A) A 110.0-g sample of a gray-colored, unknown, pure metal was heated to 92.0 oC and put into a coffee-cup calorimeter containing 75.0 g of water at 21.0 oC. When the heated metal was put into the water, the temperature of the water rose to a final temperature of 24.2 oC. The specific heat of water is 4.184 J/goC. B) A sample of water at 21.5 °C required an input of 2.53 × 104 J of heat to reach its boiling point, 100.0 °C. What was the mass of the water?
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) A 110.0-g sample of a gray-colored, unknown, pure metal was heated to 92.0 oC and put into a coffee-cup calorimeter containing 75.0 g of water at 21.0 oC. When the heated metal was put into the water, the temperature of the water rose to a final temperature of 24.2 oC. The specific heat of water is 4.184 J/goC.
B) A sample of water at 21.5 °C required an input of 2.53 × 104 J of heat to reach its boiling point, 100.0 °C. What was the mass of the water?
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