Two 20.0 g ice cubes at -12.0 °C are placed into 255 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tr, of the water after all the ice melts. heat capacity of H, O(s) 37.7 J/(mol-K) °C T = heat capacity of H, O(1) 75.3 J/(mol-K) enthalpy of fusion of H,O 6.01 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.
Solution
Heat energy is that the live of the full internal energy of a system. This includes the full mechanical energy of the system and also the P.E. of the molecules.
It has been seen that the interior energy of a system may be modified by either activity heat to that, or doing work on that.
The internal energy of a system is found to extend with the rise in temperature. This increase in internal energy depends on the temperature distinction, the number of matter, etc.
Heat capability is outlined because the quantity of warmth energy needed to boost the temperature of a given amount of matter by one C.
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