chemistry-class-11-unit-06-chapter-02-chemical-thermodynamics-l-2-8-p6iewcsn1li

### <Success style="font-size:25px"> Chemical Thermodynamics L-2 </Success>
### <primary style="font-size:24px"> Thermodynamics </primary>
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- Essential concepts and definitions
- Heat, work & energy, internal energy
- First Law of thermodynamics
- Calculation of work, heat in different process for an ideal gas
- Enthalpy and heat capacity
- Determination of $\Delta$U and $\Delta$H

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<footer style = "font-size: 18px">Chemical thermodynamics $\rightarrow$  $\rightarrow$ <span style = "color:blue"> Thermodynamics </span> $\rightarrow$ Introduction basic concepts $\rightarrow$ Basic concepts Boundary/Wall </footer>

### <Success style="font-size:25px"> Chemical Thermodynamics L-2 </Success>
### <primary style="font-size:24px"> Introduction basic concepts </primary>
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- System, the part of the world in which is under study
- Surroundings, the region outside the system
- Boundary/Wall, a barrier between system and surroundings
- **Thermodynamic systems**
  - **Open systems** can exchange both matter and energy with the environment
  - **Closed systems** exchange energy but not matter with the environment
  - **Isolated systems** does not interact anyway with the surroundings

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<footer style = "font-size: 18px"> $\rightarrow$ Thermodynamics $\rightarrow$ <span style = "color:blue"> Introduction basic concepts </span> $\rightarrow$ Basic concepts Boundary/Wall $\rightarrow$ Basic concepts state of the system </footer>

### <Success style="font-size:25px"> Chemical Thermodynamics L-2 </Success>
### <primary style="font-size:24px"> Basic concepts Boundary/Wall </primary>
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- Rigid - non-rigid / movable

$\quad\quad\quad\downarrow$

- mechanical exchange / Work 
- Impermeable-permeable (matter is allowed to pass through it)

$\quad\downarrow\quad\quad\quad\quad\quad\quad\downarrow$

- closed system $\quad\quad$ material exchange

- Adiabatic - nonadiabatic / diathermic boundary (permits the passage of heat)

$\quad\quad\quad\downarrow$

- thermal exchange / Heat
- **A system surrounded by a rigid, impermeable, adiabatic wall - Isolated system**

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<footer style = "font-size: 18px">Thermodynamics $\rightarrow$ Introduction basic concepts $\rightarrow$ <span style = "color:blue"> Basic concepts Boundary/Wall </span> $\rightarrow$ Basic concepts state of the system $\rightarrow$ Classification of properties and processes </footer>

### <Success style="font-size:25px"> Chemical Thermodynamics L-2 </Success>
### <primary style="font-size:24px"> Basic concepts state of the system </primary>
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- **How do we define a system? state of a system**
- Macroscopic state of a system can be specified by the values of a small number of macroscopic variables - properties/parameters / thermodynamic variables of a system

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<footer style = "font-size: 18px">Introduction basic concepts $\rightarrow$ Basic concepts Boundary/Wall $\rightarrow$ <span style = "color:blue"> Basic concepts state of the system </span> $\rightarrow$ Classification of properties and processes $\rightarrow$ Classification of properties and processes </footer>

### <Success style="font-size:25px"> Chemical Thermodynamics L-2 </Success>
### <primary style="font-size:24px"> Classification of properties and processes </primary>
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- **Intensive properties** do not depend upon size (the quantity of matter present) of the system at all pressure, temp, viscosity, density etc

- **Extensive properties** depend upon size of the system, mass, volume, surface area etc

- **Homogenoeous system** a system having uniform values of each intensive properties throughout - a single phase - solution / pure

- **Heterogeneous system** a system with more than one phase
- **Phase**- a homogeneous part of a system is called a phase

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<footer style = "font-size: 18px">Basic concepts Boundary/Wall $\rightarrow$ Basic concepts state of the system $\rightarrow$ <span style = "color:blue"> Classification of properties and processes </span> $\rightarrow$ Classification of properties and processes $\rightarrow$ Basic Concepts Equilibrium </footer>

