Home
Learn
Plan & Focus
Community
Pricing
Play & Compete
Free Resources

Log in Join Free

by JEE Master

Ask. Share. Learn. Grow Together. India's all-in-one community for JEE Main & JEE Advanced aspirants.

Explore

Learn
Plan & Focus
Community
Play & Compete
Free Resources

Resources

JEE Main PYQs
JEE Advanced PYQs
Formula Sheets
NCERT Mapping
Mock Analysis

Support

Help Center
Privacy Policy
Terms of Use
Contact Us

© 2026 PadhoNa. All rights reserved.

Formula Sheets / Chemistry

Chapter 5

Thermodynamics

Revise with flashcards Download this chapter (PDF) All Chemistry formulas (PDF)

First law and work Enthalpy changes Entropy, Gibbs energy and equilibrium

First law and work

$Δ U = q + w (w = - P_{ext} Δ V$ for expansion $)$
Reversible isothermal
$w = - 2.303 n R T lo g \frac{V _{2}}{V _{1}}$
$Δ H = Δ U + Δ n_{g} R T,$ $C_{p} - C_{v} = R$

Enthalpy changes

Hess's law
$Δ_{r} H = \sum Δ_{f} H_{products} - \sum Δ_{f} H_{reactants}$
From bond enthalpies
$Δ H \approx - 57.1$ BE $_{bonds broken} - \sum$ BE $_{bonds formed}$
Neutralisation
$Δ H \approx - 57.1$ kJ mol $^{- 1}$ (strong acid + strong base)

Entropy, Gibbs energy and equilibrium

$Δ G^{\circ} = - R T ln K = - 2.303 R T lo g K;$ $Δ G = Δ H - T Δ S$
$Δ G^{\circ} = - R T ln K = - 2.303 R T lo g K;$ $Δ G = Δ G^{\circ} + R T ln Q$
Spontaneity
$Δ G < 0$ spontaneous $;$ $T = \frac{Δ H}{Δ S}$ at the switch
Phase change
$Δ S = \frac{Δ H _{trans}}{T}$

Chemical Bonding and Molecular Structure States of Matter