A student is performing bomb calorimetry for a combustion reaction. The bomb calorimeter normally holds 5 L of water with a heat capacity of 4.184 J/g•°C. However, the student misread the directions and used 6 L of ethanol which has a heat capacity of 2.46 J/g•°C. If the student calculates the energy released by the reaction assuming it was 5 L of water, what will be the difference between the actual energy of the reaction and the calculated energy? Note: the densities of ethanol and water under normal conditions are 0.8 g/mL and 1.0 g/mL, respectively.

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06-11-2022
Physics

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A student is performing bomb calorimetry for a combustion reaction. The bomb calorimeter normally holds 5 L of water with a heat capacity of 4.184 J/g•°C. However, the student misread the directions and used 6 L of ethanol which has a heat capacity of 2.46 J/g•°C. If the student calculates the energy released by the reaction assuming it was 5 L of water, what will be the difference between the actual energy of the reaction and the calculated energy? Note: the densities of ethanol and water under normal conditions are 0.8 g/mL and 1.0 g/mL, respectively.

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