For example, if we take two bodies A and B, and contain them in adiabatic chambers (which do not allow heat to pass through them) then the, if they allow being in contact still there, is no heat transfer as adiabatic chambers do not allow heat to pass through it so they are considered to in thermal equilibrium.
The zeroth law of thermodynamics follows the translation relation between various bodies i.e. if we take three bodies A, B, and C then if A and B are in thermal equilibrium and B and C are in thermal equilibrium then A and c are also considered to be in thermal equilibrium.
Application of Zeroth Law of Thermodynamics
The law is crucial for the mathematical formulation of thermodynamics, or, to put it another way, for expressing the mathematical definition of temperature.
The most common use of this concept is to compare the temperatures of different things.
If we want to accurately measure temperature, we’ll need a reference body and a characteristic of that body that changes with temperature.
The change in that characteristic could be interpreted as a temperature change. The chosen feature is referred to as a thermodynamic property.
Nonetheless, Thermometers are the most prevalent application of the zeroth law of thermodynamics.
Using a simple thermometer with mercury in a tube, we may witness the zeroth law in operation.
Because the area of the tube remains constant as the temperature rises, the mercury expands.
The height has grown as a result of this development.
Now, the variation in the height of the mercury label indicates temperature changes and, in essence, aids us in measuring it.
Depending on their thermometric characteristic, several types of thermometers can be utilized. The following is a list of thermometers
Constant pressure gas thermometer – Volume
Constant volume gas thermometer – Pressure
Electrical resistance thermometer – Resistance
Mercury-in-glass thermometer – Length
Thermocouple – Thermal e.m.f.
When you have two glasses of water, you have another illustration of the zeroth law of thermodynamics. One glass will be filled with hot water, while the other will be filled with cold water. If we leave them on the table for a few hours, they will achieve thermal equilibrium with the room’s temperature.
Conclusion of Zeroth Law of Thermodynamics
The Zeroth Law of Thermodynamics establishes the foundation for understanding temperature and thermal equilibrium. Its significance lies in allowing us to compare temperatures and develop thermodynamic scales. Through the concept of thermal equilibrium, it enables the measurement of temperature using reference bodies and thermodynamic properties. Moreover, the ubiquitous application of thermometers exemplifies the practical implications of this law, facilitating temperature measurement in various contexts.
Zeroth Law of Thermodynamics- FAQs
Define Zeroth Law of Thermodynamics?
According to the Zeroth Law of Thermodynamics, two systems that are in thermal equilibrium with a third system separately are also in thermal equilibrium with each other.
Who gave the Zeroth Law of Thermodynamics?
The credit for stating the zeroth law of Thermodynamics goes to British scientist Ralph H. Fowler.
What is the Significance of the Zeroth Law of Thermodynamics?
Zeroth Law of Thermodynamics provides a significant relationship which is very helpful for the mathematical formulation of thermodynamics. It mathematically transforms the relationship between systems’ thermal equilibrium into an equivalence relation, which can represent the equality of a particular quantity related to each system.
How does Zeroth Law lead to the concept of temperature?
Zeroth law tells that heat always flows from a hot body to a cold body till both bodies have an equal temperature. The degree of hotness or coldness is called the temperature and thus, the zeroth law of thermodynamics leads to the temperature.
Why is it called the “zeroth law” of thermodynamics?
It was named “zeroth” because the first and second laws were already named, reflecting its foundational importance.
What is the difference between Heat and Temperature?
Difference between Heat and Temperature are,
Heat is a form of energy that is transferred between two bodies because if there is a temperature difference between them.
Temperature is degree of hotness and coldness of the body and it may be defined as the thermal condition of a body that determines the direction of heat flow i.e. it determines whether the body will receive heat from another body or it will give heat to the same.
What is the Internal Energy?
Internal energy is the sum of all forms of energy stored in atoms or molecules.
Neeraj Anand, Param Anand
Er. Neeraj K.Anand is a freelance mentor and writer who specializes in Engineering & Science subjects. Neeraj Anand received a B.Tech degree in Electronics and Communication Engineering from N.I.T Warangal & M.Tech Post Graduation from IETE, New Delhi. He has over 30 years of teaching experience and serves as the Head of Department of ANAND CLASSES. He concentrated all his energy and experiences in academics and subsequently grew up as one of the best mentors in the country for students aspiring for success in competitive examinations.
