Write a balanced equation for the reaction of liquid bromine with chlorine gas.

The balanced equation for the reaction of liquid bromine (Br2) with chlorine gas (Cl2) is as follows:

Br2 + Cl2 -> 2BrCl

To write a balanced equation for the reaction between liquid bromine (Br2) and chlorine gas (Cl2), we need to know the products formed. In this case, bromine and chlorine combine to form two possible products: bromine chloride (BrCl) and bromine trichloride (BrCl3).

Since we know the reactants and possible products, we can write the generic equation as follows:

Br2 + Cl2 → BrClx

To determine the values of x (the stoichiometric coefficient), we need to consider the oxidation states of bromine and chlorine.

Bromine can have an oxidation state of 0, +1, +3, +5, or +7. Chlorine, on the other hand, typically has an oxidation state of -1.

To form bromine chloride (BrCl), bromine must have an oxidation state of +1 and chlorine -1. Therefore, the balanced equation for the formation of bromine chloride is:

Br2 + Cl2 → 2BrCl

If we consider the formation of bromine trichloride (BrCl3), bromine has an oxidation state of +3 and chlorine -1. Thus, the balanced equation for the formation of bromine trichloride is:

Br2 + 3Cl2 → 2BrCl3

Therefore, the balanced equation for the reaction of liquid bromine with chlorine gas can be one of the following, depending on the product formed:

Formation of bromine chloride:
Br2 + Cl2 → 2BrCl

Formation of bromine trichloride:
Br2 + 3Cl2 → 2BrCl3

2,2,2

Bromine and Chlorine react to form Bromine monochloride.

Bromine and Chloride are both diatomics so, in their elemental forms, they have two atoms.

_Br2 + _Cl2 -> _BrCl

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