When 500mL 0.2M H2SO4 completely reacts with sufficient LiOH dissolved in 400mL solution. The mostly water mixture increases in temperature by 3.0ºC. Calculate the heat given off when one mole H2SO4 reacts.
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.
When 500mL 0.2M H2SO4 completely reacts with sufficient LiOH dissolved in 400mL solution. The mostly water mixture increases in temperature by 3.0ºC. Calculate the heat given off when one mole H2SO4 reacts.
Volume Of LiOH solution = 400 ml
Volume Of H2SO4 solution = 500 ml
Total Volume of Solution= 400+500
= 900 ml
temperature change of water = T = 3C
Density of water = 1g/ml
Mass Of water = 900 ml * 1 g/ml
= 900 g
Heat capacity of water = 4.18J/g C
Heat given off by the reaction = q = mcT
= 900 g * 4.18 J/g C * 3C
= 11286 J
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