For the reaction, `2Cl(g) to Cl_2(g)`, what are the signs of `DeltaH and DeltaS` ?

Explanation

To determine the signs of ΔH (enthalpy change) and ΔS (entropy change) for the reaction \(2Cl(g) \rightarrow Cl_2(g)\), we can analyze the process step by step.

### Step 1: Understanding the Reaction
The reaction involves two chlorine atoms (Cl) in the gas phase combining to form one molecule of chlorine gas (Cl₂).

### Step 2: Analyzing ΔH (Enthalpy Change)
- **Bond Formation**: When two chlorine atoms combine to form a Cl₂ molecule, a bond is formed. The formation of bonds releases energy, which means this process is exothermic.
- **Sign of ΔH**: Since the reaction is exothermic, the enthalpy change (ΔH) is negative.
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