The values based on the enthalpy of vaporization of ethanol illustrated is given below.
<h3>What is enthalpy?</h3>
It should be noted that enthalpy is the sum of the internal energy as well as the product of the pressure and the volume of a thermodynamic system.
It should be noted that enthalpy is a property of a thermodynamic system, and it's the sum of the system's internal energy and the product of its pressure and volume.
It is a state function that's used in many measurements in biological, chemical, and physical systems at a constant pressure.
ΔSsys = ΔH/T = (38700 J/mol) /(78+273) = 110.3 J/Kmol
ΔSsurr = -ΔSsys = -110.3 J/Kmol
ΔSuniverse = ΔSsurr +ΔSsys = 110.3 + -110.3 = 0 J/Kmol
Complete question:
The enthalpy of vaporization of ethanol is 38.7 kJ/mol at its boiling point (78°C).
Determine ΔSsys,ΔSsurr, andΔSuniv when 1.00 mol of ethanol is vaporized at 78°C and 1.00 atm
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Explanation:
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Answer:
The inner core is solid because the inner core consists of a lot of pressure and high temperatures. And the more pressure and high temperatures the more dense the substance gets.
