1. Determining the Molar Heat of Combustion for Paraffin
Background: similar to specific heat capacity, Molar Heat is the amount of energy required to raise one mole of the substance 1°C. Water can be used to trap the energy released in the form of heat from the candle wax. Molar heat: J/mol°C

2. Data to collect: Volume of water _____
Initial mass of candle _________ Final mass of candle _________ Mass burned _________
Initial temperature of water _________ Final temperature of water ________ ΔT __________
Class averages:
Mass of water used _______
Mass of candle wax burned __________ Change in temperature (ΔT) ________

3. Calculations and Questions:
What mass of water was used in this lab (note: the density of water is 1 g/mL)?
Using individual and class averages, calculate the heat absorbed by the water (assume c = 4.18 J/g°C).
Assume that the heat absorbed by the water is equal to the heat given off by the candle. Calculate the amount of heat released per gram of wax (i.e. the specific heat of combustion).
Paraffin wax has the formula C25H52. Calculate the amount of heat released per mole of wax (i.e. calculate the molar heat of combustion for paraffin).
Write the thermochemical equation that represents the combustion of paraffin wax.
In question three, 4.18 J/g°C was used as the specific heat capacity of the calorimeter. Suggest a reason why this is not entirely accurate. What other sources of error are there in this lab?

5. Accepted Molar Enthalpy (Heat) of Combustion for Paraffin
KJ/g = 14,600-14,800 KJ/mol
12-15 MJ/mol = 10/10
MJ/mol = 9/10
8-9.9 MJ/mol = 9/10
Below 8 MJ/mol = 7/10