A sample of benzene (C6H6), weighing 7.05 g underwent combustion in a bomb calorimeter by the following reaction: 2 C6H6 (l) + 15 O2 (g) → 12 CO2 (g) + 6 H2O (l) If the heat capacity of the calorimeter and contents was 10.5 kJ / oC and the temperature of the calorimeter rose from 25.00 to 53.13, (1) what is the ΔH of the reaction? Using the definitions at the beginning of the module describe (2) the calorimeter + contents, (3) the type of process.

(1) ΔH of the reaction:

(2) Calorimeter + content: the hardware + water

(3) Type of process: exothermic.

Explanation:

(1) what is the ΔH of the reaction?

The enthalpy of the reaction will be equal to the heat absorbed by the calorimeter.

The heat absorbed by the calorimeter will be the product of the heat capacity of the calorimeter by the increase of temperature:

Taht is the total ΔH of the reactions but generally they are reported on a molar basis.

That means that you must divide by the number of moles of the sample.

The molar mass of benzen is 78.11g/mol

Then:

Rounding to 3 significant figures:

(2)  Describe the calorimeter + contents:

The calorimeter is a bomb calorimeter, which consists of an insulated container, made with resistant materials, with water within it. The materials must be resistant because inside will be performed vigorous reactions, which produce large amount of energy; normally combustion reactions.

When the reaction occurs the water and the calorimeter will absorb the heat of the reaction and both will increase their temperature.

That is why the bomb calorimeters are calibrated to determine the heat capacity of the calorimeter and the content.

The calorimeter must be equipped whith a small device to ignite the reaction, which is part of the hardware.

(3) the type of process.

The process is exothermic because the reaction, like any combusion reaction, is releasing energy, which is what makes that the temperature of the calorimeter and its content increase.

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