Match Column I with Column II.
`{:(,"Column I ",,,"Column II"),((i) ,"Equilibrium",,(a),Delta G gt 0 ","K lt 1),((ii),"Spontaneous reaction",,(b),DeltaG=0),((iii),"Non-spontaneous reaction",,(c),Delta G ^(Θ)=0),(,,,(d),DeltaG lt 0 "," K gt 1):}`

Explanation

To solve the problem of matching Column I with Column II, we will analyze each item in Column I and determine its corresponding item in Column II based on the principles of thermodynamics and equilibrium.

### Step-by-Step Solution:

1. **Identify the first item in Column I: Equilibrium**
- At equilibrium, the Gibbs free energy change (ΔG) is equal to zero. This is because the forward and reverse reactions occur at the same rate, resulting in no net change in the system.
- Therefore, the correct match for equilibrium is **(b) ΔG = 0**.

2. **Identify the second item in Column I: Spontaneous reaction**
- A spontaneous reaction is characterized by a negative Gibbs free energy change (ΔG < 0). This indicates that the reaction can proceed without external energy input.
- Additionally, for spontaneous reactions, the equilibrium constant (K) is greater than 1, indicating that products are favored at equilibrium.
- Thus, the correct match for spontaneous reaction is **(d) ΔG < 0, K > 1**.

3. **Identify the third item in Column I: Non-spontaneous reaction**
- A non-spontaneous reaction occurs when the Gibbs free energy change is positive (ΔG > 0). This means that the reaction requires energy input to proceed.
- For non-spontaneous reactions, the equilibrium constant (K) is less than 1, indicating that reactants are favored at equilibrium.
- Therefore, the correct match for non-spontaneous reaction is **(a) ΔG > 0, K < 1**.

### Final Matches:
- (i) Equilibrium → (b) ΔG = 0
- (ii) Spontaneous reaction → (d) ΔG < 0, K > 1
- (iii) Non-spontaneous reaction → (a) ΔG > 0, K < 1

### Summary of Matches:
- i → b
- ii → d
- iii → a

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