ith the given data: Initial temperature = 30oC; Final temperature = 50oC Initial volume of water = 100 mL; Final volume of water = 100 mL Initial volume of isopropyl alcohol = 200 mL; Final volume of isopropyl alcohol = 195 mL Density of water = 1.00 g/mL specific heat of water = 4.18 J/goC Relative density of 70% isopropyl alcohol is 0.79 a.) Find the mass of the fuel burnt (mfuel) b.) The amount of moles of the fuel burnt, (nfuel) c.) molar enthalpy of combustion of the fuel by using the equation: ΔcH=(q/nfuel)(1kJ/1000J) d.) Would there be a change in the value of enthalpy of combustion if the water is heated until a 30oC change is observed, rather than 20oC? Why or why not?
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.
With the given data:
Initial temperature = 30oC; Final temperature = 50oC
Initial volume of water = 100 mL; Final volume of water = 100 mL
Initial volume of isopropyl alcohol = 200 mL; Final volume of isopropyl alcohol = 195 mL
Density of water = 1.00 g/mL
specific heat of water = 4.18 J/goC
Relative density of 70% isopropyl alcohol is 0.79
a.) Find the mass of the fuel burnt (mfuel)
b.) The amount of moles of the fuel burnt, (nfuel)
c.) molar enthalpy of combustion of the fuel by using the equation:
ΔcH=(q/nfuel)(1kJ/1000J)
d.) Would there be a change in the value of enthalpy of combustion if the water is heated until a 30oC change is observed, rather than 20oC? Why or why not?
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