### <Success style="font-size:25px"> Chemical Thermodynamics L-2 </Success>
### <primary style="font-size:24px"> Classification of properties and processes </primary>
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- **Processes** When one or more of the parameters of a system changes, the state of the system also changes and system is undergoing a process

- Isothermal (I), isobaric (p), isochoric (V)

- Cyclic

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<footer style = "font-size: 18px">Basic concepts state of the system $\rightarrow$ Classification of properties and processes $\rightarrow$ <span style = "color:blue"> Classification of properties and processes </span> $\rightarrow$ Basic Concepts Equilibrium $\rightarrow$ Internal energy </footer>

### <Success style="font-size:25px"> Chemical Thermodynamics L-2 </Success>
### <primary style="font-size:24px"> Basic Concepts Equilibrium </primary>
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- **Thermodynamic equilibrium**
- For isolated system
  - Macroscopic properties do not change with time
- For Non isolated system
  - Macroscopic properties do not change with time
  - Removal of the system from contact with its surroundings causes no change in the properties of the system
  - A system in thermodynamic equilibrium is an equilibrium system
  - State of a thermodynamic only defined by the present values of the state variables not by the history

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<footer style = "font-size: 18px">Classification of properties and processes $\rightarrow$ Classification of properties and processes $\rightarrow$ <span style = "color:blue"> Basic Concepts Equilibrium </span> $\rightarrow$ Internal energy $\rightarrow$ Internal energy </footer>

### <Success style="font-size:25px"> Chemical Thermodynamics L-2 </Success>
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- Internal energy (U) - due to molecular motions + intermolecular interactions
- U = molecular traslation, rotational, vibrational, and electronic energies, +relativistic rest-mass energy, $m_{rest}$ C² of electrons ad the nuclei+potential energy of interaction between the molecules
- U =$f(T,V,n_1,n_2....)$
- $\Delta$U = f(T,V,)
- ideal gass U = f(T)
- $\Delta$U =f(T)

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<footer style = "font-size: 18px">Classification of properties and processes $\rightarrow$ Basic Concepts Equilibrium $\rightarrow$ <span style = "color:blue"> Internal energy </span> $\rightarrow$ Internal energy $\rightarrow$ Internal energy </footer>

### <Success style="font-size:25px"> Chemical Thermodynamics L-2 </Success>
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- $\Delta$u=q+w (closed system) first
- Increase in energy of the system due to heat exchange between system and surroundings across a non-adiabatic wall
- W = increase in energyu of the system due to exchange of energy as work between system and surroundings across a non-rigid wall
- An isolated system, $\Delta$u=0
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<footer style = "font-size: 18px">Internal energy $\rightarrow$ Internal energy $\rightarrow$ <span style = "color:blue"> Internal energy </span> $\rightarrow$ Internal energy $\rightarrow$ Internal energy </footer>

### <Success style="font-size:25px"> Chemical Thermodynamics L-2 </Success>
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- Force = $P_{ex}.A$
- Work done = force × distance
- $P_{ex}.A.l $
- $P_{ex}\Delta$v
- $P_{ex}(V_f-V_i)$
- W=-$P_{ex}(V_f-V_i)$

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### <Success style="font-size:25px"> Chemical Thermodynamics L-2 </Success>
### <primary style="font-size:24px"> Internal energy </primary>
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- $\omega$ depends on path which has bean adopted for going from state 1 to state 2
- $\Delta$U = q + w

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<footer style = "font-size: 18px">Internal energy $\rightarrow$ Internal energy $\rightarrow$ <span style = "color:blue"> Internal energy </span> $\rightarrow$ Reversible process $\rightarrow$ Reversible process </footer>

### <Success style="font-size:25px"> Chemical Thermodynamics L-2 </Success>
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- Reversible process
- Is a process where system is always infinisimally close to equilibrium, an infinisimal change in condition can reverse the process to restore both system and surroundings to the initial state
- $P_{ex}$ -P  infinisimally small
- Infinisimally slow process - infinite time - idealized

