A piece of metal weighing 56.1 g was heated to 100.0°C and then put into 100.0 mL of water (initially at 26.2°C). The metal and water were allowed to come to equilibrium, and the final temperature was 28.2°C. Assuming no heat lost to the environment, calculate the specific heat of the metal, and identify the metal using the table below.
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
A piece of metal weighing 56.1 g was heated to 100.0°C and then put into 100.0 mL of water (initially at 26.2°C). The metal and water were allowed to come to equilibrium, and the final temperature was 28.2°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 |
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