Merge pull request #18 from cse23-mora/sangeeth

added thermo notes

Author: NipunSGeeTH

src/content/docs/3rd-semester/thermodynamics/1.Types of systems.md

@@ -0,0 +1,59 @@
+---
+title: Types of systems
+description: ""
+---
+
+## Types of systems
+| open systems  | closed systems | Isolated systems |
+|-|-|-|
+| Mass  transfer ✔  | ~~Mass transfer~~  | ~~Mass transfer~~|
+| Energy tranfer ✔ |  Energy tranfer ✔ | ~~Energy tranfer~~ |
+
+## Thermodynamics Properties
+
+
+| Intensitive properties<br> (not dependent on mass) |Extensive properties <br> (dependent on mass)| 
+|-|-|
+| Pressure  | Mass | 
+| Temperature  |  |
+|Specific enthalpy (h)| Enthalpy (H) |
+| Specific volume (v)| Volume (V)   |
+|Specific entropy (s)| Entropy (S) |
+| Specific heat capacity | Heat capacity|
+| Specific internal energy (u)| Internal energy (U)| 
+
+
+#### * All Properties are point functions (state functions)
+####  * Work and Heat are path functions .Therefore, work and heat are not properties of a thermodynamic system; they are path-dependent quantities.
+
+
+## Thermodynamic Equilibrium
+
+#### for thermodynamic equilibrium, following must be true
+1. Mechanical Equilibrium
+2. Chemical Equilibrium
+3. Phase Equilibrium
+4. Thermal Equilibrium
+
+
+
+## Common thermodynamic processes
+1. Isobaric Process --> Pressure constant
+2. Isochoric Process --> Volume constant
+3. Isothermal Process --> Temperature constant
+4. Adiabatic Process -->  ΔQ =0 (no heat transfer)
+5. Isentropic Process --> Entropy constant
+6. Polytropic Process --> PV<sup>n</sup> = C ;   n := polytropic index
+
+
+* $PV^n=C$ </br>
+n=0 : Isobaric </br>
+n=1 : Isothermal </br>
+n -->  ∞: Isochoric
+
+
+#### *For an isentropic process in an ideal gas
+$ PV^γ  = C $ </br>
+γ  --> heat capacity ratio </br>
+$ γ  = \frac{C_p}{C_v} $   and    $C_p$ > $C_v$</br>
+

src/content/docs/3rd-semester/thermodynamics/2.Zeroth law and first law.md

@@ -0,0 +1,70 @@
+---
+title: 2.Zeroth law and first law
+
+---
+
+## Zeroth Law
+
+> If two systems are each in thermal equilibrium with a third system, then they are also in thermal equilibrium with each other
+
+![alt text](<2.Zeroth law and first law/image-1.png>)
+
+
+
+## First Law 
+
+> Enegy cannot be created and it cannot be destroyed. </br>
+
+“When a system (closed) undergoes a thermodynamic
+cycle, sum of the net heat supplied to the system from its
+surroundings and the net work input to the system from
+its surroundings must equal zero"
+
+$\Sigma Q + \Sigma W = 0 $
+
+$\ Q $ Heat transfer in to the system <br>
+$\ W $ Work transfer in to the system
+
+
+![alt text](<2.Zeroth law and first law/image-2.png>)
+
+- Heat supplied to the system - POSITIVE
+- Work done by the system - POSITIVE
+- Heat rejected by the system - NEGATIVE
+- Work done on the system - NEGATIVE
+
+
+### - Corollary
+
+* The internal energy of a closed system remain
+unchanged if the system is isolated from its
+surrounding
+
+$ \Sigma (Q + W) = \Delta U $  `                      `  if 𝐼𝑓 𝑄 = 0 𝑎𝑛𝑑 𝑊 = 0 𝑡ℎ𝑒𝑛, ∆𝑈 = 0
+
+
+### - Corollary
+*   For a cycle, the net work done by the system is equal to the net heat added to the system.
+
+
+ #### Energy balance for closed system: <br>
+  $ heat + work = total \space  energy $<br>
+  $ Q -W = \Delta E$ <br>
+  $Q - W = \Delta U + \Delta KE + \Delta PE$ <br>
+  $E = U + \frac{1}{2}mC^2 + mgz$
+
+  $\therefore $ Specific total energy $e = u + \frac{1}{2} C^2 + gz$
+
+
+## note
+* Transient state  - Change with time
+* Steady state - No change with time
+* Heat and work depend on the path it followed.
+They are called “path functions”.
+
+
+
+
+
+
+