1. The problem statement, all variables and given/known data If 4.0 g of boiling water at 100.0°C was splashed onto a burn victim’s skin, and if it cooled to 45.0°C on the 37.0°C skin, (a) how much heat is given up by the water? (b) How much tissue mass, originally at 37.0°C, was involved in cooling the water? 2. Relevant equations Q=mcΔT 3. The attempt at a solution For part a) ΔT = 100.0°C - 45.0° = 55.0°C c for human tissue is 3.5kJ\kgK m = 4.0g = 0.004kg Q=(0.004kg)(3.5kJ\kgK)(55.0°C) Q=0.77kJ Is this correct, or am I supposed to convert my temperatures to Kelvin? The 3.5kJ\kg*K throws me off a bit. For part b) I used the same equation, but plugged in my answer from part a, and 37°C 0.77kJ=m(3.5kJ\kgK)(37.0°C) m=0.77kJ/(3.5kJ\kgK)(37.0°C) m=0.005945946kg m=5.95g Have I done everything correctly here? I am reasonably sure that my answer for part a is correct, but part b I am not.