Chemistry Concept Notes for JEE: Thermodynamics
Explore reliable concept summaries and revision materials through the JEE Chemistry Thermodynamics Notes Set 02. Tailored for JEE learners, utilizing these notes for Chemistry Thermodynamics ensures thorough preparation and strengthens core academic definitions before final evaluations.
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Access the complete concept summary PDF for Thermodynamics below. Regular review of these targeted notes builds familiarity with complex JEE Chemistry themes and helps secure higher marks in final school evaluations.
Basic Terms and the First Law
1. System, surroundings and boundary. An open system exchanges matter and energy, a closed system exchanges energy only, an isolated system exchanges neither.
2. State functions (U, H, S, G, P, V, T) depend only on the present state of the system. Path functions (q and w) depend on how the change is carried out. Extensive properties depend on the amount of matter (U, H, S, G, V); intensive ones do not (T, P, density, pH, boiling point).
3. Sign convention used here: heat absorbed by the system and work done on the system are positive. Then \(\Delta U=q+w\) is the first law.
Work
| Process | Work done on the gas |
|---|---|
| Expansion against constant external pressure | \(w=-P_{ext}(V_2-V_1)\) |
| Free expansion into vacuum | \(w=0\) |
| Reversible isothermal (ideal gas) | \(w=-nRT\ln\dfrac{V_2}{V_1}=-nRT\ln\dfrac{P_1}{P_2}\) |
| Reversible adiabatic (ideal gas) | \(w=nC_V(T_2-T_1)\) with \(TV^{\gamma-1}=\) constant, \(PV^{\gamma}=\) constant |
| Irreversible adiabatic (single step) | \(nC_V(T_2-T_1)=-P_{ext}(V_2-V_1)\) |
| Isochoric | \(w=0\) |
The reversible path gives the maximum work obtained from the system in an expansion and the minimum work needed in a compression. The area under the curve on a P-V graph is the magnitude of the work.
Internal Energy, Enthalpy and Heat Capacity
1. \(H=U+PV\), so \(\Delta H=\Delta U+\Delta n_gRT\) for a reaction at constant temperature involving gases.
2. At constant volume \(q_V=\Delta U\); at constant pressure \(q_P=\Delta H\).
3. For an ideal gas, U and H depend only on temperature: \(\Delta U=nC_V\Delta T\), \(\Delta H=nC_P\Delta T\) for every process, and \(C_P-C_V=R\).
4. \(C_V=\tfrac32R\) (monatomic), \(\tfrac52R\) (diatomic, no vibration), \(3R\) (non-linear polyatomic); \(\gamma=C_P/C_V\).
5. Kirchhoff's law: \(\Delta H_{T_2}=\Delta H_{T_1}+\Delta C_P(T_2-T_1)\).
6. For solids and liquids \(\Delta H\approx\Delta U\) because the volume change is tiny.
Special Processes of an Ideal Gas
| Process | q | \(\Delta U\) | w (on gas) |
|---|---|---|---|
| Isothermal | \(-w\) | 0 | \(-nRT\ln(V_2/V_1)\) |
| Isochoric | \(nC_V\Delta T\) | \(nC_V\Delta T\) | 0 |
| Isobaric | \(nC_P\Delta T\) | \(nC_V\Delta T\) | \(-nR\Delta T\) |
| Adiabatic | 0 | \(nC_V\Delta T\) | \(\Delta U\) |
Remember
1. In any cycle \(\Delta U=0\), so heat absorbed equals work done by the system.
2. A line through the origin on a V-T graph is isobaric; a vertical line is isothermal; a horizontal line is isochoric.
3. Adiabatic compression heats a gas and adiabatic expansion cools it.
4. An irreversible adiabatic expansion cools the gas less than a reversible one.
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Study Material and Revision Notes for JEE Chemistry Thermodynamics
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