1. The problem statement, all variables and given/known data Finding the specific heat capacity of an unknown metal. A cylinder was placed into boiling water, originally at 24.2 C. The heat transfered from the metal, and the water then was 29.5 C. Original Temperature-24.2 C Temperature after the metal has been placed into the water.-29.5 C m=mass of water (100 g) C=Specific Heat of Water (1 C) deltaT=Change of Temperature in water=5.3 (29.5-24.2) Metal M=Mass of metal (86.79 g) deltaT=? (I think it is 5.3, equivalent to the change of temperature in the water) C=? I am not entirely sure what I am doing wrong. I thought that the heat gained by the water is equivalent to the heat lost by the metal, therefore the change 2. Relevant equations Q=mCdeltaT Q/m*deltaT=c 3. The attempt at a solution First I found the heat gained by the water by using the formula Q=mCdeltaT. Where m=mass of water (100 g) C=Specific Heat of Water (1 C) deltaT=Change of Temperature in water=5.3 (29.5-24.2) Q=100x1x5.3 Therefore Q=530 Next, I used the Q to calculate the specific heat capacity of the unknown metal. Q=mCdeltaT, with the variables changed to Q/m*deltaT=c Where Q=Heat Gained by Water/Lost by metal (530) m=Mass of metal (86.79 g) deltaT=This is what I am unsure about. Would the heat lost by the metal be equivalent to the heat gained by the water? Which would equal to 5.3 C. If I calculate using that assumption for Delta T the answer equals 1.15 c/ g cal which is quite high for the specific heat capacity of a metal. Was my process correct?