A piece of metal weighing 60.92 g was heated to 100.0°C and then put into 100.0 mL of water (initially at 23.7°C). The metal and water were allowed to come to equilibrium, and the final temperature was 27.8°C. Assuming no heat lost to the environment, calculate the specific heat of the metal, and identify the metal using the table below.
Specific heat of metal (round to 3 decimal places) = J/g·°C
What is the metal?
(Note: choose the metal closest to your calculated specific heat value)
| Metal | Specific heat (J/g·°C) |
|---|---|
| Ag | 0.240 |
| Al | 0.900 |
| Au | 0.129 |
| Ca | 0.650 |
| Cu | 0.385 |
| Fe | 0.444 |
| Mg | 1.020 |
| Ni | 0.440 |
| Pb | 0.160 |
| Sn | 0.210 |
| Zn | 0.390 |