Suppose 1.319 grams of an organic compound of formula, C3H7O2, is combusted in a bomb calorimeter
with a heat capacity of 12.4 kJ/ 0C. Temperature of the calorimeter before the combustion was 17.91 0C
and that after the combustion the maximum temperature recorded was 20.13 0C.
a. Determine the enthalpy of combustion for this reaction.
b. Determine the enthalpy of formation for the organic compound of formula, C3H7O2
(ΔH0
f CO2 = -393 kJ/mol; ΔH0
f H2O = -285 kJ/mol; ΔH0
f O2 = 0 kJ/mol)

Question

Suppose 1.319 grams of an organic compound of formula, C3H7O2, is combusted in a bomb calorimeter
with a heat capacity of 12.4 kJ/ 0C. Temperature of the calorimeter before the combustion was 17.91 0C
and that after the combustion the maximum temperature recorded was 20.13 0C.
a. Determine the enthalpy of combustion for this reaction.
b. Determine the enthalpy of formation for the organic compound of formula, C3H7O2
(ΔH0
f CO2 = -393 kJ/mol; ΔH0
f H2O = -285 kJ/mol; ΔH0
f O2 = 0 kJ/mol)

anonymous · Answer

Ok so Enthalpy equals q/moles, So figure out delta T and multiply it by the heat capacity. Then divide it by the moles of sample. This will give you delta H of combustion.

anonymous · Answer

the figure out the formation chemical equation and set it equal to the enthalpy of combustion and solve for the unknown value.