1. The problem statement, all variables and given/known data Okay, so I am having difficulties with understanding the concepts around entropy, take this question: What is the total entropy change for 7 kg of ice melting from -5 C° to 5 C° in room at 5 C°. 2. Relevant equations dS=dQ/T Q =mΔH m*c*ln(tfinal/tinitial) c_ice=2 c_water=4 c_air=1 3. The attempt at a solution Okay, so this is my reasoning so far: as the ice heats up to zero centigrades, the total change in entropy is given by integrating dS=dQ/T wrt T, and we end up at : m*c*ln(tfinal/tinitial), so 7*2*ln(273.15/(273.15-5)) j/k. As the ice changes its state to water, the change in entropy is given directly by dS=dQ/T, where dQ is =mdH=7*330=2310 j/k. When the water heats up from 0 centigrades to 5 centigrades its change in entropy is again given by, 7*4*ln(273.15+5/(273.15)) j/k, and adding these we get the total entropy change for the melting ice. Now to the part that I am having big difficulties understanding: the change in entropy of the room. I've read that it is given by m*c_air*((tfinal-tinitial)/tfinal), so in this case this would be negative 7*1*((273.15+5°-(273.15-5°))/(273.15+5°)) j/k. So adding all these would give me the answer? 7*2*ln(273.15/(273.15-5)) j/k + 2310 j/k + 7*4*ln(273.15+5/(273.15)) j/k - 7*1*((273.15+5°-(273.15-5°))/(273.15+5°)) j/k. Am i even close to getting this question right?