50.0 mL sample of a 1.00 MM solution of CuSO4CuSO4 is mixed with 50.0 mL of 2.00 MM KOHKOH in a calorimeter. The temperature of both solutions was 24.6 oCoC before mixing and 32.8 oCoC after mixing. The heat capacity of the calorimeter is 12.1 J/K. From these data, calculate ΔHΔH for the process: CuSO4(1M)+2KOH(2M)→Cu(OH)2(s)+K2SO4(0.5M)CuSO4(1M)+2KOH(2M)→Cu(OH)2(s)+K2SO4(0.5M) Assume that the specific heat and density of the solution after mixing are the same as those of pure water and that the volumes are additive.
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.
A 50.0 mL sample of a 1.00 MM solution of CuSO4CuSO4 is mixed with 50.0 mL of 2.00 MM KOHKOH in a calorimeter. The temperature of both solutions was 24.6 oCoC before mixing and 32.8 oCoC after mixing. The heat capacity of the calorimeter is 12.1 J/K. From these data, calculate ΔHΔH for the process:
CuSO4(1M)+2KOH(2M)→Cu(OH)2(s)+K2SO4(0.5M)CuSO4(1M)+2KOH(2M)→Cu(OH)2(s)+K2SO4(0.5M)
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