Name

Period

Date

Specific Heat of Metal Lab

OBJECTIVE

• Use change in enthalpy equations.

INFO

• water = 4.184 J/g^.oC
• lead (Pb) = 0.129 J/g^.oC = 1
• iron (Fe) = 0.448 J/g^.oC = 2
• copper (Cu) = 0.387 J/g^.oC = 3
• aluminum (Al) = 0.900 J/g^.oC = 4

MATERIALS

1. sample

DATA Mass to hundredths place.

1. metal type & number =
2. m_METAL = g
3. m_WATER = g (1 mL water = 1 g water)
4. T_INIT-WATER = ^oC
5. T_INIT-METAL = ^oC (temp of boiling water)
6. T_FINAL-SYSTEM = ^oC

PROCEDURE

1. Record metal type & number (a).
2. Mass out metal (b).
3. Half fill a 250-mL beaker with tap water.
4. Place metal into beaker, put beaker on hot plate, and heat.
5. Measure 100.0 mL water in a graduated cylinder, and pour into the Styrofoam cup (c).
6. Record temperature of water in cup (d).

*** Back to Desks ***

7. When water in beaker comes to a boil, record temp of boiling water (e). TAKE OUT THERMOMETER (to cool)
8. Place metal into cup, put on lid, record final (hottest) temp of metal-water system (f).
9. Enter data: specific_heat.pl

CALCULATIONS Numbered, space between, show work.

1. ∆T_METAL = <e-f> = ^oC
2. ∆T_WATER = <f-d> = ^oC
3. q_WATER = J
4. Cp_METAL = J/g^.oC
5. % discrepancy = %