Combustion of glucose takes place according to the equation ${{\rm{C}}_6}{{\rm{H}}_{12}}{{\rm{O}}_6} + {\rm{C}}{{\rm{O}}_2} \to 6{\rm{C}}{{\rm{O}}_2} + 6{{\rm{H}}_2}{\rm{O}};\Delta H = - 72\;kcal$ How much energy will be required for the production of 1.6 g of glucose (Molecular mass of glucose = 180)?

NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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Combustion of glucose takes place according to the equation

{\mathrm{C}_6}{\mathrm{H}_{12}}{\mathrm{O}_6} + \mathrm{C}{\mathrm{O}_2} \to 6\mathrm{C}{\mathrm{O}_2} + 6{\mathrm{H}_2}\mathrm{O};\Delta H = - 72\;kcal

How much energy will be required for the production of 1.6 g of glucose (Molecular mass of glucose = 180)?

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Correct option: B

0.64 kcal

Option B (0.64 kcal) 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