If a 68 gram piece of copper is heated to 100.0oC and then put into a vessel containing 250.0 mL of water at 1.5oC, what will be the final temperature of the water (in oC)? Take the heat capacity of copper to be 0.385 J/(g oC) and that of H2O(l) to be 4.184 J/(g oC). Assume the density of water is 1.00 g/mL.
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.
If a 68 gram piece of copper is heated to 100.0oC and then put into a vessel containing 250.0 mL of water at 1.5oC, what will be the final temperature of the water (in oC)? Take the heat capacity of copper to be 0.385 J/(g oC) and that of H2O(l) to be 4.184 J/(g oC). Assume the density of water is 1.00 g/mL.
This question is based on principal of calorimetry.
Heat released by Cu will equal to heat gain by water because heat flow from high temperature to low temperature
Heat = mc(T2-T1)
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