Problem: Consider two processes: sublimation of I2 (s) and melting of I2 (s) (Note: the latter process can occur at the same temperature but somewhat higher pressure).I2(s) ⟶ I2(g)                    I 2(s) ⟶ I2(l)Is ΔS  positive or negative in these processes? In which of the processes will the magnitude of the entropy change be greater?

🤓 Based on our data, we think this question is relevant for Professor Grant's class at HUNTER.

FREE Expert Solution

entropy: gas > liquid > solid


I2 (s) → I2 (g)

solid to gas

increase in entropy


I2 (s) → I2 (l)

solid to liquid


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Problem Details

Consider two processes: sublimation of I2 (s) and melting of I2 (s) (Note: the latter process can occur at the same temperature but somewhat higher pressure).

I2(s) ⟶ I2(g)                    I 2(s) ⟶ I2(l)

Is ΔS  positive or negative in these processes? In which of the processes will the magnitude of the entropy change be greater?

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