Questions: A student runs two experiments with a constant-volume "bomb" calorimeter containing 1200. g of water. First, a 5.000 g tablet of benzoic acid (C6H5CO2H) 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 16.00°C to 41.05°C over a time of 14.3 minutes. Next, 4.030 g of ethane (C2H6) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 16.00°C to 54.08°C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: A "bomb" calorimeter. 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.

Transcript text: A student runs two experiments with a constant-volume "bomb" calorimeter containing 1200. g of water (see sketch at right). First, a 5.000 g tablet of benzoic acid $\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{CO}_{2} \mathrm{H}\right)$ is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of $26.454 \mathrm{~kJ} / \mathrm{g}$.) The temperature of the water is observed to rise from $16.00^{\circ} \mathrm{C}$ to $41.05^{\circ} \mathrm{C}$ over a time of 14.3 minutes. Next, 4.030 g of ethane $\left(\mathrm{C}_{2} \mathrm{H}_{6}\right)$ are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from $16.00^{\circ} \mathrm{C}$ to $54.08^{\circ} \mathrm{C}$. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: A "bomb" calorimeter. 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.