2.  Different substances require different amounts of heat to change their temperature.  Objects that require more energy have a high heat capacity like water.

3. Specific heat (C p ) the heat needed to raise the temperature of 1 gram of a substance by 1 degree Celsius. Unit = J / (g X 0 C) Instrument = calorimeter Equation = q = m x C p X ΔT q = heat in Joules m = mass in grams ΔT = change in temperature in 0 C

4. The temperature of a piece of copper with a mass of 95.4 g changes from 25 to 48 o C when the metal absorbs 849J of heat energy. What is the specific heat of copper? q= 849Jq = m x Cp x ΔT m= 95.4g 849J = 95.4g x C p x 23 o C ΔT= 23 o C (95.4g x 23 o C) (95.4g x 23 o C) C p = 0.387 J/g x o C

5. Another piece of copper with a mass of 75.0g is heated until it’s temperature increases from 2 to 150 o C. How much heat energy is released or absorbed? m= 75.0gq = m x C p x ΔT C p = 0.387 J/g x o C ΔT= 148 o C q = 75.0g x 0.387J/g x 148 o C q = 4,300J