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A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch at right). thermometer First, a 6.500 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 19.00 °C to 53.74 °C over a time of 13.8 minutes. Next, 4.460 g of ethane (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 19.00 °C to 64.80 °C. chemical reaction "boab 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. 2C,H,) + 70,) 4CO,) + 6H,0 (2) 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.

A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch at right). thermometer First, a 6.500 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 19.00 °C to 53.74 °C over a time of 13.8 minutes. Next, 4.460 g of ethane (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 19.00 °C to 64.80 °C. chemical reaction "boab 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. 2C,H,) + 70,) 4CO,) + 6H,0 (2) 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.

Chemistry
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 1100.g of water (see sketch at right). First, a 6.500 g tablet of benzoic acid (C H,CO,H) is put into the "bomb" and burned completely in an excess of 圖 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 19.00 °C to 53.74 °C over a time of 13.8 minutes. Next, 4.460 g of ethane (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 19.00 °C to 64.80 °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. 2C,H,e) + 70,g) 4CO,(g) + 6H,0 () 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 6.500 g tablet of benzoic acid (C H,CO,H) is put into the "bomb" and burned completely in an excess of 圖 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 19.00 °C to 53.74 °C over a time of 13.8 minutes. Next, 4.460 g of ethane (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 19.00 °C to 64.80 °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. 2C,H,e) + 70,g) 4CO,(g) + 6H,0 () 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.
2C,H,() + 70,(g) → 4CO,(g) + 6 H,O (2) 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 Calculate the reaction enthalpy AH per mole of C,H. mol
Transcribed Image Text:2C,H,() + 70,(g) → 4CO,(g) + 6 H,O (2) 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 Calculate the reaction enthalpy AH per mole of C,H. mol
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