In parallel, he started a Technical Publication "ANAND TECHNICAL PUBLISHERS" in 2002 and Educational Newspaper "NATIONAL EDUCATION NEWS" in 2014 at Jalandhar. Now he is a Director of leading publication "ANAND TECHNICAL PUBLISHERS", "ANAND CLASSES" and "NATIONAL EDUCATION NEWS".
He has published more than hundred books in the field of Physics, Mathematics, Computers and Information Technology. Besides this he has written many books to help students prepare for IIT-JEE and AIPMT entrance exams. He is an executive member of the IEEE (Institute of Electrical & Electronics Engineers. USA) and honorary member of many Indian scientific societies such as Institution of Electronics & Telecommunication Engineers, Aeronautical Society of India, Bioinformatics Institute of India, Institution of Engineers. He has got award from American Biographical Institute Board of International Research in the year 2005.
CBSE Class 11 Chemistry Syllabus is a vast which needs a clear understanding of the concepts and topics. Knowing CBSE Class 11 Chemistry syllabus helps students to understand the course structure of Chemistry.
Unit-wise CBSE Class 11 Syllabus for Chemistry
Below is a list of detailed information on each unit for Class 11 Students.
UNIT I – Some Basic Concepts of Chemistry
General Introduction: Importance and scope of Chemistry.
Nature of matter, laws of chemical combination, Dalton’s atomic theory: concept of elements, atoms and molecules.
Atomic and molecular masses, mole concept and molar mass, percentage composition, empirical and molecular formula, chemical reactions, stoichiometry and calculations based on stoichiometry.
UNIT II – Structure of Atom
Discovery of Electron, Proton and Neutron, atomic number, isotopes and isobars. Thomson’s model and its limitations. Rutherford’s model and its limitations, Bohr’s model and its limitations, concept of shells and subshells, dual nature of matter and light, de Broglie’s relationship, Heisenberg uncertainty principle, concept of orbitals, quantum numbers, shapes of s, p and d orbitals, rules for filling electrons in orbitals – Aufbau principle, Pauli’s exclusion principle and Hund’s rule, electronic configuration of atoms, stability of half-filled and completely filled orbitals.
UNIT III – Classification of Elements and Periodicity in Properties
Significance of classification, brief history of the development of periodic table, modern periodic law and the present form of periodic table, periodic trends in properties of elements -atomic radii, ionic radii, inert gas radii, Ionization enthalpy, electron gain enthalpy, electronegativity, valency. Nomenclature of elements with atomic number greater than 100.
UNIT IV – Chemical Bonding and Molecular Structure
Valence electrons, ionic bond, covalent bond, bond parameters, Lewis structure, polar character of covalent bond, covalent character of ionic bond, valence bond theory, resonance, geometry of covalent molecules, VSEPR theory, concept of hybridization, involving s, p and d orbitals and shapes of some simple molecules, molecular orbital theory of homonuclear diatomic molecules(qualitative idea only), Hydrogen bond.
UNIT V – Chemical Thermodynamics
Concepts of System and types of systems, surroundings, work, heat, energy, extensive and intensive properties, state functions. First law of thermodynamics – internal energy and enthalpy, measurement of U and H, Hess’s law of constant heat summation, enthalpy of bond dissociation, combustion, formation, atomization, sublimation, phase transition, ionization, solution and dilution. Second law of Thermodynamics (brief introduction) Introduction of entropy as a state function, Gibb’s energy change for spontaneous and nonspontaneous processes. Third law of thermodynamics (brief introduction).
UNIT VI – Equilibrium
Equilibrium in physical and chemical processes, dynamic nature of equilibrium, law of mass action, equilibrium constant, factors affecting equilibrium – Le Chatelier’s principle, ionic equilibrium- ionization of acids and bases, strong and weak electrolytes, degree of ionization, ionization of poly basic acids, acid strength, concept of pH, hydrolysis of salts (elementary idea), buffer solution, Henderson Equation, solubility product, common ion effect (with illustrative examples).
