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1. 1. Please read:7 tips to solve physics faster in MHT-CETSeptember 19, 2010 By Prof. Rohan Shenoy40 Comments 1. Play chess or any other mild puzzle for improving basic logical, analytic and reasoning skills. 2. By-heart logarithm tables of common nos (Ex: 0 – 9) for faster calculation. 3. Wherever you are dealing with fractional nos, always eliminate the decimal and spin it into a power of 10. Example: (5.1/17) should be solved as [(51/17)*10-1]. Eliminating fractions will improve the accuracy exponentially. In MHT-CET physics paper, many times the only difference in options is their decimal place. Ex: a) 1.3 b) 0.13 c) 0.013 d) 0.0013 4. Learn inter-conversion of units in various systems such as MKS and CGS. 5. While solving numerical MCQs from any book, such as P.S. Bangui, start solving from the last question to first question, i.e in reverse order. The difficult questions are usually given in the last. If reverse order is too difficult, you can solve alternate questions in serial order. 6. Use common sense, and do not be nervous or anxious while approaching questions. Most of the questions are straight forward formula based. Students blow it up because they are weak on calculation parts, or are not prepared fully. 7. Instead of “reading” formulas, practice them in the form of numericals. This will give dual benefit of learning the formula as well math speed.For your information: Atleast 45 out of 50 questions in physics paper are numerical questions. It is foolish on the part of any student to appear for CET without having practiced numerica personal appeal fromWikipedia founder Jimmy Wales Read nowLaws of thermodynamicsFrom Wikipedia, the free encyclopediaJump to: navigation, searchThermodynamicsThe classical Carnot heat engineBranches[show]Classical · Statistical · ChemicalEquilibrium / Non-equilibrium
2. 2. Laws[hide]Zeroth · First · Second · ThirdSystems[show]State:Equation of stateIdeal gas · Real gasPhase of matter · EquilibriumControl volume · Instruments--------------------------------------------------------------------------------Processes:Isobaric · Isochoric · IsothermalAdiabatic · Isentropic · IsenthalpicQuasistatic · PolytropicFree expansionReversibility · IrreversibilityEndoreversibility--------------------------------------------------------------------------------Cycles:Heat engines · Heat pumpsThermal efficiencySystem properties[show]Property diagramsIntensive and extensive properties--------------------------------------------------------------------------------Functions of state:Temperature / Entropy (intro.) †Pressure / Volume †Chemical potential / Particle no. †
3. 3. († Conjugate variables)Vapor qualityReduced properties--------------------------------------------------------------------------------Process functions:Work · HeatMaterial properties[show]Specific heat capacityCompressibilityThermal expansionProperty databaseEquations[show]Carnots theorem · Clausius theorem · Fundamental relation · Ideal gas law · Maxwellrelations · Onsager reciprocal relations--------------------------------------------------------------------------------Table of thermodynamic equationsPotentials[show]Free energy · Free entropy--------------------------------------------------------------------------------Internal energyEnthalpyHelmholtz free energyGibbs free energy
4. 4. History and culture[show]Philosophy:Entropy and time · Entropy and lifeBrownian ratchetMaxwells demonHeat death paradoxLoschmidts paradoxSynergetics--------------------------------------------------------------------------------History:General · Heat · Entropy · Gas lawsPerpetual motionTheories:Caloric theory · Vis vivaTheory of heatMechanical equivalent of heatMotive powerPublications:"An Experimental Enquiry Concerning ... Heat""On the Equilibrium of Heterogeneous Substances""Reflections on theMotive Power of Fire"--------------------------------------------------------------------------------Timelines of:Thermodynamics · Heat engines
5. 5. --------------------------------------------------------------------------------Art:Maxwells thermodynamic surface--------------------------------------------------------------------------------Education:Entropy as energy dispersalScientists[show]Bernoulli · Carnot · Clapeyron · Clausius · von Helmholtz · Carathéodory · PierreDuhem · Gibbs · Joule · Maxwell · von Mayer · Onsager · Rankine · Smeaton · Stahl · Thompson · Kelvin· Watersonv ·t ·eThe four laws of thermodynamics define fundamental physical quantities (temperature, energy, andentropy) that characterize thermodynamic systems. The laws describe how these quantities behaveunder various circumstances, and forbid certain phenomena (such as perpetual motion).The four laws of thermodynamics are:[1][2][3][4][5][6]Zeroth law of thermodynamics: If two systems are in thermal equilibrium with a third system, theymust be in thermal equilibrium with each other. This law helps define the notion of temperature.First law of thermodynamics: Heat and work are forms of energy transfer. Energy is invariablyconserved but the internal energy of a closed system changes as heat and work are transferred in orout of it. Equivalently, perpetual motion machines of the first kind are impossible.Second law of thermodynamics: The entropy of any isolated system not in thermal equilibrium almostalways increases. Isolated systems spontaneously evolve towards thermal equilibrium—the state ofmaximum entropy of the system—in a process known as "thermalization". Equivalently, perpetualmotion machines of the second kind are impossible.Third law of thermodynamics: The entropy of a system approaches a constant value as thetemperature approaches zero. The entropy of a system at absolute zero is typically zero, and in allcases is determined only by the number of different ground states it has. Specifically, the entropy of apure crystalline substance at absolute zero temperature is zero.
