The temperature rise depends directly on the total heat released (Q$Q$) normalized by the total heat capacity of the resulting mixed volume (m · c$m \cdot c$). Let's evaluate the millimoles of H^+$\mathrm{H}^+$ and OH^-$\mathrm{OH}^-$ that react in each mixture:
Option 1:30 mL of 1M HCl + 30 mL of 1M NaOH$30\text{ mL of } 1\mathrm{M } \mathrm{HCl} + 30\text{ mL of } 1\mathrm{M } \mathrm{NaOH}$
Reactive millimoles = 30 mmol$\text{Reactive millimoles} = 30\text{ mmol}$. Both are strong electrolytes, releasing full neutralization energy (-57.3 kJ/mol$\sim -57.3\text{ kJ/mol}$).
Total volume = 60 mL$60\text{ mL}$.
Option 2:30 mL of 1M CH₃COOH + 30 mL of 1M NaOH$30\text{ mL of } 1\mathrm{M } \mathrm{CH_3COOH} + 30\text{ mL of } 1\mathrm{M } \mathrm{NaOH}$
Reactive millimoles = 30 mmol$\text{Reactive millimoles} = 30\text{ mmol}$. However, since acetic acid is a weak acid, part of the heat is consumed in its ionization. Thus, less total heat is evolved compared to Option 1.
Option 3:50 mL of 1M HCl + 20 mL of 1M NaOH$50\text{ mL of } 1\mathrm{M } \mathrm{HCl} + 20\text{ mL of } 1\mathrm{M } \mathrm{NaOH}$
Comparing Option 1 and Option 3, Option 1 releases significantly more heat (30 mmol$30\text{ mmol}$ vs 20 mmol$20\text{ mmol}$) into a smaller volume (60 mL$60\text{ mL}$ vs 70 mL$70\text{ mL}$), yielding the largest increase in temperature Δ T$\Delta T$.
Pattern Recognition
To maximize Δ T$\Delta T$, look for the option that maximizes the amount of reacting strong acid and strong base equivalents while keeping the total solution volume as small as possible.
Chapter Mix
Class 11 Chemistry: Thermodynamics
Class 11 Chemistry: Equilibrium
Keywords:#heat of neutralization#maximum temperature rise acid base#JEE Main 2025 Evening Q31#Thermodynamics calorimetry
More Thermodynamics Previous-Year Questions
Q68jee_main_2026_21_jan_morningWork Done in PV Graph
Which of the following graphs between pressure ‘P’ versus volume ‘V’ represent the maximum work done?
A.Option 1$\text{Option 1}$
B.Option 2$\text{Option 2}$
C.Option 3$\text{Option 3}$
D.Option 4$\text{Option 4}$
Solution
Core Logic
The magnitude of work done by or on a gas is given by the area under the P-V curve projected onto the volume axis.
Graph 1: Cyclic process forming a triangle. Area is bounded, represents net work.
Graph 2: Isochoric drop (vertical line at V=22.4L$V=22.4L$). Area = 0, so work done is zero.
Graph 3: Expansion process forming a cycle. Area is enclosed in a convex shape.
Graph 4: Direct expansion from V=22.4$V=22.4$ to V=44.8$V=44.8$ at pressure P=1$P=1$ up to P=2$P=2$ (a rectangle combined with a triangle). The total area under the upper curve from V=22.4$V=22.4$ to V=44.8$V=44.8$ covers the entire shaded region under the path down to the V-axis.
Option (4) provides the largest total area under the curve extending down to the horizontal axis (maximum magnitude of work done).
Chapter Mix
Class 11 Chemistry: Thermodynamics
Q69jee_main_2026_21_jan_morningGibbs Free Energy and Equilibrium
For the reaction, N₂O₄ leftharpoons 2NO₂$N_{2}O_{4} \rightleftharpoons 2NO_{2}$, graph is plotted as shown below. Identify correct statements.
A. Standard free energy change for the reaction is -5.40 kJ mol⁻¹$-5.40\text{ kJ mol}^{-1}$.
B. As Δ G$\Delta G^{\ominus}$ in graph is positive, N₂O₄$N_{2}O_{4}$ will not dissociate into NO₂$NO_{2}$ at all.
C. Reverse reaction will go to completion.
D. When 1 mole of N₂O₄$N_{2}O_{4}$ changes into equilibrium mixture, value of Δ G = -0.84 kJ mol⁻¹$\Delta G = -0.84\text{ kJ mol}^{-1}$.
E. When 2 mole of NO₂$NO_{2}$ changes into equilibrium mixture, Δ G$\Delta G$ for equilibrium mixture is -6.24 kJ mol⁻¹$-6.24\text{ kJ mol}^{-1}$.
A plot of Gibbs free energy against the fraction of N2O4 dissociated.
Choose the correct answer from the options given below :
A.D and E only$\text{D and E only}$
B.C and E only$\text{C and E only}$
C.A and D only$\text{A and D only}$
D.B and C only$\text{B and C only}$
Solution
Core Logic
Let's analyze the statements based on the given Gibbs free energy (G) vs. extent of reaction plot.
A plot of Gibbs free energy against the fraction of N2O4 dissociated.
A. Standard free energy change (Δᵣ G°$\Delta_r G^{\circ}$) is the difference between standard free energies of pure products (point B) and pure reactants (point A): Δᵣ G° = GB° - GA°$\Delta_r G^{\circ} = G_B^{\circ} - G_A^{\circ}$. Since B is higher than A, Δᵣ G°$\Delta_r G^{\circ}$ is positive, not -5.40 kJ mol⁻¹$-5.40\text{ kJ mol}^{-1}$. Statement A is false.
