A 4.348 g sample of NaOH(s) is dissolved in 100 g of water in a calorimeter making 104.348 g of solution. The temperature rises from 23.6 oC to 47.4 oC. Calculate1 ∆Hdiss in kJ/mol. ALL DIMENSIONAL ANALYSIS MUST BE EXPLICITLY SHOWN: Assume: Ccalorimeter = 35.5J / °C and Csolution = Cwater = 4.18 J / g·K. Calculate the amount of heat absorbed by the solution (qsoln). Calculate the amount of heat absorbed by the calorimeter (qcal). Assume the temperature change is the same for the solution and the calorimeter. Determine the amount of heat given off as the 4.348g NaOH dissolved (qdiss). Look at equation 2. Make sure to include an appropriate sign indicating whether it is an endothermic (+) or exothermic (-) process. Determine the number of moles of NaOH that dissolved. Determine the amount of heat given off per mole of NaOH dissolved (ΔHdiss). Look at equation 3. Provide your answer in units of kJ/mol.
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 4.348 g sample of NaOH(s) is dissolved in 100 g of water in a calorimeter making 104.348 g of solution. The temperature rises from 23.6 oC to 47.4 oC. Calculate1 ∆Hdiss in kJ/mol. ALL DIMENSIONAL ANALYSIS MUST BE EXPLICITLY SHOWN:
Assume: Ccalorimeter = 35.5J / °C and Csolution = Cwater = 4.18 J / g·K.
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Calculate the amount of heat absorbed by the solution (qsoln).
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Calculate the amount of heat absorbed by the calorimeter (qcal). Assume the temperature change is the same for the solution and the calorimeter.
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Determine the amount of heat given off as the 4.348g NaOH dissolved (qdiss). Look at equation 2. Make sure to include an appropriate sign indicating whether it is an endothermic (+) or exothermic (-) process.
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Determine the number of moles of NaOH that dissolved.
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Determine the amount of heat given off per mole of NaOH dissolved (ΔHdiss). Look at equation 3. Provide your answer in units of kJ/mol.
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