In the reaction of `I_(2)` with water, change in free energy is

Options

A. Negative
B. Positive
C. Zero
D. Can't be predicted

Answer

To determine the change in free energy (ΔG) for the reaction of iodine (I₂) with water, we can follow these steps:

### Step 1: Understand the Gibbs Free Energy Equation
The Gibbs free energy change (ΔG) can be calculated using the equation:
\[ \Delta G = \Delta H - T \Delta S \]
where:
- ΔG = change in Gibbs free energy
- ΔH = change in enthalpy
- T = temperature (in Kelvin)
- ΔS = change in entropy

### Step 2: Identify the Nature of the Reaction
The reaction of iodine with water can be represented as:
\[ I_2 + H_2O \rightarrow 2 HI \]
This reaction is known to be endothermic, meaning it absorbs heat.

### Step 3: Analyze the Enthalpy Change (ΔH)
Since the reaction is endothermic, the enthalpy change (ΔH) is positive:
\[ \Delta H > 0 \]

### Step 4: Analyze the Entropy Change (ΔS)
In this reaction, the formation of HI from I₂ and H₂O increases the disorder of the system, leading to a positive change in entropy:
\[ \Delta S > 0 \]

### Step 5: Determine the Sign of ΔG
Using the Gibbs free energy equation:
\[ \Delta G = \Delta H - T \Delta S \]
Given that ΔH is positive and ΔS is also positive, we need to consider the temperature (T). If the enthalpy change (ΔH) is greater than the product of temperature (T) and entropy change (ΔS), then:
\[ \Delta G > 0 \]
This indicates that the reaction is non-spontaneous under standard conditions.

### Conclusion
Thus, the change in free energy (ΔG) for the reaction of I₂ with water is positive.

### Final Answer
ΔG is positive.

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