B. Even if Δᵣ G°$\Delta_r G^{\circ}$ is positive, the minimum of the curve (equilibrium state E) lies between the pure reactant and product states. Therefore, partial dissociation occurs to reach equilibrium. It is false to say it will not dissociate at all. Statement B is false.
C. The minimum E is not at fraction = 0 or 1, meaning an equilibrium mixture exists. Reverse reaction does not go to completion. Statement C is false.
D. From 1 mole of pure reactant (point A) to the equilibrium mixture (point E), the drop in Gibbs energy is 0.84 kJ mol⁻¹$0.84\text{ kJ mol}^{-1}$. Thus Δ G = -0.84 kJ mol⁻¹$\Delta G = -0.84\text{ kJ mol}^{-1}$ is correct. Statement D is true.
E. The difference from pure products (point B, equivalent to 2 moles NO₂$NO_2$) to equilibrium (E) is the entire vertical distance. The drop from B to A is 5.40$5.40$, and A to E is 0.84$0.84$. So drop from B to E is - (5.40 + 0.84) = -6.24 kJ mol⁻¹$- (5.40 + 0.84) = -6.24\text{ kJ mol}^{-1}$. Statement E is true.
Step 1: Final Conclusion
Only statements D and E are correct.
Pattern Recognition
The free energy of mixing creates a minimum 'dip' (Equilibrium) below both pure reactants and pure products, preventing either forward or reverse reactions from going absolutely to 100% completion.
Chapter Mix
Class 11 Chemistry: Thermodynamics
Class 11 Chemistry: Equilibrium
Q73jee_main_2026_21_jan_morningGibbs Free Energy and Equilibrium Constant
One mole each of A₂(g)$A_{2}(g)$ and B₂(g)$B_{2}(g)$ are taken in a 1L closed flask and allowed to establish the equilibrium at 500K.
A₂(g) + B₂(g) leftharpoons 2AB(g)$$A_{2}(g) + B_{2}(g) \rightleftharpoons 2AB(g)$$
The value of x (in kJ mol⁻¹$\text{kJ mol}^{-1}$) is .... (Nearest integer)
(Given: K=2.2, R=8.314 J K⁻¹ mol⁻¹$\log K=2.2, R=8.314\text{ J K}^{-1}\text{ mol}^{-1}$)
Class 11 Chemistry: Thermodynamics
Class 11 Chemistry: Equilibrium
Q56jee_main_2026_21_jan_eveningBond Enthalpy and Enthalpy of Atomization
Consider the following data:
Δf H(methane, g) = -X kJ mol⁻¹$\Delta_f H^{\ominus}(\text{methane, g}) = -X \text{ kJ mol}^{-1}$
Enthalpy of sublimation of graphite = Y kJ mol⁻¹$= Y \text{ kJ mol}^{-1}$
Dissociation enthalpy of H₂ = Z kJ mol⁻¹$\text{H}_2 = Z \text{ kJ mol}^{-1}$
The bond enthalpy of C-H$\text{C-H}$ bond is given by:
A.(1) (X + Y + 2Z)/(4)$(1) \ \frac{X + Y + 2Z}{4}$
B.(2) (X + Y + 4Z)/(2)$(2) \ \frac{X + Y + 4Z}{2}$
C.(3) X + Y + Z$(3) \ X + Y + Z$
D.(4) (-X + Y + Z)/(4)$(4) \ \frac{-X + Y + Z}{4}$
-X = (Δ Hsub of carbon) + 2 × (B.E. of H-H) - 4 × (B.E. of C-H)$-X = (\Delta H_{\text{sub}} \text{ of carbon}) + 2 \times (\text{B.E. of H-H}) - 4 \times (\text{B.E. of C-H})$
-X = Y + 2Z - 4(B.E. of C-H)$-X = Y + 2Z - 4(\text{B.E. of C-H})$
Step 1: Rearranging for Bond Enthalpy
Rearranging the equation for C-H bond enthalpy:
B.E. of C-H = (X + Y + 2Z)/(4)$$\text{B.E. of C-H} = \frac{X + Y + 2Z}{4}$$
Pattern Recognition
Sees: bond enthalpy derivation from heat of formation, sublimation, and dissociation.
Trap: Sign convention errors when substituting formation enthalpies.
Chapter Mix
Class 11 Chemistry: Chemical Thermodynamics
Q60jee_main_2026_22_january_morningWork and Internal Energy
A. Work done in reversible, isothermal expansion of 2 mol of ideal gas from 2 dm³$2\text{ dm}^{3}$ to 20 dm³$20\text{ dm}^{3}$ at 300 K.
I. 4
B. Work done in irreversible isothermal expansion of 1 mol ideal gas from 1 m³$1\text{ m}^{3}$ to 3 m³$3\text{ m}^{3}$ at 300 K against a constant pressure of 3kPa.
II. 11.5
C. Change in internal energy for adiabatic expansion of a 1 mol ideal gas with change of temperature = 320 K and Cv = (3)/(2)R$\overline{C}_{v} = \frac{3}{2}R$
III. 6
D. Change in enthalpy at constant pressure of 1 mole ideal gas with change of temperature = 337 K and Cₚ = (5)/(2)R$\overline{C}_{p} = \frac{5}{2}R$
IV. 7
Choose the correct answer from the option given below:
Practice past-year questions one chapter at a time. Pick an exam → subject → chapter and get every PYQ for that topic — pulled together from all past papers — with the chapter's key formulas alongside.
