Hi all, I am learning about balancing chemical reactions using redox oxidation #s, and I am having trouble with questions with this format:
-one side of the reaction has more of the redox elements than the other side
e.g.
K2Cr2O7+3HCl -> CrCl3+KCl + Cl2 +H2O
What I did so far was finding the RA (reducing agent) and OA, i found out that obviously the Cr +6 reduced to Cr +3 and Cl -1 oxidized 0 (Cl2).
But I am still having trouble, because even though Cl undergoes redox, what about the other Cl-containing compounds like KCl and such, do I have to balance the Cl of those with my HCl??