50.0 mL of 1.50 M CaCl2 solution and 80.0 mL of 2.00 M NaOH solution both initially at 22.3℃ are mixed in a coffee-cup calorimeter with a calorimeter constant of 12.8 J/℃,
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.
Calcium chloride and sodium hydroxide react according to the equation:
CaCl2 (aq) + 2 NaOH (aq) → Ca(OH)2 (s) + 2 NaCl (aq)
When 50.0 mL of 1.50 M CaCl2 solution and 80.0 mL of 2.00 M NaOH solution both initially at 22.3℃ are mixed in a coffee-cup calorimeter with a calorimeter constant of 12.8 J/℃, the temperature fell to 20.0℃. If the density of the reaction mixtrure is 1.03 g/mL and its specific heat 3.94 J/g℃, calculate the heat absorbed by the reaction.
(the answer is 1.24 x 103 J, but I need to know how to get there)
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