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NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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Theenthalpy change for the transition of liquid water to steam is ΔHvap=37.3kJmol(−1)\Delta {H_v}ap = 37.3kJmo{l^{( - 1)}}at 373 K. The entropy change for the process is
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Correct option: B
100Jmol−1K−1100\mathrm{J mo}{\mathrm{l}^{ - 1}}{\mathrm{K}^{ - 1}}
Option B (100Jmol−1K−1100\mathrm{J mo}{\mathrm{l}^{ - 1}}{\mathrm{K}^{ - 1}}) is correct because the entropy change is calculated using ∆S = ∆H/T for a phase transition at constant temperature.

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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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