write the balanced half reaction for the conversion of CL(g)to Cl-(aq)
To write the balanced half-reaction for the conversion of Cl(g) to Cl-(aq), we need to consider the transfer of electrons.
The half-reaction for the reduction of chlorine gas (Cl2) to chloride ions (Cl-) is as follows:
Cl2(g) + 2e- → 2Cl-(aq)
In this reaction, two electrons are added to each molecule of Cl2 gas, resulting in the formation of two chloride ions (Cl-) with a negative charge.
Hence, the balanced half-reaction for the conversion of Cl(g) to Cl-(aq) is:
Cl2(g) + 2e- → 2Cl-(aq)
To write a balanced half-reaction for the conversion of Cl(g) to Cl-(aq), we need to consider the gain or loss of electrons during the reaction.
First, let's determine the oxidation state of chlorine in each species:
- Cl(g) is the elemental form of chlorine, so its oxidation state is 0.
- Cl-(aq) is the chloride ion, which has an oxidation state of -1.
Since the elemental form of chlorine has an oxidation state of 0, it means it does not gain or lose any electrons during the reaction, and its half-reaction will only include the Cl(g) species.
Now, let's write the balanced half-reaction:
Cl(g) → Cl-(aq)
To balance the equation, we need to add electrons (e-) on the appropriate side to equalize the charge. Since the oxidation state of Cl- is -1, we need to add one electron to the product side:
Cl(g) + e- → Cl-(aq)
This is the balanced half-reaction for the conversion of Cl(g) to Cl-(aq), where one electron is gained by Cl(g) to form Cl-(aq).