You have the six pieces of metal listed below, plus a beaker of water containing 300 g of water. The water temperature is 21.0 °C and its specific heat is 4.184 J/g⋅°C. Metal Specific heat (J/g⋅°C) Mass (g) 1. Al 0.9002 100.0 2. Al 0.9002 50.0 3. Au 0.1289 100.0 4. Au 0.1289 50.0 5. Zn 0.3860 100.0 6. Zn 0.3860 50.0 In an experiment, you are asked to select one piece of metal and heat it to 100.0 °C, and then select a second piece of metal and cool it to ‒10.0 °C. Both pieces of metal are then placed in the beaker of water and the temperatures of the metals and water eventually reach thermal equilibrium. You want to select two pieces of metal to use such that the final temperature of the water is as low as possible. What piece of metal will you heat and what piece of metal will you cool ? heat metal 1, cool metal 4 heat metal 2, cool metal 3 heat metal 4, cool metal 3 heat metal 1, cool metal 2 heat metal 4, cool metal 1 heat metal 6, cool metal 5
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.
You have the six pieces of metal listed below, plus a beaker of water containing 300 g of water. The water temperature is 21.0 °C and its specific heat is 4.184 J/g⋅°C.
Metal Specific heat (J/g⋅°C) Mass (g)
1. Al 0.9002 100.0
2. Al 0.9002 50.0
3. Au 0.1289 100.0
4. Au 0.1289 50.0
5. Zn 0.3860 100.0
6. Zn 0.3860 50.0
In an experiment, you are asked to select one piece of metal and heat it to 100.0 °C, and then select a second piece of metal and cool it to ‒10.0 °C. Both pieces of metal are then placed in the beaker of water and the temperatures of the metals and water eventually reach thermal equilibrium. You want to select two pieces of metal to use such that the final temperature of the water is as low as possible. What piece of metal will you heat and what piece of metal will you cool ?
heat metal 1, cool metal 4
heat metal 2, cool metal 3
heat metal 4, cool metal 3
heat metal 1, cool metal 2
heat metal 4, cool metal 1
heat metal 6, cool metal 5
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