**Objective:** Using a calorimeter, you will determine the
specific heat of metals.

**Procedure:**

You must write your own procedure (10 points). You must detail what you did so your grandma could repeat this experiment in her kitchen.

Some hints….. Less water in the calorimeter is better than more water. (enough to cover the metal is all you need)

Density of water is 1g/ml (and if you don’t know why this is important, transfer to Physical Science)

Equilibrium occurs when the thermometer hits its highest point after the metal is added to the water.

Minimize heat loss by getting the metal into the cup quickly and putting a lid on it!

**Data Table: There are two data tables because you are
going to test two metals.**

**Mass of H _{2}O
_____**g

**Mass of H _{2}O
_____**g

**Calculations: YOU MUST SHOW ALL OF YOUR WORK**

1. Find q_{water}.

2. Use q_{water}
to solve for the specific heat of the metal.
(Remember that the heat (q_{water}) absorbed by the water is
equal to the heat (q_{metal}) given off by the metal.

3. Subtract the value you get for the specific heat of the metal from the actual value of specific heat for that metal and then divide by the actual specific heat of the metal to find your percentage error (of course you need to multiply that by 100 to find %).

**Determine which metal you have: (once you have found your calculation answer to #2, you can
determine which metal you have)**

Mg has a specific
heat of 1.02 J/g^{o}C

Al has a specific
heat of 0.90 J/g^{o}C

Ni has a specific
heat of 0.44 J/g^{o}C

Zn has a specific
heat of 0.39 J/g^{o}C

Sn has a specific
heat of 0.22 J/g^{o}C

Pb has a specific heat of 0.13 J/g^{o}C

Au has a specific
heat of 0.13 J/g^{o}C

Cu has a specific
heat of 0.39 J/g^{o}C

**What is due for this lab:**

1. A step-by-step procedure

2. Data table for each metal (minimum of 2 metals)

3. Calculations 1-3 for each metal

4. Predict which
metals you have based on your calculations.