UNIT VII – Redox Reactions
Concept of oxidation and reduction, redox reactions, oxidation number, balancing redox reactions, in terms of loss and gain of electrons and change in oxidation number, applications of redox reactions.
UNIT VIII – Organic Chemistry: Some basic Principles and Techniques
General introduction, classification and IUPAC nomenclature of organic compounds. Electronic displacements in a covalent bond: inductive effect, electromeric effect, resonance and hyper conjugation. Homolytic and heterolytic fission of a covalent bond: free radicals, carbocations, carbanions, electrophiles and nucleophiles, types of organic reactions.
UNIT IX – Hydrocarbons
Classification of Hydrocarbons Aliphatic Hydrocarbons: Alkanes – Nomenclature, isomerism, conformation (ethane only), physical properties, chemical reactions. Alkenes – Nomenclature, structure of double bond (ethene), geometrical isomerism, physical properties, methods of preparation, chemical reactions: addition of hydrogen, halogen, water, hydrogen halides (Markovnikov’s addition and peroxide effect), ozonolysis, oxidation, mechanism of electrophilic addition. Alkynes – Nomenclature, structure of triple bond (ethyne), physical properties, methods of preparation, chemical reactions: acidic character of alkynes, addition reaction of – hydrogen, halogens, hydrogen halides and water.
Aromatic Hydrocarbons:
Introduction, IUPAC nomenclature, benzene: resonance, aromaticity, chemical properties: mechanism of electrophilic substitution. Nitration, sulphonation, halogenation, Friedel Craft’s alkylation and acylation, directive influence of functional group in monosubstituted benzene. Carcinogenicity and toxicity.
To know the CBSE Syllabus for all the classes from 1 to 12, visit the Syllabus page of CBSE. Meanwhile, to get the Practical Syllabus of Class 11 Chemistry, read on to find out more about the syllabus and related information in this page.
CBSE Class 11 Chemistry Practical Syllabus with Marking Scheme
In Chemistry subject, practical also plays a vital role in improving their academic scores in the subject. The overall weightage of Chemistry practical mentioned in the CBSE Class 11 Chemistry syllabus is 30 marks. So, students must try their best to score well in practicals along with theory. It will help in increasing their overall academic score.
CBSE Class 11 Chemistry Practical Syllabus
The experiments will be conducted under the supervision of subject teacher. CBSE Chemistry Practicals is for 30 marks. This contribute to the overall practical marks for the subject.
The table below consists of evaluation scheme of practical exams.
Evaluation Scheme
Marks
Volumetric Analysis
08
Salt Analysis
08
Content Based Experiment
06
Project Work
04
Class record and viva
04
Total
30
CBSE Syllabus for Class 11 Chemistry Practical
Micro-chemical methods are available for several of the practical experiments. Wherever possible such techniques should be used.
A. Basic Laboratory Techniques 1. Cutting glass tube and glass rod 2. Bending a glass tube 3. Drawing out a glass jet 4. Boring a cork
B. Characterization and Purification of Chemical Substances 1. Determination of melting point of an organic compound. 2. Determination of boiling point of an organic compound. 3. Crystallization of impure sample of any one of the following: Alum, Copper Sulphate, Benzoic Acid.
C. Experiments based on pH
1. Any one of the following experiments:
Determination of pH of some solutions obtained from fruit juices, solution of known and varied concentrations of acids, bases and salts using pH paper or universal indicator.
Comparing the pH of solutions of strong and weak acids of same concentration.
Study the pH change in the titration of a strong base using universal indicator.
2. Study the pH change by common-ion in case of weak acids and weak bases.
D. Chemical Equilibrium One of the following experiments:
1. Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing the concentration of either of the ions. 2. Study the shift in equilibrium between [Co(H2O)6] 2+ and chloride ions by changing the concentration of either of the ions.
E. Quantitative Estimation i. Using a mechanical balance/electronic balance. ii. Preparation of standard solution of Oxalic acid. iii. Determination of strength of a given solution of Sodium hydroxide by titrating it against standard solution of Oxalic acid. iv. Preparation of standard solution of Sodium carbonate. v. Determination of strength of a given solution of hydrochloric acid by titrating it against standard Sodium Carbonatesolution.
