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Answer :
Final answer:
The enthalpy change of the surroundings, ΔHsurr, can be found using the equation ΔHsurr = -ΔHsystem. The entropy change of the surroundings, ΔSsurr, can be calculated using the equation ΔSsurr = -ΔHsurr / T. The change in the universe, ΔSuniv, is equal to the sum of the entropy changes of the system and surroundings.
Explanation:
The enthalpy change of the surroundings, ΔHsurr, can be calculated using the equation:
ΔHsurr = -ΔHsystem
where ΔHsystem is the enthalpy change of the system, which in this case is the enthalpy of vaporization. The entropy change of the surroundings, ΔSsurr, can be calculated using the equation:
ΔSsurr = -ΔHsurr / T
where T is the temperature in Kelvin. The change in the universe, ΔSuniv, is equal to the sum of the entropy changes of the system and surroundings:
ΔSuniv = ΔSsystem + ΔSsurr
In order to calculate the values of ΔHsurr and ΔSsurr, we need the temperature in Kelvin. To convert 55°C to Kelvin, we add 273.15 which gives us a temperature of 328.15 K. Now we can substitute the values into the equations:
ΔHsurr = -(38.6 kJ/mol)
ΔSsurr = -(-38.6 kJ/mol) / 328.15 K
We can then calculate ΔSuniv by adding the entropy change of the system to the entropy change of the surroundings:
ΔSuniv = 110 J/(K*mol) + -(38.6 kJ/mol) / 328.15 K
Therefore, the values of ΔHsurr, ΔSsurr, and ΔSuniv at 55°C are approximately -38.6 kJ/mol, 118.4 J/(K*mol), and 109.7 J/(K*mol), respectively.
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