6. 6. Classical thermodynamics describes the exchange of work and heat between systems. It has a specialinterest in systems that are individually in states of thermodynamic equilibrium. Thermodynamicequilibrium is a condition of systems which are adequately described by only macroscopic variables.Every physical system, however, when microscopically examined, shows apparently randommicroscopic statistical fluctuations in its thermodynamic variables of state (entropy, temperature,pressure, etc.). These microscopic fluctuations are negligible for systems which are nearly inthermodynamic equilibrium and which are only macroscopically examined. They become important,however, for systems which are nearly in thermodynamic equilibrium when they are microscopicallyexamined, and, exceptionally, for macroscopically examined systems that are in critical states[7], andfor macroscopically examined systems that are far from thermodynamic equilibrium.There have been suggestions of additional laws, but none of them achieve the generality of the fouraccepted laws, and they are not mentioned in standard textbooks.[1][2][3][4][5][8][9]The laws of thermodynamics are important fundamental laws in physics and they are applicable inother natural sciences.Contents [hide]1 Zeroth law2 First law3 Second law4 Third law5 History6 See also7 References8 Further reading Zeroth lawThe zeroth law of thermodynamics may be stated as follows:
7. 7. If system A and system B are individually in thermal equilibrium with system C, then system A is inthermal equilibrium with system BThe zeroth law implies that thermal equilibrium, viewed as a binary relation, is a Euclidean relation. Ifwe assume that the binary relationship is also reflexive, then it follows that thermal equilibrium is anequivalence relation. Equivalence relations are also transitive and symmetric. The symmetricrelationship allows one to speak of two systems being "in thermal equilibrium with each other",which gives rise to a simpler statement of the zeroth law:If two systems are in thermal equilibrium with a third, they are in thermal equilibrium with each otherHowever, this statement requires the implicit assumption of both symmetry and reflexivity, ratherthan reflexivity alone.The law is also a statement about measurability. To this effect the law allows the establishment of anempirical parameter, the temperature, as a property of a system such that systems in equilibriumwith each other have the same temperature. The notion of transitivity permits a system, for examplea gas thermometer, to be used as a device to measure the temperature of another system.Although the concept of thermodynamic equilibrium is fundamental to thermodynamics and wasclearly stated in the nineteenth century, the desire to label its statement explicitly as a law was notwidely felt until Fowler and Planck stated it in the 1930s, long after the first, second, and third lawwere already widely understood and recognized. Hence it was numbered the zeroth law. Theimportance of the law as a foundation to the earlier laws is that it allows the definition oftemperature in a non-circular way without reference to entropy, its conjugate variable. First lawThe first law of thermodynamics may be stated thus:Increase in internal energy of a body = heat supplied to the body - work done by the body. U = Q - WFor a thermodynamic cycle, the net heat supplied to the system equals the net work done by thesystem.More specifically, the First Law encompasses several principles:
