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In the process , Cl(g) + e^(-) overset(D...

In the process , `Cl(g) + e^(-) overset(DeltaH)(to)Cl^(-)(g)`, `DeltaH` is

A

positive

B

negative

C

zero

D

unpredictable

Text Solution

AI Generated Solution

The correct Answer is:
To determine the value of ΔH in the process \( Cl(g) + e^- \rightarrow Cl^-(g) \), we need to analyze the nature of the reaction involving chlorine gas and the addition of an electron. ### Step-by-Step Solution: 1. **Understanding the Process**: - The reaction involves a neutral chlorine atom in the gaseous state (\( Cl(g) \)) gaining an electron (\( e^- \)) to form a negatively charged chloride ion (\( Cl^-(g) \)). 2. **Defining Electron Gain Enthalpy**: - The energy change associated with the addition of an electron to a neutral atom is known as the electron gain enthalpy. For chlorine, this is specifically referred to as the first electron gain enthalpy. 3. **Nature of Electron Gain Enthalpy**: - The first electron gain enthalpy is typically exothermic for non-metals, including halogens like chlorine. This means that energy is released when an electron is added to the neutral atom. 4. **Sign of ΔH**: - Since the process is exothermic, the enthalpy change (ΔH) will be negative. This indicates that energy is released during the formation of the chloride ion from the neutral chlorine atom. 5. **Conclusion**: - Therefore, for the reaction \( Cl(g) + e^- \rightarrow Cl^-(g) \), the value of ΔH is negative. ### Final Answer: ΔH is negative. ---
To determine the value of ΔH in the process \( Cl(g) + e^- \rightarrow Cl^-(g) \), we need to analyze the nature of the reaction involving chlorine gas and the addition of an electron. ### Step-by-Step Solution: 1. **Understanding the Process**: - The reaction involves a neutral chlorine atom in the gaseous state (\( Cl(g) \)) gaining an electron (\( e^- \)) to form a negatively charged chloride ion (\( Cl^-(g) \)). 2. **Defining Electron Gain Enthalpy**: ...
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