How much heat (in kJ) is evolved when 2.7 g of aluminium reacts with a stoichiometric amount of ${\rm{F}}{{\rm{e}}_2}{{\rm{O}}_3}$?$2{\rm{A}}{{\rm{l}}_2} + {\rm{F}}{{\rm{e}}_2}{{\rm{O}}_3} \to 2{\rm{Fe}} + {\rm{A}}{{\rm{l}}_2}{{\rm{O}}_3};\Delta {H^o} = - 852\,{\rm{kJ}}$

NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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How much heat (in kJ) is evolved when 2.7 g of aluminium reacts with a stoichiometric amount of

\mathrm{F}{\mathrm{e}_2}{\mathrm{O}_3}

2\mathrm{A}{\mathrm{l}_2} + \mathrm{F}{\mathrm{e}_2}{\mathrm{O}_3} \to 2\mathrm{Fe} + \mathrm{A}{\mathrm{l}_2}{\mathrm{O}_3};\Delta {H^o} = - 852\,\mathrm{kJ}

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Correct option: C

- 42.6\,\mathrm{kJ}

Option C (-42.6 kJ) is correct because it is calculated based on the stoichiometry of the reaction and the given enthalpy change.

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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