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<footer style = "font-size: 18px">Internal energy $\rightarrow$ Internal energy $\rightarrow$ <span style = "color:blue"> Reversible process </span> $\rightarrow$ Reversible process $\rightarrow$ # Isothermal reversible process of an ideal gas </footer>

### <Success style="font-size:25px"> Chemical Thermodynamics L-2 </Success>
### <primary style="font-size:24px"> Reversible process </primary>
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- dw = -$P_{ex} dv $  ( $P_{ex}≈P$)
- dw =-pdv   (reversible process)
- w = $\int^2_1$pdv = reversible process
- w = -$P_{ex}\Delta$V = irreversible process
- Ideal gas $p=\frac{nRT}{V}$
- w = $\int^{v_2}_{v_1}\frac{nRT}{V} dv \Rightarrow $ isothermal process
- $ w = nRT\int^{v_2}_{v_1} \frac{dv}{V}$
- w  = nRT $ln \frac{V_2}{V_1}$

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<footer style = "font-size: 18px">Internal energy $\rightarrow$ Reversible process $\rightarrow$ <span style = "color:blue"> Reversible process </span> $\rightarrow$ # Isothermal reversible process of an ideal gas $\rightarrow$ Adiabatic process </footer>

### <Success style="font-size:25px"> Chemical Thermodynamics L-2 </Success>
### <primary style="font-size:24px"> # Isothermal reversible process of an ideal gas </primary>
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- w = -nRT $ln\frac{V_2}{V_1}$
- $\Delta u = 0$ , q= -w
- Compression $V_2 < V_1, \quad w > 0$
- expansion $V_2 > V_1 , \quad w < 0$
- **Free expansion**
- $P_{ex} = 0$
- $w =-P_{ex} \Delta V = 0$
- **isothermal process for ideal gas**
- $\Delta V= 0$ , $q=0$

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<footer style = "font-size: 18px">Reversible process $\rightarrow$ Reversible process $\rightarrow$ <span style = "color:blue"> # Isothermal reversible process of an ideal gas </span> $\rightarrow$ Adiabatic process $\rightarrow$ Isobaric process </footer>

### <Success style="font-size:25px"> Chemical Thermodynamics L-2 </Success>
### <primary style="font-size:24px"> Isobaric process </primary>
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- Isobaric process, constant P process 
- $\Delta u= q+w$
- $q_p - p\Delta v$
- $U_2-U_1 = q_p -p(V_2 -V_1)$
- $\therefore q_p = (U_2 + P_{v_2}) - (U_1 + P_{v_1})$
- New thermodynamic parameter $H = U + PV$
- enthalpy - "enthalpien" to work or heat content.....
- $\Delta H = H_2 -H_1$

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<footer style = "font-size: 18px"># Isothermal reversible process of an ideal gas $\rightarrow$ Adiabatic process $\rightarrow$ <span style = "color:blue"> Isobaric process </span> $\rightarrow$ Isobaric process $\rightarrow$ Isobaric process </footer>

### <Success style="font-size:25px"> Chemical Thermodynamics L-2 </Success>
### <primary style="font-size:24px"> Isobaric process </primary>
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- $q_p = (U_2 + P{V_2}) - ( U_1 + P{V_1})$
- $ H  = U + PV$
- $q_p = H_2 - H_1 = \Delta H$
- Heat absorbed by the system at constant p
- exothermic process,$\Delta H <0$
- endothermic process, $ \Delta H > 0$
- $\Delta H = \Delta U + \Delta PV$
- for liquids and solids
- $\Delta H \approx \Delta U $

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<footer style = "font-size: 18px">Adiabatic process $\rightarrow$ Isobaric process $\rightarrow$ <span style = "color:blue"> Isobaric process </span> $\rightarrow$ Isobaric process $\rightarrow$ Thank you </footer>