CHM-120 Lab 9 Rev4-17 (1 - mx4 . 184 x /0 10/12 CHM 1= 409 .75 x 4.184 X10 CALCULATIONS; Rest Specific Heat of Metals: 1 Determine the mass of the water used, assuming that the density of water is 1.0g/mL let 2 Determine the LIT of the water (Tfinal -Tinitial) 3 Using the specific heat of water (4.184J/g.C), determine the energy absorbed by the water. 4 Determine the LIT of the METAL (Tfinal -Tinilial). 5 The metal gave off energy to the water, which heated the water and cooled the metal. The amount of energy given off can be assumed to be the same as the amount absorbed by the water (which you just calculated in step 3 above!). Using the mass and temperature for the metal, calculate the specific heat of the metal: q S = (m)( DT) Heat of Fusion of Water: 1 Determine the mass of the water used in the beaker 2 Determine the LiT of the water (Tfinal - Tinitial) 3 Using the specific heat of water (4. 184J/g'C), determine the energy transferred to the ice by the water. 4 Divide the amount of energy transferred by the mass of the melted ice to calculate the heat of fusion in Joules per gram. 5 Convert the result from part 4 into Joules per mole by multiplying by the molecular weight o water (18g/mol) so that grams cancel