NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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Analyzing +4 | -1

For electron gain enthalpies of the elements denoted as

\Delta_{\mathrm{eg}} \mathrm{H}

, the incorrect option is

View answer and explanation

Correct option: B

\Delta_{\mathrm{eg}} \mathrm{H}(\mathrm{Se}) < \Delta_{\mathrm{eg}} \mathrm{H}(\mathrm{S})

Option A (

\Delta_{\mathrm{eg}} \mathrm{H}(\mathrm{Cl}) < \Delta_{\mathrm{eg}} \mathrm{H}(\mathrm{F})

) is correct because the electron gain enthalpy of chlorine is more negative (higher electron affinity) than that of fluorine due to fluorine's small size and strong interelectronic repulsions.

More Questions from THERMODYNAMICS

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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

{T_i}

is the initial temperature and

{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

\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,

\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}

300 \mathrm{~K}

. Hence,

\Delta G