not sure what i did wrong says incorrect i need help ### Calorimetry Experiment: Understanding Exothermic and Endothermic ReactionsA student runs two experiments with a constant-volume "bomb" calorimeter containing 1400 g of water (see sketch at right).First, a 6.500 g tablet of benzoic acid (C\(_6\)H\(_5\)CO\(_2\)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 26.454 kJ/g.) The temperature of the water is observed to rise from 13.00 °C to 38.59 °C over a time of 5.8 minutes.Next, 5.920 g of ethylene (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 13.00 °C to 58.70 °C.Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction:\[ \text{C}_2 \text{H}_4 (\text{g}) + 3 \text{O}_2 (\text{g}) \rightarrow 2 \text{CO}_2 (\text{g}) + 2 \text{H}_2 \text{O} (\text{g}) \]**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 match published values for this reaction.**Question:**Is this reaction exothermic, endothermic, or neither?**Options:**- exothermic ✔️- endothermic - 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.** \[ \text{Answer: } -132.5 \, \text{kJ} \]### Diagram ExplanationThe image contains a simple sketch of a bomb calorimeter indicating key components:- **Stirrer**: Ensures uniform temperature distribution in the water.- **Thermometer**: Measures **Combustion Reaction Analysis**---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 38.59°C over a time of 5.8 minutes.Next, 5.920 g of ethylene (C₂H₄) 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 58.70°C.Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction:\[ \text{C}_2\text{H}_4(g) + 3\text{O}_2(g) \rightarrow 2\text{CO}_2(g) + 2\text{H}_2\text{O}(g) \]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.### Questions:1. Is this reaction exothermic, endothermic, or neither? - **Options:** - exothermic [X] - endothermic [ ] - neither [ ]2. 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. - **Answer:** \[ -132.5 \, \text{kJ} \]3. Calculate the reaction enthalpy \(\Delta H_{\text{rxn}}\) per mole of C₂H₄. - **Answer:** \[ -1160.9 \, \text{kJ/mol} \]### Diagram:- A visual labeled "A 'bomb' calorimeter" shows a schematic of a bomb calorimeter, a device used to measure the heat of combustion of substances.---End of the analysis.

To determine whether the reaction has been exothermic or endothermic, the heat absorbed or released…

A student runs two experiments with a constant-volume "bomb" calorimeter containing 1400. g of water (see sketch at -ight). First, a 6.500 g tablet of benzoic acid (C6H,CO₂H) 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 38.59 °C over a time of 5.8 minutes. Next, 5.920 g of ethylene (C₂H4) 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 58.70 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: 4 exothermic stirrer endothermic thermom O C₂H₂(g) + 30₂(g) 2CO₂(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 published values for this reaction. chemical reac "bomb" A "bomb" calorimete