A 28.602 g sample of a metal is heated to 99.9°C in a hot water bath until thermal equilibrium is reached. The sample is quickly transferred to 55.604 g of water at 22.6°C contained in a calorimeter. When thermal equilibrium is reached the temperature of the water is measured to be 27.3°C. What is the specific heat of the metal? Specific heat of water is 4.184 J/ grams•°C In part A, (metal-water ) how was the initial temperature of WATER determined? In part A, (metal-water ) how was the initial temperature of METAL determined?
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 28.602 g sample of a metal is heated to 99.9°C in a hot water bath until thermal equilibrium is reached.
The sample is quickly transferred to 55.604 g of water at 22.6°C contained in a calorimeter.
When thermal equilibrium is reached the temperature of the water is measured to be 27.3°C. What is the specific heat of the metal? Specific heat of water is 4.184 J/ grams•°C
In part A, (metal-water ) how was the initial temperature of WATER determined?
In part A, (metal-water ) how was the initial temperature of METAL determined?
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