8. 8. The law of conservation of energy.This states that energy can be neither created nor destroyed. However, energy can change forms, andenergy can flow from one place to another. The total energy of an isolated system remains the same.The concept of internal energy and its relationship to temperature.If a system, for example a rock, has a definite temperature, then its total energy has threedistinguishable components. If the rock is flying through the air, it has kinetic energy. If it is highabove the ground, it has gravitational potential energy. In addition to these, it has internal energywhich is the sum of the kinetic energy of vibrations of the atoms in the rock, and other sorts ofmicroscopic motion, and of the potential energy of interactions between the atoms within the rock.Other things being equal, the internal energy increases as the rocks temperature increases. Theconcept of internal energy is the characteristic distinguishing feature of the first law ofthermodynamics.The flow of heat is a form of energy transfer.In other words, a quantity of heat that flows from a hot body to a cold one can be expressed as anamount of energy being transferred from the hot body to the cold one.Performing work is a form of energy transfer.For example, when a machine lifts a heavy object upwards, some energy is transferred from themachine to the object. The object acquires its energy in the form of gravitational potential energy inthis example.Combining these principles leads to one traditional statement of the first law of thermodynamics: it isnot possible to constuct a perpetual motion machine which will continuously do work withoutconsuming energy. Second lawThe second law of thermodynamics asserts the existence of a quantity called theentropy of a system and further states thatWhen two isolated systems in separate but nearby regions of space, each in thermodynamicequilibrium in itself (but not necessarily in equilibrium with each other at first) are at some timeallowed to interact, breaking the isolation that separates the two systems, allowing them to exchangematter or energy, they will eventually reach a mutual thermodynamic equilibrium. The sum of theentropies of the initial, isolated systems is less than or equal to the entropy of the final combinationof exchanging systems. In the process of reaching a new thermodynamic equilibrium, total entropyhas increased, or at least has not decreased.
9. 9. It follows that the entropy of an isolated macroscopic system never decreases. The second law statesthat spontaneous natural processes increase entropy overall, or in another formulation that heat canspontaneously be conducted or radiated only from a higher-temperature region to a lower-temperature region, but not the other way around.The second law refers to a wide variety of processes, reversible and irreversible. Its main import is totell about irreversibility.The prime example of irreversibility is in the transfer of heat by conduction or radiation. It was knownlong before the discovery of the notion of entropy that when two bodies of different temperaturesare connected with each other by purely thermal connection, conductive or radiative, then heatalways flows from the hotter body to the colder one. This fact is part of the basic idea of heat, and isrelated also to the so-called zeroth law, though the textbooks statements of the zeroth law areusually reticent about that, because they have been influenced by Carathéodorys basing hisaxiomatics on the law of conservation of energy and trying to make heat seem a theoreticallyderivative concept instead of an axiomatically accepted one. Šilahvý (1997) notes that Carathéodorysapproach does not work for the description of irreversible processes that involve both heatconduction and conversion of kinetic energy into internal energy by viscosity (which is another primeexample of irreversibility), because "the mechanical power and the rate of heating are not expressibleas differential forms in the external parameters".[10]The second law tells also about kinds of irreversibility other than heat transfer, and the notion ofentropy is needed to provide that wider scope of the law.According to the second law of thermodynamics, in a reversible heat transfer, an element of heattransferred, δQ, is the product of the temperature (T), both of the system and of the sources ordestination of the heat, with the increment (dS) of the systems conjugate variable, its entropy (S)[1]The second law defines entropy, which may be viewed not only as a macroscopic variable of classicalthermodynamics, but may also be viewed as a measure of deficiency of physical information aboutthe microscopic details of the motion and configuration of the system, given only predictableexperimental reproducibility of bulk or macroscopic behavior as specified by macroscopic variablesthat allow the distinction to be made between heat and work. More exactly, the law asserts that for
