1. Heat Capacity of Metals
A. Calorimetry = science of measuring heat changes (uses a calorimeter)
Each substance changes temperature at a different rate = Heat Capacity
Specific Heat capacity = J/g•oC = Cs = Sh
Molar Heat capacity = J/mol•oC
Water has a high heat capacity
Very good coolant
Heat change = q = Sh x m x DT
2. Constant-Pressure Calorimeter
Experiment done under atmospheric pressure
44.0 g hot iron (100 oC) is added to 100 g of cool water (20.0 oC) in a calorimeter
T = 23.6 oC after the temperature stabilizes (equilibrium)
Key Concept: all of the heat lost from the iron goes to the water
qwater = qiron

2. Procedure
Use water bath on a hot plate to heat metal in a test tube, record Temp
Record the initial temperature and weight of your calorimeter
(calorimeter = two styrofoam cups)
Add the hot metal to the calorimeter and record the final (highest) Temp
Weigh the calorimeter + metal
Repeat two more times to get an average specific heat of the metal
Repeat the whole thing on a second metal
Recycle the cups and the metal: don’t throw them away
Deviation from the mean = |Shi – Shavg|

3. Incident: Broken Mercury Thermometer