Physical Chemistry
Mole concept, stoichiometry, thermodynamics, chemical equilibrium, and solutions
Key Concepts
- Mole concept and stoichiometry underpin all quantitative chemistry
- Thermodynamics: spontaneity is decided by Gibbs free energy
- Chemical equilibrium: Le Chatelier's principle predicts the shift
- Electrochemistry: the Nernst equation relates EMF to concentration
- Chemical kinetics: rate laws are determined experimentally
Important Formulae
| Number of moles | n = m/M |
| Ideal gas law | PV = nRT |
| Gibbs free energy | ΔG = ΔH − TΔS |
| Kp from Kc | Kp = Kc(RT)^Δn |
| Nernst equation | E = E° − (RT/nF) ln Q |
| First-order half-life | t₁/₂ = 0.693/k |
Quick Tips
- Always balance the equation before any stoichiometric calculation.
- ΔG < 0 means spontaneous; ΔG = 0 means equilibrium.
- For gases, 1 mole occupies 22.4 L at STP.
Sample Practice Questions
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For a spontaneous reaction, the Gibbs free energy change ΔG is:
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Answer: Negative
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Avogadro's number is approximately:
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Answer: 6.022×10²³
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The pH of a neutral aqueous solution at 25 °C is:
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Answer: 7
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The number of moles in 36 g of water (molar mass 18 g/mol) is:
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Answer: 2
Practice Questions
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What are the key concepts in Physical Chemistry for JEE?
Mole concept and stoichiometry underpin all quantitative chemistry; Thermodynamics: spontaneity is decided by Gibbs free energy; Chemical equilibrium: Le Chatelier's principle predicts the shift; Electrochemistry: the Nernst equation relates EMF to concentration; Chemical kinetics: rate laws are determined experimentally.
Which formulae are important for Physical Chemistry in JEE?
Number of moles: n = m/M; Ideal gas law: PV = nRT; Gibbs free energy: ΔG = ΔH − TΔS; Kp from Kc: Kp = Kc(RT)^Δn; Nernst equation: E = E° − (RT/nF) ln Q; First-order half-life: t₁/₂ = 0.693/k.
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