A student runs two experiments with a constant$-$volume "bomb" calorimeter containing $1300.g$ of water $($see sketch at right$).$

First, a $6\mathrm{.}000g$ tablet of benzoic acid $(C_6{H}_{5}C{O}_{2}H)$ is put into the "bomb" and burned completely in an excess of oxygen. $($Benzoic acid is known to have a heat of combustion of $26\mathrm{.}454k\frac{J}{g}.)$ The temperature of the water is observed to rise from $22\mathrm{.}00C$ to $48\mathrm{.}54C$ over a time of $8\mathrm{.}5$ minutes.

Next, $5\mathrm{.}450g$ of ethyler $(C_2{H}_4)$ are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from $22\mathrm{.}00C$ to $62\mathrm{.}83C.$

Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction:

$C_2{H}_4(g)+3O_2(g)2C{O}_2(g)+2H_{2}O(g)$

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.

$\backslash$table$[[,$exothermic$],[$Is this reaction exothermic, endothermic, or neither?,endothermic$],[$neither$,],[\backslash$table$[[$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.$]],kJ$