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Help ? Steps on how to solve the problem are appreciated.
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answerhappygod
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Help ? Steps on how to solve the problem are appreciated.
Help ? Steps on how to solve the problem are appreciated.
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1400. g of water (see sketch at right). First, a 8.000 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 57.15 °C over a time of 10.7 minutes. Next, 4.630 g of acetaldehyde (C₂H₂O) 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 40.13 °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 C₂H₂O. O exothermic O endothermic O neither KJ stirrer kJ mol 2C₂H₂O(g) + 50₂(g) → 4CO₂ (g) + 4H₂O(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. chemical reaction 0 thermometer "bomb" A "bomb" calorimeter. O x10 water insulation
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1400. g of water (see sketch at right). First, a 8.000 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 57.15 °C over a time of 10.7 minutes. Next, 4.630 g of acetaldehyde (C₂H₂O) 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 40.13 °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 C₂H₂O. O exothermic O endothermic O neither KJ stirrer kJ mol 2C₂H₂O(g) + 50₂(g) → 4CO₂ (g) + 4H₂O(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. chemical reaction 0 thermometer "bomb" A "bomb" calorimeter. O x10 water insulation