I know the final and initial temperatures of .259kg of aluminum. Specific heat of almuninum is 900 J/(kg*K). The aluminum is cooled from 373K to 333.45K. I need to find the entropy change. This is what I did: let c = specific heat, m = mass, T = final temperature Q = cm(T - 373) <=> Q = Tcm - 373cm <=> T = Q/cm + 373 Now that I had T in terms of Q, I subsituted it into the entropy integral: delta S = [integral from initial heat to final heat] (Q/cm + 373) dQ Initial heat lost is cm(373K-373K) = 0, final amount of heat lost is cm(333.45K-373K) = -9219 J My integration yielded -3.256 x 10^6 J/K. The right answer should be only around -20 j/k or so. I am WAY off, but my approach seems like it should work. What did I do wrong?