∆H for the reaction given below represents, ${\rm{C}}{{\rm{O}}_2}\left( {\rm{g}} \right) + {{\rm{H}}_2}\left( {\rm{g}} \right) \to {\rm{CO}}\left( {\rm{g}} \right) + {{\rm{H}}_2}{\rm{O}}\left( {\rm{g}} \right);\Delta {\rm{H}} = 40{\rm{kJ}}:$

NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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∆H for the reaction given below represents,

\mathrm{C}{\mathrm{O}_2}\left( \mathrm{g} \right) + {\mathrm{H}_2}\left( \mathrm{g} \right) \to \mathrm{CO}\left( \mathrm{g} \right) + {\mathrm{H}_2}\mathrm{O}\left( \mathrm{g} \right);\Delta \mathrm{H} = 40\mathrm{kJ}:

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Correct option: D

Heat of reaction

Option D (Heat of reaction) is correct because the given \u0394H represents the enthalpy change for the overall reaction as written.

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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