their A student runs two experiments with a constant-volume "bomb" calorimeter containing 1500 g of water (see sketch at

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Their A Student Runs Two Experiments With A Constant Volume Bomb Calorimeter Containing 1500 G Of Water See Sketch At 1 (36.85 KiB) Viewed 43 times

their A student runs two experiments with a constant-volume "bomb" calorimeter containing 1500 g of water (see sketch at night) First, a 6.000 g tablet of benzoic acid (CH.CO,H) is put into the "bomb" and burned completely in an excess or 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 15.00 °C to 39.05 C over a time of 10.0 minutes. Next, 4.850 g of ethylene (CH) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 15.00 °C to 47.58 "C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: chemical reaction "bomb A "bomb" calorimeter. - CH,(s) + 30,6) - 200,(s) + 2H,0 (2) 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. O exothermic endothermic Is this reaction exothermic, endothermic, or neither? ? 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 J Calculate the reaction enthalpy AH per mole of CH: 0 mol