By a hot summer day, you want to serve some refreshments to your friends. To each glass, if you pore 200.0 mL of cold tea at 20.0°C and add 10 ice cubes at – 10.0°C each weighing 10.0 g. When you measure the temperature of a glass of tea, you find that the final temperature is 0.0° How much heat did the ice cubes gain to reach that temperature. Will the entire ice melt? If not, how much ice will melt? Useful data: Density of ice tea: ~ 1.00 g/mL C (ice tea) = 4.12 J/g.°C C (ice) = 2.11 J/g.°C DH = 6.02 kJ/mol
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.
- By a hot summer day, you want to serve some refreshments to your friends. To each glass, if you pore 200.0 mL of cold tea at 20.0°C and add 10 ice cubes at – 10.0°C each weighing 10.0 g.
- When you measure the temperature of a glass of tea, you find that the final temperature is 0.0° How much heat did the ice cubes gain to reach that temperature.
- Will the entire ice melt? If not, how much ice will melt?
Useful data: Density of ice tea: ~ 1.00 g/mL
C (ice tea) = 4.12 J/g.°C
C (ice) = 2.11 J/g.°C
DH = 6.02 kJ/mol
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