Given that the normal boiling point of CCl4 is 77 °C, which of the following statements about the process below is/are correct? You may choose more than one, or none, of the statements.

Question

CCl4(l, 68 °C, 1 atm) ⟶ CCl4(g, 101 °C, 1 atm)

Assume that the temperature of the surroundings is constant and also equal to 101 °C.

Note: The normal boiling point (Tnbp) is the boiling temperature at 1 atm. The phase change is reversible at the normal boiling point but irreversible if P = 1 atm and T ≠ Tnbp.

a. The entropy of the system increases: ΔS > 0.
b. The entropy of the surroundings increases: ΔSsurr > 0.
c. The entropy of the universe increases: ΔSuniv > 0.
d. Work is done by the system on the surroundings.
e. Heat flows from the system into the surroundings.
f. The entropy change for the system is equal to ΔH / Tvap.
g. The entropy change for the system is equal to ΔH / Tsurr.
h. The process is thermodynamically reversible.

would be grateful if you can explain how to solve this question

Answer 1

I think you could make some picks if you just looked up the definitions. For example, If CCl4 changes from a liquid to a gas, you know molecules are more random in a gas than in the liquide; therefore, disorder has increased so dS must be > 0. So you pick a. For c, you KNOW that the universe is increasing disorder. That's c. etc.