,4.580g of acetaldehyde C2H4O are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 17.00°C to 35.79°C. 2C2H4Og + 5O2g -> 4CO2g + 4H2Og Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. 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 ΔHrxn per mole of C2H4O.
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1500.g of water (see sketch at right).
First, a 5.500g tablet of benzoic acid C6H5CO2H is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454kJ/g.) The temperature of the water is observed to rise from 17.00°C to 39.05°C over a time of 8.9 minutes.
Next,4.580g of acetaldehyde C2H4O are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 17.00°C to 35.79°C.
Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits.
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 ΔHrxn per mole of C2H4O.
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