AIPMT-PRELIMS Chemistry Thermodynamics Class 11 Questions

From the following bond energies: H – H bond energy: 431.37 kJ mol⁻¹ C = C bond energy: 606.10 kJ mol⁻¹ C – C bond energy: 336.49 kJ mol⁻¹ C – H bond energy: 410.50 kJ mol⁻¹ Enthalpy for the reaction, H H H H | | | | C = C + H – H ⟶ H – C – C – H | | | | H H H H will be:

Bond dissociation enthalpy of H₂, Cl₂, and HCl are 434, 242 and 431 kJ mol⁻¹ respectively. Enthalpy of formation of HCl is -

For the gas phase reaction, PCl₅(g) ⇌ PCl₃(g) + Cl₂(g) Which of the following conditions are correct ?

Given that bond energies of H—H and Cl—Cl are 430 kJ mol⁻¹ and 240 kJ mol⁻¹ respectively and ΔHf for HCl is –90 kJ mol⁻¹, bond enthalpy of HCl is

The enthalpy of combustion of H₂, cyclohexene (C₆H₁₀) and cyclohexene (C₆H₁₂) are^{-241}, -3800 and^{-3920} kJ per mol respectively. Heat of hydrogenation of cyclohexene is:

If the bond energies of H–H, Br–Br and H–Br are 433, 192 and 364 kJ mol⁻¹ respectively the ΔH° for the reaction H₂(g) + Br₂(g) → 2HBr(g) is-

Standard enthalpy and standard entropy changes for the oxidation of ammonia at 298 K are −382.64 kJ mol⁻¹ and −145.6 JK⁻¹ mol⁻¹, respectively. Standard Gibbs energy change for the same reaction at 298 K is :-

The work done during the expansion of a gas from a volume of 4 dm³ to 6 dm³ against a constant external pressure of 3 atm is :-

For the reaction : C₃H₈(g) + 5O₂(g) → 3CO₂(g) + 4H₂O(ℓ) at constant temperature, ΔH – ΔE is :

For which one of the following equations is \( \Delta H_{\text{reaction}} \) equal to \( \Delta H_f^\circ \) for the product:

Heat of combustion ΔH° for C(s), H₂(g) and CH₄(g) are –94, –68 and –213 Kcal/mol. then ΔH° for C(s) + 2H₂(g) → CH₄ (g) is :-

PbO₂ → PbO [ΔG₂₉₈ < 0] , SnO₂ → SnO [ΔG₂₉₈ > 0] Most probable oxidation state of Pb & Sn will be :

The Beans are cooked earlier in pressure cooker, because :

Zn + O₂ → ZnO ΔG° = – 616 J Zn + S₂ → ZnS ΔG° = – 293 J S₂ + 2O₂ → 2SO₂ ΔG° = – 408 J ΔG° for the following reaction is : ZnS + 3O₂ → ZnO + 2SO₂,

At 27°C latent heat of fusion of a compound is 2930 J/mol. Entropy change is :