Consider the given data: (a) HCl(g) + 10 H₂O(l) → HCl.10 H₂O Δ H = -69.01 kJ mol⁻¹ (b) HCl(g) + 40 H₂O(l) → HCl.40 H₂O Δ H = -72.79 kJ mol⁻¹ Choose the correct statement:

(C) The heat of solution depends on the amount of solvent.

(A) The heat of dilution for the HCl (HCl.10 H₂O to HCl.40 H₂O) is 3.78 kJ mol⁻¹.

(B) The heat of formation of HCl solution is represented by both (a) and (b).

(D) Dissolution of gas in water is an endothermic process.

Chemical Thermodynamics: JEE Main 2025 Chemistry question

JEE Main 2025 · 4 Apr, Evening shift · Q63

JEE Main 20254 Apr, Evening shiftChemistryMediumChemical Thermodynamics84× since 2002

Consider the given data : (a)

\mathrm{HCl(g) + 10\,H_2O(l) \rightarrow HCl.10\,H_2O}

\Delta H = -69.01\ \mathrm{kJ\,mol^{-1}}

(b)

\mathrm{HCl(g) + 40\,H_2O(l) \rightarrow HCl.40\,H_2O}

\Delta H = -72.79\ \mathrm{kJ\,mol^{-1}}

Choose the correct statement :

JEE Main 2025 Chemical Thermodynamics Question with Solution (4 Apr Evening shift, Q63) | JEE Arc

JEE Main 2025 · 4 Apr, Evening shift · Q63

JEE Main 20254 Apr, Evening shiftChemistryMediumChemical Thermodynamics84× since 2002

Consider the given data : (a)

\mathrm{HCl(g) + 10\,H_2O(l) \rightarrow HCl.10\,H_2O}

\Delta H = -69.01\ \mathrm{kJ\,mol^{-1}}

(b)

\mathrm{HCl(g) + 40\,H_2O(l) \rightarrow HCl.40\,H_2O}

\Delta H = -72.79\ \mathrm{kJ\,mol^{-1}}

Choose the correct statement :