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Chemistry / Chemistry 11 / Chapter 6 / Problem 108P

Chemistry | 11th Edition | ISBN: 9780073402680 | Authors: Raymond Chang

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Solved: The enthalpy of combustion of benzoic acid

Chapter 6, Problem 108P

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QUESTION:

The enthalpy of combustion of benzoic acid \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\right)\) is commonly used as the standard for calibrating constant-volume bomb calorimeters; its value has been accurately determined to be -3226.7 kJ/mol. When 1.9862 g of benzoic acid are burned in a calorimeter, the temperature rises from \(21.84^{\circ} \mathrm{C}\) to \(25.67^{\circ} \mathrm{C}\). What is the heat capacity of the bomb? (Assume that the quantity of water surrounding the bomb is exactly 2000 g.)

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QUESTION:

The enthalpy of combustion of benzoic acid \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\right)\) is commonly used as the standard for calibrating constant-volume bomb calorimeters; its value has been accurately determined to be -3226.7 kJ/mol. When 1.9862 g of benzoic acid are burned in a calorimeter, the temperature rises from \(21.84^{\circ} \mathrm{C}\) to \(25.67^{\circ} \mathrm{C}\). What is the heat capacity of the bomb? (Assume that the quantity of water surrounding the bomb is exactly 2000 g.)

ANSWER:

Step 1 of 4

Here we have to calculate the heat capacity of the bomb.

Given:

The enthalpy of combustion of benzoic acid () = -3226.7 KJ/mol

Mass of benzoic acid = 1.9862 g

Initial temperature = 21.84 °C

Final temperature = 25.67 °C

Mass of water surrounding the bomb = 2000 g

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