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

Explanation

To determine the signs of ΔH (change in enthalpy) and ΔS (change in entropy) for the reaction:

\[ 2Cl(g) \rightarrow Cl_2(g) \]

we can analyze the process step by step.

### Step 1: Analyze ΔH (Change in Enthalpy)

1. **Identify the nature of the reaction**: The reaction involves the formation of a chlorine molecule (Cl₂) from two chlorine atoms (Cl).
2. **Bond formation**: When two Cl atoms combine to form Cl₂, a bond is formed. The formation of bonds typically releases energy.
3. **Sign of ΔH**: Since energy is released during the formation of the Cl₂ molecule, ΔH is negative.

### Step 2: Analyze ΔS (Change in Entropy)

1. **Understanding entropy**: Entropy (S) is a measure of the randomness or disorder of a system.
2. **Initial and final states**: Initially, we have two separate Cl atoms (2Cl), which have a higher degree of randomness compared to a single Cl₂ molecule.
3. **Change in randomness**: The formation of one molecule from two atoms results in a decrease in the number of gas particles, leading to a decrease in randomness.
4. **Sign of ΔS**: Since the final state (Cl₂) is more ordered than the initial state (2Cl), ΔS is negative.

### Conclusion

- The sign of ΔH is **negative**.
- The sign of ΔS is **negative**.

### Summary of Results
- ΔH: Negative
- ΔS: Negative

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