A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch atright).First, a 7.500 g tablet of benzoic acid (CH-CO₂H) is put into the "bomb" and burned completely in an excess ofoxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water isobserved 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 questionsbelow about this reaction:1stirrernthermometerchemical reaction"bomb"A "bomb" calorimeter.waterinsulationC₂H₂(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 matchpublished 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 matchpublished 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 wasreleased or absorbed by the reaction in the second experiment.Calculate the reaction enthalpy ΔΗ per mole of C₂H4.rxnOOOexothermicendothermicneitherKJkJmolx10×

Given Data:Mass of water = 1100 gMass of benzoic acid = 7.500 gTemperature change for the addition…

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)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A student runs two experiments with a constant-volume "bomb" calorimeter containing 1300. g of water (see sketch at right). First, a 5.000 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 22.00 °C to 42.76 °C over a time of 9.6 minutes. Next, 5.990 g of ethane (C₂H) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 22.00 °C to 71.14 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about 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 C₂H6.…
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