F. Qualitative Analysis 1) Determination of one anion and one cation in a given salt Cations‐ Pb2+, Cu2+, As3+, Al3+, Fe3+, Mn2+, Ni2+, Zn2+, Co2+, Ca2+, Sr2+, Ba2+, Mg2+, NH4+ Anions – (CO3)2‐ , S2‐, NO2‐ , SO32‐, SO2‐ , NO ‐ , Cl‐ , Br‐, I‐, PO43‐ , C2O2‐ ,CH3COO‐ (Note: Insoluble salts excluded)
2) Detection of ‐ Nitrogen, Sulphur, Chlorine in organic compounds.
G) PROJECTS Scientific investigations involving laboratory testing and collecting information from other sources.
A few suggested projects are as follows:
Checking the bacterial contamination in drinking water by testing sulphide ion
Study of the methods of purification of water.
Testing the hardness, presence of Iron, Fluoride, Chloride, etc., depending upon the regional variation in drinking water and study of causes of presence of these ions above permissible limit (if any).
Investigation of the foaming capacity of different washing soaps and the effect of addition of Sodium carbonate on it.
Study the acidity of different samples of tea leaves.
Determination of the rate of evaporation of different liquids Study the effect of acids and bases on the tensile strength of fibres.
Study of acidity of fruit and vegetable juices.
Note: Any other investigatory project, which involves about 10 periods of work, can be chosen with theapproval of the teacher.
Practical Examination for Visually Impaired Students of Class 11
Below is a list of practicals for the visually impaired students.
A. List of apparatus for identification for assessment in practicals (All experiments) Beaker, tripod stand, wire gauze, glass rod, funnel, filter paper, Bunsen burner, test tube, test tube stand, dropper, test tube holder, ignition tube, china dish, tongs, standard flask, pipette, burette, conical flask, clamp stand, dropper, wash bottle • Odour detection in qualitative analysis • Procedure/Setup of the apparatus
B. List of Experiments A. Characterization and Purification of Chemical Substances 1. Crystallization of an impure sample of any one of the following: copper sulphate, benzoic acid B. Experiments based on pH 1. Determination of pH of some solutions obtained from fruit juices, solutions of known and varied concentrations of acids, bases and salts using pH paper 2. Comparing the pH of solutions of strong and weak acids of same concentration.
C. Chemical Equilibrium 1. Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing the concentration of eitherions. 2. Study the shift in equilibrium between [Co(H2O)6]2+ and chloride ions by changing the concentration of either of the ions.
D. Quantitative estimation 1. Preparation of standard solution of oxalic acid. 2. Determination of molarity of a given solution of sodium hydroxide by titrating it against standard solution of oxalic acid.
E. Qualitative Analysis 1. Determination of one anion and one cation in a given salt 2. Cations – NH+4 Anions – (CO3)2-, S2-, (SO3)2-, Cl-, CH3COO- (Note: insoluble salts excluded) 3. Detection of Nitrogen in the given organic compound. 4. Detection of Halogen in the given organic compound.
Note: The above practicals may be carried out in an experiential manner rather than recording observations.
We hope students must have found this information on CBSE Syllabus useful for their studying Chemistry. Learn Maths & Science in interactive and fun loving ways with ANAND CLASSES (A School Of Competitions) App/Tablet.
Frequently Asked Questions on CBSE Class 11 Chemistry Syllabus
Q1
How many units are in the CBSE Class 11 Chemistry Syllabus?
There are 9 units in the CBSE Class 11 Chemistry Syllabus. Students can access various study materials for the chapters mentioned in this article for free at ANAND CLASSES (A School Of Competitions).
Q2
What is the total marks for practicals examination as per the CBSE Class 11 Chemistry Syllabus?
The total marks for the practicals as per the CBSE Class 11 Chemistry Syllabus is 30. It includes volumetric analysis, content-based experiment, salt analysis, class record, project work and viva.
Q3
Which chapter carries more weightage as per the CBSE Syllabus for Class 11 Chemistry?
The organic chemistry chapter carries more weightage as per the CBSE Syllabus for Class 11 Chemistry.
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