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This is by doing Heat of combustion with a 400ml beaker with candle, tin can with 150 ml of tap water, temperature probe and labpro data lagger.
And got the following answer:
If this was not done in a calorimeter, then pretty much all of the heat was likely lost to the surroundings. Plus a single candle is not sufficient heat source for 150 g water. And what happens to energy going into the can itself? It has a specific heat capacity, too. Is the energy more likely to be transferred to the water with high capacity 4.184 j/gc or to the surrounding air?