?A 2.200-g sample of quinone \(\left(\mathrm{C}_{6} \mathrm{H}_{4}
Chapter 5, Problem 5.57(choose chapter or problem)
A 2.200-g sample of quinone \(\left(\mathrm{C}_{6} \mathrm{H}_{4} \mathrm{O}_{2}\right)\) is burned in a bomb calorimeter whose total heat capacity is \(7.854 \mathrm{~kJ} /{ }^{\circ} \mathrm{C}\). The temperature of the calorimeter increases from 23.44 to \(30.57^{\circ} \mathrm{C}\). What is the heat of combustion per gram of quinone? Per mole of quinone?
Text Transcription:
(C6H4O2)
7.854 kJ/^{\circ} C
30.57^{\circ} C
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