What is the Heat of Combustion for Quinone in kJ/mol?

Thread starter ben4life86
Start date Apr 12, 2005
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Combustion Heat Heat of combustion

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To calculate the heat of combustion of quinone (C6H4O2), the heat released during the combustion can be determined using the formula Q = C × ΔT, where Q is the heat absorbed by the calorimeter, C is the heat capacity, and ΔT is the temperature change. In this case, Q equals 1.56 kJ/C multiplied by the temperature increase of 3.2 C, resulting in a total heat release of 4.992 kJ. To find the heat of combustion per mole, the mass of quinone (0.196 g) is converted to moles using its molar mass (approximately 110.11 g/mol), yielding about 0.00178 moles. Finally, the heat of combustion is calculated by dividing the total heat released (4.992 kJ) by the number of moles, resulting in approximately 2805 kJ/mol.

Apr 12, 2005

ben4life86

A 0.196 g sample of quinone (C6H4O2) is burned in a bomb calorimeter that has a heat capacity of 1.56 kJ/C. What is the heat of combustion (kJ/mol) if the temperature increases by 3.2 C?

-I have no idea how to do this problem...

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Apr 12, 2005

Gokul43201

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Look at your text. It has examples of similar problems.

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