Give the half-equations for the reaction between aluminium metal and liquid bromine (Br2):
Al ==> Al^3+ + 3e
Br2 + 2e ==> 2Br^-
To determine the half-equations for the reaction between aluminium metal and liquid bromine (Br2), we need to consider the oxidation and reduction half-reactions that occur.
Step 1: Identify the oxidation and reduction reactions:
In this case, aluminium is oxidized from its elemental state (Al) to Al3+ ions, and bromine molecules (Br2) are reduced to bromide ions (Br-).
Step 2: Write the half-equations for oxidation and reduction:
Oxidation half-equation:
Al(s) -> Al3+(aq) + 3e-
Reduction half-equation:
Br2(l) + 2e- -> 2Br-(aq)
Note that the number of electrons released in the oxidation half-equation must be equal to the number of electrons consumed in the reduction half-equation. This ensures that the overall charge is balanced in the chemical reaction.
Step 3: Balance the equations (optional):
In this case, the equations are already balanced. However, if they were unbalanced, you would need to adjust the coefficients to ensure that the number of atoms and charges are balanced on both sides of the equation.
Overall redox reaction:
Al(s) + Br2(l) -> Al3+(aq) + 3Br-(aq)
These half-equations show the transfer of electrons during the reaction between aluminium metal and liquid bromine.