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Thermodynamics & Thermochemistry formulas

Master Thermodynamics & Thermochemistry through 22 JEE Advanced-level formulas, systematically structured with every variable spelled out. Revise concept-wise, identify the areas where you need improvement, and focus your preparation with greater precision.

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Thermodynamics & Thermochemistry, every formula

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First law of thermodynamics
$Δ U = q + W$
Q1MCQFirst law
The first law of thermodynamics is:
- A
  $\Delta U=q+W$
- B
  $\Delta U=q-W$
- C
  $q=\Delta U$
- D
  $W=\Delta U$
Work of expansion
$W = - P_{e x t} Δ V$
Enthalpy
$H = U + P V$
Q1MCQEnthalpy
Enthalpy is defined as:
- A
  $U+PV$
- B
  $U-PV$
- C
  $PV$
- D
  $U$
Enthalpy change
$Δ H = Δ U + Δ n_{g} R T$
Q1MCQΔH–ΔU
For a gaseous reaction, $\Delta H$ equals:
- A
  $\Delta U+\Delta n_g RT$
- B
  $\Delta U-\Delta n_g RT$
- C
  $\Delta U$
- D
  $\Delta n_g RT$
Heat at constant volume
$q_{v} = Δ U$
Q1MCQq at const V
At constant volume, the heat absorbed equals:
- A
  $\Delta U$
- B
  $\Delta H$
- C
  $W$
- D
  $0$
Heat at constant pressure
$q_{p} = Δ H$
Q1MCQq at const P
At constant pressure, the heat absorbed equals:
- A
  $\Delta H$
- B
  $\Delta U$
- C
  $W$
- D
  $0$
Isothermal reversible work
$W = - n R T ln \frac{V _{2}}{V _{1}}$
Q1MCQIsothermal work
The reversible isothermal work of an ideal gas is:
- A
  $-nRT\ln\dfrac{V_2}{V_1}$
- B
  $-P\Delta V$
- C
  $nRT$
- D
  $0$
Adiabatic condition
$q = 0, Δ U = W$
Q1MCQAdiabatic
In an adiabatic process:
- A
  $q=0$ and $\Delta U=W$
- B
  $\Delta U=0$
- C
  $W=0$
- D
  $\Delta H=0$
Cp − Cv (ideal gas)
$C_{p} - C_{v} = R$
Q1MCQCp − Cv
For an ideal gas, $C_p-C_v$ equals:
- A
  $R$
- B
  $\dfrac{R}{2}$
- C
  $2R$
- D
  $0$
Enthalpy of reaction (Hess)
$Δ H = \sum Δ H_{p r o d u c t s} - \sum Δ H_{r e a c t an t s}$
Q1MCQHess's law
By Hess's law, the enthalpy of reaction is:
- A
  $\sum\Delta H_{prod}-\sum\Delta H_{react}$
- B
  $\sum\Delta H_{react}-\sum\Delta H_{prod}$
- C
  $0$
- D
  $\sum\Delta H_{prod}$
Bond enthalpy
$Δ H = \sum (bonds broken) - \sum (bonds formed)$
Q1MCQBond enthalpy
Using bond enthalpies, $\Delta H$ equals:
- A
  bonds broken $-$ bonds formed
- B
  bonds formed $-$ bonds broken
- C
  bonds broken
- D
  $0$
Entropy change
$Δ S = \frac{q _{r e v}}{T}$
Q1MCQEntropy change
The entropy change of a reversible process is:
- A
  $\dfrac{q_{rev}}{T}$
- B
  $q_{rev}T$
- C
  $\dfrac{T}{q_{rev}}$
- D
  $q_{rev}$
Gibbs free energy
$Δ G = Δ H - T Δ S$
Q1MCQGibbs energy
The Gibbs free energy change is:
- A
  $\Delta H-T\Delta S$
- B
  $\Delta H+T\Delta S$
- C
  $T\Delta S-\Delta H$
- D
  $\Delta H$
Spontaneity criterion
$Δ G < 0 (spontaneous)$
Q1MCQSpontaneity
A process is spontaneous when:
- A
  $\Delta G<0$
- B
  $\Delta G>0$
- C
  $\Delta G=0$
- D
  $\Delta H<0$ only
Free energy and equilibrium
$Δ G^{\circ} = - R T ln K$
Q1MCQΔG° and K
The relation between $\Delta G^{\circ}$ and the equilibrium constant is:
- A
  $\Delta G^{\circ}=-RT\ln K$
- B
  $\Delta G^{\circ}=RT\ln K$
- C
  $\Delta G^{\circ}=-\dfrac{RT}{\ln K}$
- D
  $\Delta G^{\circ}=K$
Entropy of surroundings
$Δ S_{s u r r} = - \frac{Δ H}{T}$
Q1MCQEntropy of surroundings
The entropy change of the surroundings is:
- A
  $-\dfrac{\Delta H}{T}$
- B
  $\dfrac{\Delta H}{T}$
- C
  $\Delta H T$
- D
  $0$
Second law
$Δ S_{t o t a l} = Δ S_{sy s} + Δ S_{s u r r} > 0$
Q1MCQSecond law
For a spontaneous process, the total entropy change is:
- A
  $>0$
- B
  $<0$
- C
  $=0$
- D
  undefined
Heat capacity
$q = n C Δ T$
Enthalpy of neutralization
$Δ H \approx - 57.1 kJ/mol$
strong acid + strong base
Q1MCQNeutralization
The enthalpy of neutralization of a strong acid and strong base is about:
- A
  $-57.1$ kJ/mol
- B
  $-13.6$ kJ/mol
- C
  $-100$ kJ/mol
- D
  $0$
Relation ΔG and ΔG°
$Δ G = Δ G^{\circ} + R T ln Q$
Q1MCQΔG and Q
The relation between $\Delta G$ and $\Delta G^{\circ}$ is:
- A
  $\Delta G=\Delta G^{\circ}+RT\ln Q$
- B
  $\Delta G=\Delta G^{\circ}-RT\ln Q$
- C
  $\Delta G=RT\ln Q$
- D
  $\Delta G=\Delta G^{\circ}$
Efficiency of a Carnot engine
$η = 1 - \frac{T _{2}}{T _{1}}$
Internal energy (ideal gas)
$Δ U = n C_{v} Δ T$
Q1MCQΔU ideal gas
The internal energy change of an ideal gas is:
- A
  $nC_v\Delta T$
- B
  $nC_p\Delta T$
- C
  $nR\Delta T$
- D
  $0$

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Thermodynamics & Thermochemistry formulas

Thermodynamics & Thermochemistry, every formula

First law of thermodynamics

Work of expansion

Enthalpy

Enthalpy change

Heat at constant volume

Heat at constant pressure

Isothermal reversible work

Adiabatic condition

Cp − Cv (ideal gas)

Enthalpy of reaction (Hess)

Bond enthalpy

Entropy change

Gibbs free energy

Spontaneity criterion

Free energy and equilibrium

Entropy of surroundings

Second law

Heat capacity

Enthalpy of neutralization

Relation ΔG and ΔG°

Efficiency of a Carnot engine

Internal energy (ideal gas)

More JEE Advanced Chemistry formula sheets

Other ways to revise this chapter

Preparing students for India’s top institutes

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