When enthalpy and entropy change for a chemical reaction are $ - 2.5{\rm{ \times }}{10^3}$ cal and 7.4 cal ${\deg ^{ - 1}}$ respectively predict the reaction at 298 K is

NEET UG CHEMISTRY MCQ: THERMODYNAMICS

1 Easy

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Application +4 | -1

When enthalpy and entropy change for a chemical reaction are

- 2.5\mathrm{ \times }{10^3}

cal and 7.4 cal

{\deg ^{ - 1}}

respectively predict the reaction at 298 K is

View answer and explanation

Correct option: A

Spontaneous

Option A (Spontaneous) is correct because the Gibbs free energy change (

\Delta G

) is negative, indicating a spontaneous reaction.

\Delta G = \Delta H - T\Delta S

, and with the given values,

\Delta G

is negative.

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{T_i}

{T_f}

\mathrm{H}_2 \mathrm{O}(\mathrm{s}) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{g})

\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}

\Delta G