Consider the processes I) NaCl(s) −→ Na+(aq) + Cl−(aq) II) CaCO3(s) −→ CaO(s) + CO2(g) III) H2O(ℓ) −→ H2O(s) For which cases would entropy of the system increase as the given process proceeds left to right? 1. I, II, III 2. I, II 3. III only 4. I, III 5. II only 6. II, III 7. I only

Option 2

In process I & II entropy of the system increases proceed from left to right.

Explanation:

Entropy is an extensive property of the system. It means it depends on the amount or quantity of the system

In case for process 1

since one mole sodium chloride dissolve in water and it dissociate into two ions i.e. Na⁺ and Cl⁻

For process 2

CaCO₃(s) → CaO(s) + CO₂(g)

Change in gaseous moles = (Product moles - reactant moles)

                                 ⇒ Δng = 1

Since  Δng > 0 it means randomness increases of the system from left to right. So, ΔS > 0