Answer :
Final answer:
To answer the student's question, (a)1kg of CO₂ loses about -8924 kJ of heat when completely condensed at 195K. (b)The change in entropy in this process is around -45.8 J/K, and (c)the process is considered to be irreversible as it decreases the total entropy of the system.
Explanation:
There are few things we need to know before solving this problem. First, heat loss is calculated by using energy conversions and the heat of formation. The standard enthalpy of formation of CO₂(g) is −393.5 kJ/mol.
Second, the entropy change in a system, ΔS, can be calculated using the formula ΔS = qrev/T, where qrev is the heat lost or gained at a constant temperature.
Third, a reversible process is one in which the system and its surroundings can be returned to the original state by exactly reversing the change.
(a) In order to determine the amount of heat lost, we need to convert 1 kg of CO₂ to moles. This gives us 22661.7 moles.
We will then multiply this by the heat of formation, leading to an answer of approximately -8924 kJ.
Therefore, 1kg of CO₂ loses about -8924 kJ of heat when completely condensed at 195K.
(b) To find the change in entropy, we divide the heat lost by the absolute temperature. ΔS = qrev/T = -8924 kJ/195k , which gives us around -45.8 J/K.
(c) If the entropy of the system decreases, it is a sign that the process is irreversible, as no real process can decrease the total entropy of the system and its surroundings.
Since the entropy decreased in this case, the process is considered to be irreversible.
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