The values of ∆H and ∆S for the reaction. ${C_{\left( {{\rm{graphite}}} \right)}} + {\rm{C}}{{\rm{O}}_2}\left( {\rm{g}} \right) \to 2{\rm{CO}}\left( {\rm{g}} \right)$ Are 170 kJ and 170 ${\rm{J}}{{\rm{K}}^{ - 1}}$ respectively. this reaction will be spontaneous at:

NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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Application +4 | -1

The values of ∆H and ∆S for the reaction.

{C_{\left( {\mathrm{graphite}} \right)}} + \mathrm{C}{\mathrm{O}_2}\left( \mathrm{g} \right) \to 2\mathrm{CO}\left( \mathrm{g} \right)

Are 170 kJ and 170

\mathrm{J}{\mathrm{K}^{ - 1}}

respectively. this reaction will be spontaneous at:

View answer and explanation

Correct option: D

1110 K

Option D (1110 K) is correct because the reaction becomes spontaneous when T > ∆H/∆S, which calculates to be 1000 K.

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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