Solved: Measuring qrrxnUsing a Bomb CalorimeterThe

Chapter , Problem 1PE

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The combustion of exactly \(1.000 \mathrm{~g}\) of benzoic acid in a bomb calorimeter releases \(26.38 \mathrm{~kJ}\) of heat. If the combustion of \(0.550 \mathrm{~g}\) of benzoic acid causes the temperature of the calorimeter to increase from \(22.01 \mathrm{to} 24.27^{\circ} \mathrm{C}\), calculate the heat capacity of the calorimeter.

(a) \(0.660 \mathrm{~kJ} /{ }^{\circ} \mathrm{C}\)

(b)  \(6.42 \mathrm{~kJ} /{ }^{\circ} \mathrm{C}\)

(c)  \(14.5 \mathrm{~kJ} /{ }^{\circ} \mathrm{C}\)

(d)  \(21.2 \mathrm{~kJ} / \mathrm{g}-{ }^{\circ} \mathrm{C}\)

(e)  \(32.7 \mathrm{~kJ} /{ }^{\circ} \mathrm{C}\)

Equation Transcription:

   

     

   

Text Transcription:

1.000 g  

26.38 kJ      

0.550 g    

22.01 to 24.27°C

0.660 kJ/°C

6.42 kJ/°C

14.5 kJ/°C

21.2 kJ/g-°C

32.7 kJ/°C