The heat of combustion of ethanol determined by a bomb calorimeter is - 670.48 kcal$mo{l^{ - 1}}$ at ${25^0}C$.What is ∆U at ${25^0}C$ for the following reaction? ${{\rm{C}}_2}{{\rm{H}}_5}{\rm{OH}}\left( l \right) + \frac{7}{2}{{\rm{O}}_2}\left( {\rm{g}} \right) \to 2{\rm{C}}{{\rm{O}}_2}\left( {\rm{g}} \right) + 3{{\rm{H}}_2}{\rm{O}}\left( {\rm{g}} \right)$

NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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The heat of combustion of ethanol determined by a bomb calorimeter is - 670.48 kcal

mo{l^{ - 1}}

{25^0}C

.What is ∆U at

{25^0}C

for the following reaction?

{\mathrm{C}_2}{\mathrm{H}_5}\mathrm{OH}\left( l \right) + \frac{7}{2}{\mathrm{O}_2}\left( \mathrm{g} \right) \to 2\mathrm{C}{\mathrm{O}_2}\left( \mathrm{g} \right) + 3{\mathrm{H}_2}\mathrm{O}\left( \mathrm{g} \right)

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Correct option: C

- 670.48\mathrm{kcal}

Option C (-670.48 kcal) is correct because at constant volume (bomb calorimeter), the heat of combustion is equal to the change in internal energy, ∆U.

NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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