A student runs two experiments with a constant-volume "bomb" calorimeter containing1200.g of water First, a 6.000g tablet of benzoic acid C6H5CO2H is put into the "bomb" and burned completely in an...

A student runs two experiments with a constant-volume "bomb" calorimeter containing1200.g
of water

First, a 6.000g 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 10.00°C to 36.99°C over a time of 6.8 minutes.

Next, 5.710g 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 10.00°C to 53.57°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 CO2.	= kJ/mol

Jun 09, 2022

SOLUTION.PDF

A student runs two experiments with a constant-volume "bomb" calorimeter containing1200.g of water First, a 6.000g tablet of benzoic acid C6H5CO2H is put into the "bomb" and burned completely in an...

Get Answer To This Question

Related Questions & Answers

Submit New Assignment