# 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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