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NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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Application +4 | -1
Given the bond energies of N ≡ N, H─H and N─H bonds as 945, 436 and 391 kJ  mol−1kJ\,\,mo{l^{ - 1}}respectively, the enthalpy of the reaction, 2N2(g)+3H2(g)→2NH3(g)2{\mathrm{N}_2}\left( \mathrm{g} \right) + 3{\mathrm{H}_2}\left( \mathrm{g} \right) \to 2\mathrm{N}{\mathrm{H}_3}\left( \mathrm{g} \right) is :
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Correct option: A
-93 kJ
Option A (-93 kJ) is correct because it correctly calculates the enthalpy of the reaction using the given bond energies and the formula ΔH=∑BEreactants−∑BEproducts\Delta H = \sum{BE_{reactants}} - \sum{BE_{products}}.

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The internal energy of one mole of a gas is: An ideal gas is allowed to expand both reversibly and irreversibly in an isolated system. If Ti{T_i} is the initial temperature and Tf{T_f} is the final temperature, which of the following statements is correct? For which of the process, ∆S is negative? The work done by a weightless piston in causing an expansion ∆V (at constant temperature), when the opposing pressure, P is variable, is given by: Assertion :- At constant pressure of the change H2O(s)→H2O(g)\mathrm{H}_2 \mathrm{O}(\mathrm{s}) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{g}) work done is negative.

Reason :- During phase transition work done is always negative. For the reaction, X2O4(l)⟶2XO2(g),ΔU=2.1 kcal,ΔS=20 cal K−1\mathrm{X}_2 \mathrm{O_4(l}) \longrightarrow 2 \mathrm{XO}_2(\mathrm{g}), \Delta U=2.1 \mathrm{~kcal}, \Delta S=20 \mathrm{~cal} \mathrm{~K}^{-1} at 300 K300 \mathrm{~K}. Hence, ΔG\Delta G is
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