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 14.00°C to 47.07°C over a time of 6.4 minutes. Next, 4.560g 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 14.00°C to 62.00°C. Use this information, to answer the questions below about this reaction:

Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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A student runs two experiments with a constant-volume "bomb" calorimeter containing 1000.g of water

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 14.00°C to 47.07°C over a time of 6.4 minutes.

Next, 4.560g 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 14.00°C to 62.00°C.

Use this information, to answer the questions below about this reaction:

 
A "bomb" calorimeter.
2C2H2(g) + 5O2(g) → 4CO2(g)  2H2O(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.

 

Is this reaction exothermic, endothermic, or neither?
 
exothermic
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 ΔHrxn per mole of C2H2.
= kJ/mol
 
 
 
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