Download JEE Chemistry Concept Summaries: JEE Chemistry Thermodynamics Notes Set 01
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Basic Terms
1. State functions depend only on the state: \(U, H, S, G\). Path functions are \(q\) and \(w\).
2. First law: \(\Delta U = q + w\), with \(w\) positive when work is done on the system. At constant volume \(q_v = \Delta U\); at constant pressure \(q_p = \Delta H\).
3. Reversible processes proceed through equilibrium states, and a cyclic process has zero change in every state function.
Key Formulas
| Topic | Formula |
|---|---|
| Isothermal reversible work on gas | \(w = -nRT\ln(V_2/V_1) = nRT\ln(P_2/P_1)\) |
| Entropy change of ideal gas, isothermal | \(\Delta S = nR\ln(V_2/V_1)\) |
| Heat from heat capacity | \(q = nC\Delta T\) |
| Enthalpy of reaction | \(\Delta H = \sum \Delta H_f(\text{products}) - \sum \Delta H_f(\text{reactants})\) |
| Fuel cell efficiency | \(\Delta G/\Delta H\) |
| Resonance energy | Observed \(\Delta H_f\) minus bond-energy \(\Delta H_f\) |
1. Hess's law: the total enthalpy change is the same by any route. Reverse a reaction to change the sign, multiply to scale.
2. Neutralisation of a strong acid and strong base releases about 57.1 kJ per mole of water, so find the limiting reagent first.
3. Sign of \(\Delta S\): increases when the number of gas moles increases. A reaction is spontaneous when \(\Delta G < 0\).
Free study material for Chemistry
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About Thermodynamics Revision Notes
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