A student performed this experiment by mixing 50.0 mL of 2.0 M NaOH solution with 50.0 mL of 2.0 M HCl solution. The student found the temperature change for this reaction to be 12.4 C. Assuming the density of the solution was 1.03 g/mL, the Cp for the solution is the specific heat for water (4.184 J/g℃) and the Ccal is 18.1 J/℃. a. Determine the amount of heat absorbed by the calorimeter (qcal). b. Determine the amount of heat absorbed by the solution (qsolution). c. Determine the heat produced in this reaction in kJ (qrxn). d. Calculate the enthalpy change, ∆H, for the reaction in kJ/mol HCl.
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 student performed this experiment by mixing 50.0 mL of 2.0 M NaOH solution with 50.0 mL of 2.0
M HCl solution. The student found the temperature change for this reaction to be 12.4 C. Assuming
the density of the solution was 1.03 g/mL, the Cp for the solution is the specific heat for water (4.184
J/g℃) and the Ccal is 18.1 J/℃.
a. Determine the amount of heat absorbed by the calorimeter (qcal).
b. Determine the amount of heat absorbed by the solution (qsolution).
c. Determine the heat produced in this reaction in kJ (qrxn).
d. Calculate the enthalpy change, ∆H, for the reaction in kJ/mol HCl.
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