We have a calorimetric bomb with a heat capacity of 555 J/K. The bomb is filled with 1000.0 mL of water. We burn 2.104 g of a solid in the calorimetric bomb. The temperature of the bomb and the water increases by 2.13 oC. The molar mass of this solid is 510.8 g/mol. How much heat would be released (in kJ, and note that we want the amount of heat going out) if we burned 0.136 mol of this solid in the calorimeter bomb? The specific heat of water is 4.184 J/K/g. Assume that the density of water is 1.00 g/mL.
We have a calorimetric bomb with a heat capacity of 555 J/K. The bomb is filled with 1000.0 mL of water. We burn 2.104 g of a solid in the calorimetric bomb. The temperature of the bomb and the water increases by 2.13 oC. The molar mass of this solid is 510.8 g/mol. How much heat would be released (in kJ, and note that we want the amount of heat going out) if we burned 0.136 mol of this solid in the calorimeter bomb? The specific heat of water is 4.184 J/K/g. Assume that the density of water is 1.00 g/mL.
Chemistry by OpenStax (2015-05-04)
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Chapter5: Thermochemistry
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Problem 31E: When a 0.740-g sample of trinitrotoluene (TNT), C7H5N2O6, is burned in a bomb calorimeter, the...
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We have a calorimetric bomb with a heat capacity of 555 J/K. The bomb is filled with 1000.0 mL of water. We burn 2.104 g of a solid in the calorimetric bomb. The temperature of the bomb and the water increases by 2.13 oC. The molar mass of this solid is 510.8 g/mol. How much heat would be released (in kJ, and note that we want the amount of heat going out) if we burned 0.136 mol of this solid in the calorimeter bomb? The specific heat of water is 4.184 J/K/g. Assume that the density of water is 1.00 g/mL.
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