10. 10. two given macroscopically specified states of a system, there is a quantity called the difference ofentropy between them. The entropy difference tells how much additional microscopic physicalinformation is needed to specify one of the macroscopically specified states, given the macroscopicspecification of the other , which is often a conveniently chosen reference state. It is often convenientto presuppose the reference state and not to explicitly state it. A final condition of a natural processalways contains microscopically specifiable effects which are not fully and exactly predictable fromthe macroscopic specification of the initial condition of the process. This is why entropy increases innatural processes. The entropy increase tells how much extra microscopic information is needed totell the final macroscopically specified state from the initial macroscopically specified state.[11] Third lawThe third law of thermodynamics is sometimes stated as follows:The entropy of a perfect crystal at absolute zero is exactly equal to zero.At zero temperature the system must be in a state with the minimum thermal energy. This statementholds true if the perfect crystal has only one state with minimum energy. Entropy is related to thenumber of possible microstates according to S = kBln(Ω), where S is the entropy of the system, kBBoltzmanns constant, and Ω the number of microstates (e.g. possible configurations of atoms). Atabsolute zero there is only 1 microstate possible (Ω=1) and ln(1) = 0.A more general form of the third law that applies to systems such as glasses that may have more thanone minimum energy state:The entropy of a system approaches a constant value as the temperature approaches zero.The constant value (not necessarily zero) is called the residual entropy of the system. HistorySee also: Philosophy of thermal and statistical physicsCount Rumford (born Benjamin Thompson) showed, about 1797, that mechanical action can generateindefinitely large amounts of heat, so challenging the caloric theory. The historically first establishedthermodynamic principle which eventually became the second law of thermodynamics wasformulated by Sadi Carnot during 1824. By 1860, as formalized in the works of those such as RudolfClausius and William Thomson, two established principles of thermodynamics had evolved, the firstprinciple and the second principle, later restated as thermodynamic laws. By 1873, for example,thermodynamicist Josiah Willard Gibbs, in his memoir Graphical Methods in the Thermodynamics of
11. 11. Fluids, clearly stated the first two absolute laws of thermodynamics. Some textbooks throughout the20th century have numbered the laws differently. In some fields removed from chemistry, the secondlaw was considered to deal with the efficiency of heat engines only, whereas what was called thethird law dealt with entropy increases. Directly defining zero points for entropy calculations was notconsidered to be a law. Gradually, this separation was combined into the second law and the modernthird law was widely adopted.Date: 21 Feb 2013 (Thursday)Paper: (Marathi / Gujarati / Kannada / Sindi / Malyalam / Tamil / Telugu / Punjabi / BengaliTime: 11.00 am to 2.00 pmDate: 22 Feb 2013 (Friday)Paper: HindiTime: 11.00 am to 2.00 pmPaper: German / Andhramagadhi / PersianTime: 3.00 am to 6.00 pmDate: 23 Feb 2013 (Saturday)Paper: EnglishTime: 11.00 am to 2.00 pmDate: 25 Feb 2013 (Monday)Paper: PhysicsTime: 11.00 am to 2.00 pmDate: 27 Feb 2013 (Wednesday)
