Consider the reaction { m C_{12}H_{22}O_{11}}({ m s}) + { m 12O_2}({ m g}) ightleftharpoons {

Consider the reaction

{\rm C_{12}H_{22}O_{11}}({\rm s}) + {\rm 12O_2}({\rm g}) \rightleftharpoons {\rm 12CO_2}({\rm g}) + {\rm 11H_2O}({\rm l})

in which 10.0 \rm g of sucrose, \rm C_{12}H_{22}O_{11}, was burned in a bomb calorimeter with a heat capacity of 7.50 \rm kJ/^\circ C. The temperature increase inside the calorimeter was found to be 22.0 \rm ^\circ C. Calculate the change in internal energy, Delta E, for this reaction per mole of sucrose.

Answer rating: 100% (QA)

Rise in the temperature produced inside the calorim... View the full answer