- (6)lf the heat of combustion for a mole of methane (CHA) is -2,200 kJ, how many grams of methane must be burned to heat 455 g of ice at 0°C to water at 88°C?
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 that,
Mass of ice = 455g
Initial temperature of ice =
Final temperature of water =
Heat evolved from combustion of 1 mole of methane = -2200 kJ.
Specific heat of water = 4.2 kJ/mole.
Latent heat of melting = 334 J/g
Latent heat of melting is the amount of heat required to melt one gram of ice at
There are two phases of heat involved in conversion of ice at to
- First conversion of ice at to water at .
- Second heating of water at to
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