12. 12. Paper: ChemistryTime: 11.00 am to 2.00 pmDate: 1 March 2013 (Friday)Paper: Mathematics & Statistics PaperTime: 11.00 am to 2.00 pmDate: 4 March 2013 (Monday)Paper: BiologyTime: 11.00 am to 2.00 pmThe Times of India Group Voice Support : 09024666666 Online Education B Schools Colleges Universities Courses Exams Loan Study Abroad Search Admit Card Answer Key Results Cutoff Time Table Syllabus Apply Online Jobs
13. 13. Home>Time Table -Maharashtra Board HSC Time TableMaharashtra Board HSC Time Table 2013, MaharashtraHSC Time Table 2013: -The MSBSHSE is a state education board of Maharashtra state. The MSBSHSE board is knownas the Maharashtra State Board of Secondary and Higher Secondary Education. The board isproviding education facilities to the students of Maharashtra state. The MSBSHSE board wasestablished on the 1st January of 1966 year. The MSBSHE board was established under the act ofthe Legislative Assembly of Maharashtra education board. The main headquarters of the board isthe Pune district of the Maharashtra state. Some other offices are also located in the Mumbai,Nagpur districts. The board is providing education in the local state language and in the Englishlanguage.Maharashtra Board HSC Time Table 2013:-The board is providing higher secondary education in different subjects in the differentdepartments. Mainly board is providing higher secondary education in the science, arts andcommerce stream with different combinations of subjects. The MSBSHSE board is conductingexams at the end of every annual session. The board conducts class 12th board exams in themarch month after the end of the session. The Maharashtra Board HSC Time Table is veryimportant for all the appearing students in the 12th class examination.The board exams of class 12th are important for the students and for this education board. Thestudents work hard in the class 12th from the start of the session to get a good percentage ofmarks. The Maharashtra board announced Maharashtra Board HSC Time Table 2013 mentionas below: - FIRST HALF SECOND HALF SUBJECT WITH INDEX SUBJECT WITHDATE/DAY TIME TIME NUMBER INDEX NUMBER Marathi (02)Thursday Gujarati (03) Urdu (05) French (13) Kannada (06) Pali (35) 3:00 pm21st 11:00 am to Tamil (09) to 6:00February, 2:00 pm Telugu (10) pm Malayalam (08)2013 Sindhi (07) Bengali (12) Punjabi (11)
14. 14. German (14)Friday 11:00 am to 3:00 pm Ardhamagadhi (16)22nd 2:00 Hindi (04) to 6:00February, pm11:00 am pm Persian (37) to 1:00 pm2013 Avesta – Pahalavi (87)Saturday 11:00 am to23th English (01) 2:00pmFebruary,2013 Secretarial Practice (C) (52) 11:00 am to 2:00 PMMonday 3:00 pm 11:00 am to Political Science (A)25th Physics (S) (54) to 6:00 2:00 pm (42)February, pm2013 11:00 am to 1:00 pm Physics Paper 1st (S) (54)Tuesday 11.00 a.m. Physics Paper – II (S) (54)26th to ( For Repeater CandidatesFebruary, Only)2013 1.00 p.m. 11.00 a.m. to Book Keeping & Accountancy (A/C) (50)Wednesday 2.00 p.m. Chemistry (S) (55) 3:00 pm27th, to 6:00 Philosophy (A) (46)February Chemistry Paper – I (S) (55) pm2013 11.00 a.m. ( For Repeater Candidates to Only) 1.00 p.m.Thursday Chemistry Paper – II (S) (55) 11:00 am to28th 1:00 pm ( For Repeater CandidatesFebruary, Only)2013Friday 11:00 am to Mathematics & Statistics Paper 3:00 pm Sociology (A/S) (45)
15. 15. 2:00 pm (A/S) (40) to 6:0001st March, pm2013 11.00 a.m. Mathematics & Statistics paper-I (A/S) (40) to ( For Repeater Candidates 1.00 p.m. Only) Mathematics & Statistics Paper – I (C) (88) Mathematics & Statistics Paper – II (A/S) (40) 3.00 p.m.Saturday ( For Repeater to02nd March, Candidates Only)2013 5.00 p.m. Mathematics & Statistics Paper – II (C) (88) 11.00 a.m. Biology (S) (56) to 2. 00 p.m. 3.00 p.m.Monday Economics (A/S/C) to04th March, (49)2013 Biology Paper – I (S) (56) 11.00 a.m. 6.00 p.m. ( For Repeater Candidates to Only) 1. 00 p.m.Tuesday 11.00 a.m. Biology Paper – II (S) (56)05th March, to ( For Repeater Candidates2013 Only) 1.00 p.m.Wednesday 11.00 a.m. Organisation of Commerce & 3.00 p.m. History (A) (38)06th March, to Management (C) (51) to2013 2.00 p.m. 6.00 p.m.
