- #1
Jacob Dale
Assuming all gases in the combustion reaction of benzoic acid (C6H5COOH) behave ideally, what is the "exact" change in internal energy?
The context in which this question is being asked is after a calorimetry experiment. For all the intents and purposes of calorimetry, the change in internal energy (ΔU) can be related to the change in enthalpy (ΔH) at a 1:1 ratio because the volume of the calorimeter remains constant.
dU = dq + dw simplifies to dU = dq
However, this question asks for the "exact" ΔU. Therefore, a correction factor needs to be introduced to account for the variable thermodynamic values.
The only variables at play here are temperature and pressure. The temperature changed around 2 degrees Celsius for each trial of the combustion of benzoic acid so it's contribution to U is negligible. Pressure, however, changes drastically. Pressure can be assumed to be function of moles of gas:
2 C6H5COOH + 15 O2 => 6 H2O + 14 CO2
There is 3:4 ratio for moles of gas. So the pressure of the system increases by a factor of 4/3.
But now I am stuck. I don't know how to calculate the "exact" ΔU. Does anyone know what my lab instructor is asking for in this situation?
Thank you for your help!
The context in which this question is being asked is after a calorimetry experiment. For all the intents and purposes of calorimetry, the change in internal energy (ΔU) can be related to the change in enthalpy (ΔH) at a 1:1 ratio because the volume of the calorimeter remains constant.
dU = dq + dw simplifies to dU = dq
However, this question asks for the "exact" ΔU. Therefore, a correction factor needs to be introduced to account for the variable thermodynamic values.
The only variables at play here are temperature and pressure. The temperature changed around 2 degrees Celsius for each trial of the combustion of benzoic acid so it's contribution to U is negligible. Pressure, however, changes drastically. Pressure can be assumed to be function of moles of gas:
2 C6H5COOH + 15 O2 => 6 H2O + 14 CO2
There is 3:4 ratio for moles of gas. So the pressure of the system increases by a factor of 4/3.
But now I am stuck. I don't know how to calculate the "exact" ΔU. Does anyone know what my lab instructor is asking for in this situation?
Thank you for your help!