Thermodynamics Laws In Pdf Notes Zeroth Law Second Law 3rd Law
Science which deals with study of different forms of energy and quantitative relationship.
The part of universe for study is called system and remaining portion is surroundings.
State of system is described in terms of T, P, V etc. The property which depends only on state of system not upon path is called state function eg. P, V, T, E, H, S etc.
Properties which depends on quantity of matter called extensive prop. eg. mass, volume, heat capacity, enthalpy, entropy etc. The properties which do not depends on matter present depends upon nature of substance called Intensive properties. eg. T,P, density, refractive index, viscosity, bp, pH, mole fraction etc.
The total energy with a system. i.e. U = Ee En + Ec + Ep + Ek + ------ ∆ U = U2 – U1 or UP – UR & U is state function and extensive properly. If U1 >U2 energy is released.
It I a form of energy which is exchanged between system and surrounding due to difference of temperature. Unit is Joule (J) or Calorie (1 Calorie = 4.18 J).
It is law of conservation energy. Energy can neither be created not destroyed, it may be converted from one from into another. Mathematically ∆U = q + w, w = –p. V∆ (work of expansion) ∆U = q – p. ∆ V or q = ∆ U + p. ∆V, q,w are not state function. ∆But U is state function.
At constant volume ∆V = 0,qv =∆So H = U + p. ∆V, qp = H2 H1 = ∆H ➱ ∆H = ∆ U + P.∆V.
Relationship between qp, qv i.e. ∆H& ∆U It is ∆ H= ∆U+ ∆ng.RT or qp = qv + ∆ ng.RT
∆H = –Ve for exothermic and ∆H = +Ve for endothermic reaction i.e. evolution and absorption of heat.
Eg C+O2 → CO2 + 393.5 KJ, H = –393.5 KJ (exothermic) N2 + O2 → 2NO – 180.7 KJ, H = 180.7 KJ (Endothermic)
The amount of heat evolved or absorbed when the reaction is completed.
Standard Enthalpy of reaction ( ∆ rHo) at 1 bar pressure and specific temp. (290K) i.e. standard state.
|( i ) Enthalpy of combustion (∆cH)||( ii) Enthalpy of formation (∆fH)|
|( iii ) Enthalpy of neutralization||( iv ) Enthalpy of solution|
|( v ) Enthalpy of atomization (∆aH)||( vi ) Enthalpy of Ionisation (∆iH)|
|( vii ) Enthalpy of Hydration (∆hyolH)||( viii ) Enthalpy of fusion (∆fusH)|
|( ix ) Enthalpy of vaporization (∆vapH)||( x ) Enthalpy of sublimation (∆subH)|
(∆subH) = ∆fus(H) - ∆vapH) --------
It is amount of energy released when gaseous atoms combines to form one mole of bonds between them or heat absorbed when one mole of bonds between them are broken to give free gaseous atoms. Further ∆ rH = ∑B.E. (Reactants) - ∑B.E. (Products)
A process which can take place by itself is called spontaneous process. A process which can neither take place by itself or by initiation is called non Spontaneous.
(i) Tendency for minimum energy state.
(ii) Tendency for maximum randomness.
It is measure of randomness or disorder of system.i.e. Gas>Liquid>Solid.
Spontaneity in term of ( ∆S ) ∆S(total) = ∆S(universe) = ∆S(system) + ∆S(surrounding) If ∆S(total) is +ve, the process is spontaneous If ∆S(total) is –ve, the process is non spontaneous.
In any spontaneous process, the entropy of the universe always increases. A spontaneous process cannot be reversed.
defined as G = H – T.S & ∆G = ∆H – T.∆S (Gibb’s Helmholts equation) it is equal useful work .e. - ∆G = W(useful) = W(max).If G = ve, process is spontaneous.
∆G = ∆H – T. ∆ S.
(i) For endothermic process may be non spontaneous at law temp.
(ii) For exothermic process may be non spontaneous at high temp. and spontaneous at law temp.
∆rGo = ∑∆fGo (p) - ∑ ∆fGo (r)
∆G = ∆Go + RTlnQ & ∆Go = –2.303RT logk.
∆rSo = ∑∆ So (p) - So (r)
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