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NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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Workdone for the conversion of 0.5 mole of water at 100∘C100^{\circ} \mathrm{C} to steam at 1Β atm1 \mathrm{~atm} pressure is (heat of vaporisation of water at 100∘C100^{\circ} \mathrm{C} is 40670Β JΒ molβˆ’140670 \mathrm{~J} \mathrm{~mol}^{-1} )
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Correct option: A
βˆ’1.54Β kJ-1.54 \mathrm{~kJ}
Option A (βˆ’1.54Β kJ-1.54 \mathrm{~kJ}) is correct because it is the work done calculated using W=βˆ’PΞ”VW = -P\Delta V during the phase change from water to steam.

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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, βˆ†S is negative? The work done by a weightless piston in causing an expansion βˆ†V (at constant temperature), when the opposing pressure, P is variable, is given by: Assertion :- At constant pressure of the change H2O(s)β†’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),Ξ”U=2.1Β kcal,Ξ”S=20Β calΒ Kβˆ’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 300Β K300 \mathrm{~K}. Hence, Ξ”G\Delta G is
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