The heat of neutralization example: A 275 mL of a 0.500 M HCl was mixed with 275 mL of a 0.500 M NaOH in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of the two solutions was room temperature (22.1 Celsius), and the final temperature of the mixed solution was 26.3 Celsius. Assume there is no heat lost to the surroundings and the densities and specific heats of the initial and final solutions are the same as for water (d = 1.00 g/mL and s = 4.184 J/g.C). Calculate the molar heat of neutralization for this reaction. Reference formula: constant Volume Calorimetry: ~used for combustion reactions ~done in the presence of XS oxygen gas ~no heat or mass is transferred (isolated system) For the above calorimeter: qsys = qcal + qrxn = 0 b/c no heat is transferred! SO qrxn = -qcal where qcal = heat absorbed by the bomb calorimeter = CcalΔT
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.
Q) The heat of neutralization example: A 275 mL of a 0.500 M HCl
was mixed with 275 mL of a 0.500 M NaOH in a constant-pressure calorimeter of negligible heat capacity. The initial
temperature of the two solutions was room temperature
(22.1 Celsius), and the final temperature of the mixed solution
was 26.3 Celsius. Assume there is no heat lost to the
surroundings and the densities and specific heats of the
initial and final solutions are the same as for water (d = 1.00
g/mL and s = 4.184 J/g.C). Calculate the molar heat of
neutralization for this reaction.
Reference formula: constant Volume Calorimetry:
~used for combustion reactions
~done in the presence of XS oxygen gas
~no heat or mass is transferred (isolated system)
For the above calorimeter:
qsys = qcal + qrxn = 0 b/c no heat is transferred! SO
qrxn = -qcal where qcal = heat absorbed by the bomb
calorimeter = CcalΔT
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