16. 16. Friday VOCATIONAL COURSES- 3.00 p.m. Education (A/S) (78) PAPER – I08th March, to2013 (TECHNICAL GROUP) 11:00 am to 6.00 p.m. 2:00 pm General Civil Engineering (A4) —————— 11.00 a.m. Electrical Maintenance (A1) to Mechanical Maintenance (A2) 1.30 p.m. Scooter and Motor Cycle Servicing (A3) Electronics (C2) 11.00 a.m. Computer Science (D9) to 2.00 p.m. COMMERCE GROUP PAPER –I Banking (A5) Office Management (A7) Marketing 11.00 a.m. & Salesmanship (A8) Small Industries & Self Employment to (A9) 2.00 p.m. FISHERY GROUP PAPER – I Fish Processing Technology (B9) Fresh Water Fish Culture 11.00 a.m. (C1) to 2.00 p.m AGRICULTURAL GROUP PAPER – I
17. 17. Animal Science & Dairying (B2), Crop Science (B4), Horticulture (B5) 11.00 a.m. to 2.00 p.mMonday VOCATIONAL COURSES- 3.00 p.m. OCCUPATIONAL PAPER – II ORIENTATION11th March, to2013 (TECHNICAL GROUP) Library & Information 11:00 am to 5.00 p.m. Science (A/C) (85) 2:00 pm General Civil Engineering (A4) —————— 3.00 p.m. Historical & 11:00 am to Electrical Maintenance (A1) Development of 1:30 pm to Mechanical Maintenance (A2) Indian classical Dance 6.00 p.m. (A) (91) Scooter and Motor Cycle Servicing (A3) 11:00 am to Electronics (C2) 2:00 pm Computer Science (D9) COMMERCE GROUP PAPER 11:00 am to – II 2:00 pm Banking (A5) Office Management (A7) Marketing & Salesmanship (A8) Small Industries & Self Employment (A9) 11:00 am to 2:00 pm FISHERY GROUP PAPER –
18. 18. II Fish Processing Technology (B9) Fresh Water Fish Culture 11:00 am to (C1) 1:00 pm AGRICULTURAL GROUP PAPER – II Animal Science & Dairying (B2), Crop Science (B4), Horticulture (B5) 3.00 p.m.Wednesday to Logic (A) (47)12th March,2013 6.00 p.m. 11.00 a.m.Wednesday to Co-operation (A/C) (53)13th March,2013 2.00 p.m. 3.00p.m. to European Music (A) 11.00 a.m.Friday (73) 4.00p.m to Geography (A/S/C) (39)15th 3.00p.m.March,2013 2.00 p.m. Japanese (21) to 6.00p.m Russian (20) Child Development 11.00 a.m. 3.00 p.m. (A/S) (43) Sanskrit (33) to toSaturday Arabic (36) 2.00 p.m. 5.30 p.m. Agriculture Science &16th TechnologyMarch,2013 General Knowledge (32) Paper-I (75), Animal 11.00 a.m. 3.00 p.m. Science & Technology (For Military School’s only)
19. 19. to to Paper-I (76) 2.00 p.m 5.00 p.m. 11.00 a.m. 3.00 p.m. Agriculture Science & Geology Paper – I (S) (41) Technology to to Paper-II (75), Animal 1.00 p.m. 5.00 p.m.Monday Science & Technology18th Paper-II (76) History & Appreciation of Artsmarch,2013 11.00 a.m. (A) 3.00 p.m. to (Painting, Sculpture & to Defense Studies Architecture) (60) (A/S/C) (77) 2.00 p.m. 5.30 p.m. 11.00 a.m.Tuesday to Textile (A/S) (44)19thmarch,2013 1.30 p.m. 3.00p.m to Geology Paper – II (S) 11.00 a.m.Wednesday (41) 5.00p.m. to Psychology (A/S) (48)20th 3.00p.mmarch,2013 2.00 p.m. Percussion (A) (69) to 5.30p.m. 11.00 a.m. 3.00p.mThursday History & Development of to to English Literature (22)21 nd Indian Music (A) (65)March,2013 2.00 p.m. 6.00p.m. Information Technology Information 11.00 a.m. 3.00 p.m. TechnologyFriday (Online Examination) to to (Online Examination)22nd Science (97)march,2013 1.30 p.m. 5.30 p.m. Science (97) Arts (98)
20. 20. Commerce (99) Arts (98) Commerce (99) Information Information Technology Technology 11.00 a.m. (Online Examination) 3.00 p.m.Saturday (Online Examination) to Science (97) to23rd Science (97)March,2013 1.30 p.m. Arts (98) 5.30 p.m. Arts (98) Commerce (99) Commerce (99) Information Information Technology Technology 11.00 a.m. (Online Examination) 3.00 p.m.Monday (Online Examination) to Science (97) to25th Science (97)March,2013 1.30 p.m. Arts (98) 5.30 p.m. Arts (98) Commerce (99) Commerce (99)Refine Your Search Term:-Maharashtra Board HSC Time Table, Maharashtra HSC Time Table, msbshse.ac.inAsk a Question, Just Fill & Submit ! Name (required) Mail (will not be published) (required)
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