Question

7. 1.00 mol \( \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6} \) (glucose) is oxidized to carbon dioxide and water at \( 25^{\circ} \mathrm{C} \) according to the following equation; \[ \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(\mathrm{~s})+6 \mathrm{O}_{2}(\mathrm{~g}) \rightarrow 6 \mathrm{CO}_{2}(\mathrm{~g})+6 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \] Calorimetric measurements give \( \Delta_{r} U^{\circ}=-2808 \mathrm{~kJ} \mathrm{~mol}^{-1} \) and \( \Delta_{\mathrm{r}} \mathrm{S}^{\circ}=+259.1 \mathrm{JK}^{-1} \mathrm{~mol}^{-1} \) at \( 25^{\circ} \mathrm{C} \). How much of this energy can be extracted as (a) heat (at constant pressure), (b) work?

          7. 1.00 mol \( \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6} \) (glucose) is oxidized to carbon dioxide and water at \( 25^{\circ} \mathrm{C} \) according to the following equation;
\[
\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(\mathrm{~s})+6 \mathrm{O}_{2}(\mathrm{~g}) \rightarrow 6 \mathrm{CO}_{2}(\mathrm{~g})+6 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})
\]

Calorimetric measurements give \( \Delta_{r} U^{\circ}=-2808 \mathrm{~kJ} \mathrm{~mol}^{-1} \) and \( \Delta_{\mathrm{r}} \mathrm{S}^{\circ}=+259.1 \mathrm{JK}^{-1} \mathrm{~mol}^{-1} \) at \( 25^{\circ} \mathrm{C} \). How much of this energy can be extracted as (a) heat (at constant pressure), (b) work?

7. 1.00 mol C6H12O6 (glucose) is oxidized to carbon dioxide and water at 25^∘C according to the following equation;

C6H12O6( s)+6 O2( g) → 6 CO2( g)+6 H2O(l)

Calorimetric measurements give Δr U^∘=-2808 kJ mol^-1 and ΔrS^∘=+259.1 JK^-1 mol^-1 at 25^∘C. How much of this energy can be extracted as (a) heat (at constant pressure), (b) work?

Added by Gregg M.

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