A student runs two experiments with a constant-volume bomb calorimeter containing 1000. g of water (see...

 

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A student runs two experiments with a constant-volume "bomb" calorimeter containing 1000. g of water (see sketch at right). First, a 6.000 g tablet of benzoic acid (C6H5COH) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 13.00 C to 45.39 C over a time of 14.8 minutes. Next, 5.610 g of acetylene (C2H2) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 13.00 C to 73.20 C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: 0 thermometer stirrer chemical reaction "bomb" A "bomb" calorimeter. water insulation 2C2H2(g) + 502(g) - 4CO2(g) + 2H2O(g) Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do these experiments sufficiently carefully, and the values you calculate may not exactly match published values for this reaction. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. Calculate the reaction enthalpy AHxn per mole of CH. exothermic x10 endothermic neither Ok 0 kJ mol X 5 A student runs two experiments with a constant-volume "bomb" calorimeter containing 1000. g of water (see sketch at right). First, a 6.000 g tablet of benzoic acid (C6H5COH) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 13.00 C to 45.39 C over a time of 14.8 minutes. Next, 5.610 g of acetylene (C2H2) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 13.00 C to 73.20 C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: 0 thermometer stirrer chemical reaction "bomb" A "bomb" calorimeter. water insulation 2C2H2(g) + 502(g) - 4CO2(g) + 2H2O(g) Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do these experiments sufficiently carefully, and the values you calculate may not exactly match published values for this reaction. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. Calculate the reaction enthalpy AHxn per mole of CH. exothermic x10 endothermic neither Ok 0 kJ mol X 5