{"id":35845,"date":"2022-11-25T11:13:16","date_gmt":"2022-11-25T05:43:16","guid":{"rendered":"https:\/\/tsboardsolutions.com\/?p=35845"},"modified":"2022-11-25T11:13:16","modified_gmt":"2022-11-25T05:43:16","slug":"ts-inter-1st-year-physics-notes-chapter-13","status":"publish","type":"post","link":"https:\/\/tsboardsolutions.com\/ts-inter-1st-year-physics-notes-chapter-13\/","title":{"rendered":"TS Inter 1st Year Physics Notes Chapter 13 Thermodynamics"},"content":{"rendered":"

Here students can locate TS Inter 1st Year Physics Notes<\/a> 13th Lesson Thermodynamics to prepare for their exam.<\/p>\n

TS Inter 1st Year Physics Notes 13th Lesson Thermodynamics<\/h2>\n

\u2192 Thermodynamics: It is a branch of physics in which we shall study the process where work is converted into heat and vice versa.<\/p>\n

\u2192 Thermodynamic variables: In thermodynamics the state of a gas is specified by macroscopic variables such as pressure, temperature, volume, mass and composition that are felt by our sense perceptions and are measurable.<\/p>\n

\u2192 Thermal equilibrium: In general at thermal equilibrium the temperatures of the two bodies or systems are equal.
\nIn a thermally isolated system it is said to be in “thermal equilibrium” if the thermodynamic variables such as pressure, volume, temperature, mass and composition do not change with time and they have fixed values.<\/p>\n

\u2192 Zeroth law of thermodynamics: It states that if two systems say A & B are in thermal equilibrium with a third system ‘C’ separately then the two systems A and B are also in thermal equilibrium with each other.<\/p>\n

\u2192 Internal energy: It includes only the energy associated with random motion of molecules of the system
\ni. e., internal energy is simply the sum of kinetic and potential energies of these molecules. Internal energy is denoted by ‘U’.<\/p>\n

\u2192 First law of thermodynamics: The heat energy (dQ) supplied to a system is partly used to increase its internal energy (dU) and the rest is used to do work (dW)
\ni. e., dQ = dU + dW. (OR)
\nHeat energy supplied to a system (dQ) always equals to the sum of change in internal energy (dU) and workdone (dW).
\nThis law is a consequence of ”law of conservation of energy.”<\/p>\n

\u2192 Isothermal expansion: If a system is taken through a thermodynamic process in which \u0394U = 0 then it is called Isothermal process.
\nIn isothermal process change in internal energy \u0394U = 0 i.e., temperature of the system is constant. Isothermal process obeys gas equation PV = RT.<\/p>\n

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\u2192 Adiabatic process: In an adiabatic process system is insulated from the surroundings. So energy absorbed or released is zero (\u0394Q = 0). In adiabatic process temperature of the system may change. It follows the equation PV\u03b3<\/sup> = constant. Where \u03b3 = \\(\\frac{C_P}{C_V}\\) ratio of specific heats of a gas.<\/p>\n

\u2192 Isobaric process: In isobaric process pressure P’ is kept constant, volume and temperature changes are permitted. Work done in isobaric process
\nW = P(V2<\/sub> – V1<\/sub>) = \u00b5R(T2<\/sub> – T1<\/sub>).<\/p>\n

\u2192 Isochoric process: In isochoric process volume (V) of the system is kept constant. Work done by isochoric process is zero. In this process heat energy absorbed is totally used to increase the internal energy of the system.<\/p>\n

\u2192 Cyclic process: In a cyclic process the system returns to initial state (P, V and T). Change in internal energy \u0394U = 0. Heat absorbed during cyclic process is equal to work done.<\/p>\n

\u2192 Reversible process : A thermodynamic process is said to be reversible if the process can be turned back such that both the system and surroundings return to their original state, with no other change any where else in universe.<\/p>\n

\u2192 Irreversible process : If a thermodynamic process cannot be reversed exactly in opposite direction of direct process then it is called irreversible process.
\nAll spontaneous process of nature are irreversible.<\/p>\n

\u2192 Quasi static process: In a quasi static process at every stage the difference on pressure and temperature of systems and surroundings is infinitesimally small.
\ni.e., P + \u0394V \u2248 P and T + \u0394T = T .
\nIn this process the thermodynamic variables (P,V,T) will change very slowly so that it remains in thermal and mechanical equilibrium with surroundings throughout that process.
\nNote: Quasi static process is an imaginary concept only.<\/p>\n

\u2192 Heat engines: A heat engine is a device by which a system is made to undergo a cyclic process. As a result heat is converted into work.
\nWork done by heat engine W= Q1<\/sub> – Q2<\/sub>;<\/p>\n

Work done by heat engine W= Q1 \u2014 Q2; efficiency \u03b7 = 1 – \\(\\frac{\\mathrm{Q}_2}{\\mathrm{Q}_1}\\) (or) \u03b7 = 1 – \\(\\frac{\\mathrm{T}_2}{\\mathrm{~T}_1}\\)<\/p>\n

Important parts of heat engine : every heat engine mainly consists of<\/p>\n