Two 66-g ice cubes at 0 °C are dropped into 5.00 x 102 mL of tea to make iced tea. The tea was initially at 20.0 °C; when thermal equilibrium was reached, the final temperature was 0 °C. How much of the ice melted, and how much remained floating in the beverage? Assume the specific heat capacity of tea is the same as that of pure water. Assume the density of the tea is 1.00 g/mL and specific heat capacity is 4.184 J/g · K. The enthalpy of fusion of ice at 0 °C is 333 J/g. Mass of ice melted = g Mass of ice remained = g
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.
Two 66-g ice cubes at 0 °C are dropped into 5.00 x 102 mL of tea to make iced tea. The tea was initially at 20.0 °C; when thermal equilibrium was reached, the final temperature was 0 °C. How much of the ice melted, and how much remained floating in the beverage? Assume the specific heat capacity of tea is the same as that of pure water. Assume the density of the tea is 1.00 g/mL and specific heat capacity is 4.184 J/g · K. The enthalpy of fusion of ice at 0 °C is 333 J/g.
Mass of ice melted = g
Mass of ice remained = g
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