An ice cube with a mass of 45.4 g at 0.0 °C is added to a glass containing 374 g of water at 45.0 °C. Determine the final temperature of the system at equilibrium. The specific heat capacity of water, C,, is 4.184 J/g-°C, and the standard enthalpy of fusion, AH; , of water is 6.01 x 10 J/mol. Assume that no energy is transferred to or from the surroundings. fus T = TOOLS
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.
Given : Mass of ice = 45.4 g
Initial temperature of ice = melting point temperature = 0.0 oC
Mass of water = 374 g
Initial temperature of water = 45.0 oC
Assuming the final temperature at equilibrium is T (which is more than melting point temperature).
Hence all the ice will melt and will reach to the final temperature.
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