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NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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Application +4 | -1
Given SC2H6∘=225 J mol−1 K−1\mathrm{S}_{\mathrm{C}_2 \mathrm{H}_6}^{\circ}=225 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}, SC2H4∘=220 J mol−1 K−1, SH2∘=130 J mol−1 K−1.\mathrm{S}_{\mathrm{C}_2 \mathrm{H}_4}^{\circ}=220 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}, \mathrm{~S}_{\mathrm{H}_2}^{\circ}=130 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}. Then ΔS∘\Delta \mathrm{S}^{\circ} for the process C2H4+H2→C2H6\mathrm{C}_2 \mathrm{H}_4+\mathrm{H}_2 \rightarrow \mathrm{C}_2 \mathrm{H}_6 is
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Correct option: B
−125 J-125 \mathrm{~J}
Option B (-125 J) is correct because the change in entropy (ΔS∘\Delta S^{\circ}) is calculated using the formula ΔS∘=Sproducts∘−Sreactants∘\Delta S^{\circ} = S^{\circ}_{products} - S^{\circ}_{reactants}.

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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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