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A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch a right). First, a 7.500 g tablet of benzoic acid (CH₂CO₂H) 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 24.00 °C to 65.95 °C over a time of 6.6 minutes. Next, 5.060 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 24.00 °C to 77.48 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: C.H.(g) + 30. (g) 260.(g) + 2H.0(g)

A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch a right). First, a 7.500 g tablet of benzoic acid (CH₂CO₂H) 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 24.00 °C to 65.95 °C over a time of 6.6 minutes. Next, 5.060 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 24.00 °C to 77.48 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: C.H.(g) + 30. (g) 260.(g) + 2H.0(g)

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 6.110QP: A 29.1-mL sample of 1.05 M KOH is mixed with 20.9 mL of 1.07 M HBr in a coffee-cup calorimeter (see...
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A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch at right). First, a 7.500 g tablet of benzoic acid (CH-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 24.00 °C to 65.95 °C over a time of 6.6 minutes. Next, 5.060 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 24.00 °C to 77.48 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: 1 stirrer n thermometer chemical reaction "bomb" A "bomb" calorimeter. water insulation 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 exactly match published values for this reaction.
Transcribed Image Text:A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch at right). First, a 7.500 g tablet of benzoic acid (CH-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 24.00 °C to 65.95 °C over a time of 6.6 minutes. Next, 5.060 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 24.00 °C to 77.48 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: 1 stirrer n thermometer chemical reaction "bomb" A "bomb" calorimeter. water insulation 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 exactly match published values for this reaction.
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 exactly match published values for this reaction. Is this reaction exothermic, endothermic, or 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. Calculate the reaction enthalpy ΔΗ per mole of C₂H4. rxn OOO exothermic endothermic neither KJ kJ mol x10 ×
Transcribed Image Text: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 exactly match published values for this reaction. Is this reaction exothermic, endothermic, or 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. Calculate the reaction enthalpy ΔΗ per mole of C₂H4. rxn OOO exothermic endothermic neither KJ kJ mol x10 ×
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