Thermodynamics class 11 physics

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This PPT is about thermodynamics. It explains isothermal, isobaric, adiabatic, and isochoric processes. In-depth explanation of formulae and derivation is provided.

1. THERMODYNAMIC PROCESSES By Mohammed Afzal 11A

2. Introduction: Conducting Insulating

3. Types of System: (Diathermic) 1)

4. Types of System: 2 )

5. Types of System: 3 )

6. Depends on amount of matter. Eg;- Mass,Vol,Moles,Heat Capacity,Energy,Enthalpy,Entropy,Gibb’s Free Energy,Internal energy Does not depend on matter. Eg:- Density,Refractive index, specific heat capacity,pressure,temp,viscosity,concentration Molarity,Molality,mole fraction,normality,molar entropy,molar enthalpy,internal energy. Extensive: Intensive :

7. Depends on initial and final state of a system. Does not depend on path of flow. Eg:-Pressure(P),Temp(T),Volume(V),moles(n), Enthalpy(H),Entropy(S),Internal Energy(U),Gibbs Free Energy(G) Depends on path of flow. Eg:-Heat(Q),Work(W) State Functions: Path Functions:

8. Cyclic Process: P V ΔP=0 ΔT=0 ΔE=0 ΔV=0 ΔS=0 ΔQ≠0 ΔW≠0

9. Gram SHC : c = Q/mΔT Molar SHC : C = Q/nΔT C isothermal -> ∞ C adiabatic = 0 (For gases) c = 4.2 J/g °C (Water) c v = Q/mΔT (At constant vol) C v = Q/nΔT (At constant vol) c P = Q/mΔT (At constant pressure) C P = Q/nΔT (At constant pressure) C v =Mc v C P= Mc P C P - C V = R C V = (f/2)R C P = (f/2 + 1)R γ=C P /C V Specific Heat Capacity:

10. f(degree of freedom) C v = (f/2)R C P = C V + R γ=C P /C V 3(Monoatomic) 3R/2 5R/2 5/3 = 1.66 5(Diatomic) 5R/2 7R/2 7/5 = 1.4 6(Polyatomic) 7R/2 4R 4/3 = 1.33 γ= 1 + 2/f

11. PV Graph for all processes: P V Isobaric Isochoric Isothermal Adiabatic Isobaric:ΔP=0 Isochoric:ΔV=0 Isothermal:ΔT=0 Adiabatic:ΔQ=0

12. Occurs in infinitely small steps -> Infinite time to finish. Slow Each step in equilibrium. Not practical. W = - ∫ P ext dV Occurs at once -> finite time. Fast Equilibrium initially and finally only. Practical situation. W = - 𝝨pΔV Reversible Process: Irreversible Process:

13. Heat given to the system -> +ve Heat given by the system -> -ve Work done on a system -> +ve Work done by a system -> -ve Conventions:

14. W=PV relation: P ext = F/A ⟹ F = P ext x A W = F Δx = P ext A Δ x ⟹ W = - P ext ΔV Why -ve? By convention

15. P V d V P ∫ dW = ∫ P dV W = - ∫ P ext dV = Area under P-V Graph Expansion: W = -ve Compression: W = +ve

16. Cyclic Process: P V W net = Area of shape(ie square in this case) enclosed -ve for clockwise (as in this case) +ve for anti-clockwise

17. Isobaric(Δp=0): W= -Pext ΔV Isochoric(ΔV=0): W = 0 Vacuum(Free Expansion): P ext = 0 ⟹ W = 0 Isobaric and Isochoric processes:

18. W = - ∫ Pext dV = - ∫ nRT dV/V = - nRT ln (V2/V1) = - 2.303 nRT log 10 (V2/V1) = - 2.303 nRT log 10 (P2/P1) = - 2.303 P 1 V 1 log 10 (V2/V1) = - 2.303 P 2 V 2 log 10 (V2/V1) = - 2.303 P 1 V 1 log 10 (P2/P1) = - 2.303 P 2 V 2 log 10 (V2/V1) Isothermal process

19. Adiabatic Process