Step-by-step explanation:
The given chemical equation is:
Fe(CN)63-(aq) + Re(s)-> Fe(CN)64-(aq) + ReO4-(aq)
Consider oxidation half reaction and balance it first in acidic conditions:
Add water on the left side to balance the O-atoms:
Add protons on the right side to balance H-atoms:
To balance the charge add electrons:
------------(1)
Reduction half reaction:
Fe(CN)63-(aq) -> Fe(CN)64-(aq)
Add electrons to balance the charge:
---------------(2)
Multiply equation(2) with seven :
------(3)
Add (1) and (3)
Add 8OH- on both sides:
It becomes:
This is the final equation in the basic medium.
Re(s) is oxidised. So it is the reducing agent.
Fe(CN)63- is reduced.It is the oxidising agent.