why would the Expected Values of Heat of Combustion of Alcohols be different from what I got in my lab calculations?

the lab is to compare a series of linear alcohols. 120 grams of water was placed in s calorimeter. the alcohols included methanol, ethanol, propanol, butanol, and pentanol. I solved dir the molar heat if combustion using the mass of the alcohol weighed before and after the combustion.

My numbers are way different from the expected value of heat of combustion for each alcohol. im confused why this is? Was it something i did wrong or is it supposed to be like that? my numbers still follow the correct trend. i have included my calculations for methanol so you can see.

Molar heat of combustion of methanol: Known: Molar mass of methanol = 32.04 g/mol Mass of methanol=0.65 g Mass of water-120 cm^3 = 120 g Temperature Increase= 8.5C Specific heat of water: cp=4.185 J/gC Solve: Amount of ethanol used: 0.65g/32.04g/mol=0.020287 mol Energy generated: 4.184J/g Cx 120g x 8.5 C =4267.68 J= 4.26768 kJ Molar heat of combustion: I 4.26768 kJ /0.020287 mol = 210.365 kJ/mol