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A student runs two experiments with a constant-volume "bomb" calorimeter containing 1000. g of water (see sketch at thermometer right). stirrer First, a 7.000 g tablet of benzoic acid (C,H,CO,H) is put into the "bomb" and burned completely in an excess of water oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is insulation observed to rise from 23.00 °C to 62.40 °C over a time of 5.5 minutes. Next, 4.300 g of ethylene (C,H,) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 23.00 °C to 63.99 °C. chemical reaction "bomb" 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. C,H,(g) + 30,(g) 2Co,(g) + 2 H,0 (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. O exothermic Is this reaction exothermic, endothermic, or neither? O endothermic O 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. kJ kJ Calculate the reaction enthalpy AH per mole of C,H4. rxn mol

A student runs two experiments with a constant-volume "bomb" calorimeter containing 1000. g of water (see sketch at thermometer right). stirrer First, a 7.000 g tablet of benzoic acid (C,H,CO,H) is put into the "bomb" and burned completely in an excess of water oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is insulation observed to rise from 23.00 °C to 62.40 °C over a time of 5.5 minutes. Next, 4.300 g of ethylene (C,H,) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 23.00 °C to 63.99 °C. chemical reaction "bomb" 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. C,H,(g) + 30,(g) 2Co,(g) + 2 H,0 (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. O exothermic Is this reaction exothermic, endothermic, or neither? O endothermic O 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. kJ kJ Calculate the reaction enthalpy AH per mole of C,H4. rxn mol

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.132QP
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A student runs two experiments with a constant-volume "bomb" calorimeter containing 1000. g of water (see sketch at thermometer right). stirrer First, a 7.000 g tablet of benzoic acid (C,H,CO,H) is put into the "bomb" and burned completely in an excess of water oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is insulation observed to rise from 23.00 °C to 62.40 °C over a time of 5.5 minutes. Next, 4.300 g of ethylene (C,H4) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 23.00 °C to 63.99 °C. chemical reaction "bomb" 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. C,H,(g) + 30,(g) 2C0,(g) + 2 H,0 (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. exothermic x10 Is this reaction exothermic, endothermic, or neither? 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. ||kJ kJ Calculate the reaction enthalpy AH_ per mole of C,H4. rxn mol
Transcribed Image Text:A student runs two experiments with a constant-volume "bomb" calorimeter containing 1000. g of water (see sketch at thermometer right). stirrer First, a 7.000 g tablet of benzoic acid (C,H,CO,H) is put into the "bomb" and burned completely in an excess of water oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is insulation observed to rise from 23.00 °C to 62.40 °C over a time of 5.5 minutes. Next, 4.300 g of ethylene (C,H4) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 23.00 °C to 63.99 °C. chemical reaction "bomb" 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. C,H,(g) + 30,(g) 2C0,(g) + 2 H,0 (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. exothermic x10 Is this reaction exothermic, endothermic, or neither? 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. ||kJ kJ Calculate the reaction enthalpy AH_ per mole of C,H4. rxn mol
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