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.

The difference between the actual heat energy of the reaction and the calculated heat energy is 9092ΔT.What is the heat energy released if 6 L of are used for a combustion reaction?The heat energy released if 6 L is used for a combustion reaction is calculated as follows:Heat change = mcΔTwhere;m is massc is the specific heat capacity ΔT is temperature changewhen 6.0 L of ethanol was used;Mass of ethanol = volume * densityThe volume of ethanol = 6.0 L or 6000 mLMass of ethanol = 6000 * 0.8Mass of ethanol = 4800 gHeat change = 4800 * 2.46 * ΔTHeat change = 11808ΔTIf 5.0 L of water was used:Mass of ethanol = volume * densityThe volume of ethanol = 5.0 L or 6000 mLMass of water = 5000 * 1.0Mass of ethanol = 5000 gHeat change = 5000 * 4.18 * ΔTHeat change = 20900ΔTHeat difference = 20900ΔT - 11808ΔTHeat difference = 9092ΔTLearn more about heat change at: https://brainly.com/question/8828503#SPJ1