4.900g of acetylene C2H2 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 60.12°C. 2C2H2g + 5O2g -> 4CO2g + 2H2Og 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 CO2.
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1500.g of water (see sketch at right).First, a 7.000g 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 23.00°C to 50.43°C over a time of 14.7 minutes.
Next, 4.900g of acetylene C2H2 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 60.12°C.
2C2H2g + 5O2g -> 4CO2g + 2H2Og
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 CO2.
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