A student runs two experiments with a constant-volume "bomb" calorimeter containing 1200. g of water (see sketch at 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 18.00 °C to 51.74 °C over a time of 14.9 minutes. Next, 4.510 g of ethane (C₂H6) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 18.00 °C to 53.35 °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 AHxn per mole of C₂H6. exothermic O endothermic O neither 0 2C₂H₂(g) + 70₂(g) → 4CO₂(g) + 6H₂O(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. kJ kJ I stirrer mol thermometer chemical reaction. "bomb" A "bomb" calorimeter. water X insulation
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1200. g of water (see sketch at 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 18.00 °C to 51.74 °C over a time of 14.9 minutes. Next, 4.510 g of ethane (C₂H6) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 18.00 °C to 53.35 °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 AHxn per mole of C₂H6. exothermic O endothermic O neither 0 2C₂H₂(g) + 70₂(g) → 4CO₂(g) + 6H₂O(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. kJ kJ I stirrer mol thermometer chemical reaction. "bomb" A "bomb" calorimeter. water X insulation
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter5: Thermochemistry
Section: Chapter Questions
Problem 5.104QE
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