An arctic explorer is trying to create drinking water by converting an ice ball into liquid. The ice ball has a mass of 225g and is at an initial temperature of -23C. The explorer heats the resulting water to a temperature of 37C. The heat of fusion of ice is 334J/g and the specific heat of ice is 2.1J/(g K). How much heat was required for the process?
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.
An arctic explorer is trying to create drinking water by converting an ice ball into liquid. The ice ball has a mass of 225g and is at an initial temperature of -23C. The explorer heats the resulting water to a temperature of 37C. The heat of fusion of ice is 334J/g and the specific heat of ice is 2.1J/(g K).
How much heat was required for the process?
Given that :
The mass of ice = 225 g
The initial temperature of ice = -23
The final temperature of ice = 37
The heat of fusion of ice = 334 J/g
The specific heat of ice = 2.1 J/g.K or 2.1 J/g.
The specific heat of water = 4.18 J/g
Trending now
This is a popular solution!
Step by step
Solved in 4 steps
