A 124 gram ice cube at -33°C is placed into a 2.50 kg iron container (assume no energy is transfered as heat to or from the surroundings). The temperature of the iron container drops by 55°C. Calculate the final temperature in °C of the water in the container. The density of water is 1.00g/mL and the heat capacity of ice to be 37.7 J mol-1K-1 and the heat capacity of water is 75.3 J mol-1K-1. The molar enthalpy of fusion of water is 6.01 kJ/mol and the heat capacity of iron is 0.45 J/(gK).
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 124 gram ice cube at -33°C is placed into a 2.50 kg iron container (assume no energy is transfered as heat to or from the surroundings). The temperature of the iron container drops by 55°C. Calculate the final temperature in °C of the water in the container. The density of water is 1.00g/mL and the heat capacity of ice to be 37.7 J mol-1K-1 and the heat capacity of water is 75.3 J mol-1K-1. The molar enthalpy of fusion of water is 6.01 kJ/mol and the heat capacity of iron is 0.45 J/(gK).
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