75.0 mL of 1.80 M CUSO 4 solution is mixed with 150 mL of 1.80 M NAOH solution in a coffee cup calorimeter of negligible heat capacity. If the initial temperature of the two solutions are both 21.0 degrees C, and the final temperature of the mixed solution is 27.1, how much heat was released by the reaction? Assume density of solution d is 1.00 g/mL and that the solution has the same specific heat as water. The thermochemical equation is: CuSO4 (ag) + 2NAOH (ag) --> Cu(OH)2 (s) + Na SO4 (ag) AH pxn = - 42.3 kJ/mol rxn Hint: no limiting reagent, substances are presented in correct molar ratios. O 6180 J O 9270 J O 3120 J O 5740 J O 9300 J O 1250 J O 6230 J O 3380 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.
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