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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: sabah on October 20, 2008, 10:38:10 AM

Title: Calorimetry
Post by: sabah on October 20, 2008, 10:38:10 AM

Consider the reaction

C12H22O11(s) + 12O2(g) ---> 12CO2(g) + 11H2O(l)

in which 10.0 g of sucrose,C12H22O11 , was burned in a bomb calorimeter with a heat capacity of 7.50 kj/C. The temperature increase inside the calorimeter was found to be 22.0 C. Calculate the change in internal energy, Delta E, for this reaction per mole of sucrose.

Express your answer numerically in kilojoules per mole.

THIS IS MY ANSWER: WHICH IS WRONG

heat generated = 22.0 C * 7.50 kJ/C = 16.5 kJ

kJ/mole sucrose = heat generated * (10.0 g sucrose / MW sucrose g/mole) = 0.48

Title: Re: Calorimetry
Post by: Astrokel on October 20, 2008, 11:21:28 AM

Quote

kJ/mole sucrose = heat generated * (10.0 g sucrose / MW sucrose g/mole) = 0.48

Check your units!