Exploring the bomb calorimeter

Chemistry Level 2

A \(0.8650 \text{ g}\) sample of lactic acid \((HC_{3}H_{5}O_{3})\) was burned in a bomb calorimeter. The chemical equation below describes the reaction that took place in the calorimeter.

\[HC_{3}H_{5}O_{3(s)} + 3O_{2(g)} \longrightarrow 3CO_{2(g)} + 3H_2O_{(l)} \quad \Delta H^{\circ}_{rxn} = -1338 \space kJ/mol\]

What is the temperature increase \((\)in \(^{\circ}C)\) in the calorimeter if the heat capacity of the calorimeter, including water, was determined to be \(4.182 \space kJ/^{\circ}C\)? Enter your answer to \(3\) decimal places.

Take the molar mass of hydrogen, carbon, and oxygen to be \(1.008 \text{ g}\), \(12.01 \text{ g}\), and \(16.00 \text{ g}\), respectively.


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