I have figured out most i needed from my earlier entropy questions but now i'm faced with a different problem... dS=δQ/T that's the formula for the equation. I just did 60 grams of water at 273 K and a room at 298 K so the system is 273 K and the surroundings are 298K Using the forumula for thermal energy (m*Cp*ΔT) i found that the thermal energy is .6285 (what are the units I measure this in?) by doing .06 kg*4.19 J/g degrees C(Cp of water)*25 K(change in temperature i.e. 298-273) then i just plugged it in so dS=.6285/273, so dS = .0023021 J/K (or is it J/ Kg K?) and the same for the surrounding but in the negative. dS = -.6825/298, so dS = -.0022902 J/K? so although this shows that entropy overall increased because of the ratio of increase from the system to decrease from the surroundings, I'm concerned because this isn't as infinitesimaly small of a change that it should be I suppose. So I'm wondering where I went wrong, units, conversions, whatever. like the specific heat capacity in J/g degrees C. Should this have been converted to J/kg K? If so, how? Please do correct me. Thanks a ton!