Measuring qrrxnUsing a Bomb CalorimeterThe combustion of

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Measuring \(q_{r x n} \) Using a Bomb Calorimeter

The combustion of methylhydrazine \(\left(\mathrm{CH}_{6} \mathrm{~N}_{2}\right)\), a liquid rocket fuel, produces \(\mathrm{N}_{2}(g), \mathrm{CO}_{2}(g) \text { and } \mathrm{H}_{2} \mathrm{O}(l)\)

\(2 \mathrm{CH}_{6} \mathrm{~N}_{2}(l)+50_{2}(g) \rightarrow 2 \mathrm{~N}_{2}(g)+2 \mathrm{CO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(l)\)

When \(4.00 \mathrm{~g}\)  of methylhydrazine is combusted in a bomb calorimeter, the temperature of the calorimeter increases from \(25.00 \text { to } 39.50^{\circ} \mathrm{C}\). In a separate experiment the heat capacity of the calorimeter is measured to be \(7.794 \mathrm{~kJ} / \circ \mathrm{C}\). Calculate the heat of reaction for the combustion of a mole of \(\mathrm{CH}_{6} \mathrm{~N}_{2}\)

A \(0.5865-\mathrm{g}\) sample of lactic acid \(\left(\mathrm{HC}_{3} \mathrm{H}_{5} \mathrm{O}_{3}\right)\) is burned in a calorimeter whose heat capacity is \(4.812 \mathrm{~kJ} / \circ \mathrm{C}\). The temperature increases from \(23.10 \text { to } 24.95^{\circ} \mathrm{C}\). Calculate the heat of combustion of lactic acid (a) per gram and (b) per mole.

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Text Transcription:

qrxn    

(CH6N2)  

N2(g), CO2(g) and H2O(l)

2CH6N2(l)+502(g) \rightarrow 2 N2(g)+2CO2(g)+6H2O(l)

4.00 g    

25.00 to 39.50°C  

 7.794 kJ/°C      

CH6N2    

0.5865-g  

(HC3H5O3)  

4.812 kJ/°C

23.10 to 24.95°C