`Delta H` for the reaction, `I_((g))+I_((g))rarr I_(2(g))` will be :-

Options

A. Zero
B. `-ve`
C. `+ve`
D. `oo`

Answer

To determine the enthalpy change (ΔH) for the reaction:

\[ \text{I}_{(g)} + \text{I}_{(g)} \rightarrow \text{I}_2{(g)} \]

we can analyze the process step by step.

### Step 1: Identify the Reactants and Products
The reactants are two iodine gas molecules (I) and the product is one iodine gas molecule (I2).

### Step 2: Understand Bond Formation
When two iodine atoms (I) come together to form a diatomic iodine molecule (I2), a bond is formed. This is a key point because bond formation is associated with the release of energy.

### Step 3: Determine the Nature of the Reaction
The formation of a bond releases energy, which means that the reaction is exothermic. In exothermic reactions, the enthalpy change (ΔH) is negative because energy is released to the surroundings.

### Step 4: Conclude the Value of ΔH
Since the formation of I2 from two I atoms involves bond formation and the release of energy, we conclude that:

\[ \Delta H < 0 \]

Thus, ΔH for the reaction is negative.

### Final Answer
The ΔH for the reaction \( \text{I}_{(g)} + \text{I}_{(g)} \rightarrow \text{I}_2{(g)} \) is negative.

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