The molar heats of fusion and vaporization for water are 6.02 kJ/mol and 40.6 kJ/mol, respectively, and the specific heat capacity of liquid water is 4.18 J/g °C. a. What quantity of heat energy is required to melt 30.8 g of ice at 0 °C? Heat= kj b. What quantity of heat is required to vaporize 37.1 g of liquid water at 100. °C? Heat= kj c. What quantity of heat is required to warm 42.6 g of liquid water from 0 °C to 100. °C? Heat = kj
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.
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The molar heats of fusion and vaporization for water are 6.02 kJ/mol and 40.6 kJ/mol, respectively, and the specific heat capacity of
liquid water is 4.18 J/g °C.
a. What quantity of heat energy is required to melt 30.8 g of ice at 0 °C?
Heat
kJ
b. What quantity of heat is required to vaporize 37.1 g of liquid water at 100. °C?
Heat =
kj
c. What quantity of heat is required to warm 42.6 g of liquid water from 0 °C to 100. °C?
Heat =
kJ
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