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A student runs two experiments with a constant-volume "bomb" calorimeter containing 1300. g of water (see sketch at right). thermometer stirrer First, a 6.000 g tablet of benzoic acid (C,H,CO,H) is put into the "bomb" and burned completely in an water excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of insulation the water is observed to rise from 23.00 °C to 48.98 °C over a time of 8.0 minutes. Next, 5.860 g of acetylene (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 64.64 °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,(g) + 50,(g) 4 CO,(g) + 2 H,O(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 Calculate the reaction enthalpy AH. per mole of CO,. rxn mol

A student runs two experiments with a constant-volume "bomb" calorimeter containing 1300. g of water (see sketch at right). thermometer stirrer First, a 6.000 g tablet of benzoic acid (C,H,CO,H) is put into the "bomb" and burned completely in an water excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of insulation the water is observed to rise from 23.00 °C to 48.98 °C over a time of 8.0 minutes. Next, 5.860 g of acetylene (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 64.64 °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,(g) + 50,(g) 4 CO,(g) + 2 H,O(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 Calculate the reaction enthalpy AH. per mole of CO,. rxn mol

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter8: Thermochemistry
Section: Chapter Questions
Problem 16QAP: Ethyl alcohol, C2H5OH, is the intoxicating agent in liquor. Burning 1.00 g of ethyl alcohol in an...
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A student runs two experiments with a constant-volume "bomb" calorimeter containing 1300. g of water (see sketch at right). thermometer stirrer First, a 6.000 g tablet of benzoic acid (C,H,CO,H) is put into the "bomb" and burned completely in an water excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of insulation the water is observed to rise from 23.00 °C to 48.98 °C over a time of 8.0 minutes. Next, 5.860 g of acetylene (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 64.64 °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. 2 C,H,(g) + 50,(g) → 4CO,(g) + 2H,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 Calculate the reaction enthalpy AH, per mole of CO,. rxn mol O
Transcribed Image Text:A student runs two experiments with a constant-volume "bomb" calorimeter containing 1300. g of water (see sketch at right). thermometer stirrer First, a 6.000 g tablet of benzoic acid (C,H,CO,H) is put into the "bomb" and burned completely in an water excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of insulation the water is observed to rise from 23.00 °C to 48.98 °C over a time of 8.0 minutes. Next, 5.860 g of acetylene (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 64.64 °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. 2 C,H,(g) + 50,(g) → 4CO,(g) + 2H,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 Calculate the reaction enthalpy AH, per mole of CO,. rxn mol O
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