# Confusion in n-factor calculation

How do we calculate the equivalent weight of a compound, in a case where certain fraction of an element of the compound is getting reduced, while the other fraction is unaffected (no change in oxidation state)? For example, consider the following reaction:

$$\ce{Zn + K4[Fe(CN)6] -> K2Zn3[Fe(CN)6]2 + K}$$

I would like to calculate the equivalent weight of potassium ferrocyanide, given its molecular weight $M$. Here some potassium gets reduced to oxidation state (0) from (I).

• "Here, some potassium gets reduced to oxidation state (0) from (I)" That reaction equation makes no sense whatsoever. $\ce{K+}$ does not get reduced that way. – Gert Dec 4 '17 at 14:55
• Your reaction isn't even balanced. Please provide a reference for it. There no reducer strong enough in there to reduce $\ce{K+}$ to elemental K. The only reducing agent present is $\ce{Zn}$. – Gert Dec 4 '17 at 15:08
• @MaxW: to be fair, he didn't specify aqueous medium. – Gert Dec 4 '17 at 15:18
• I found numerous sources which suggest the following reaction: $$\ce{3Zn^2+ + 2[K4Fe(CN)6] -> K2Zn3[Fe(CN)6]2 + 6K+}$$ which is also performed in aqueous media only. Sorry, no potassium metal among products, not by a chance. – andselisk Dec 4 '17 at 16:23
• @andselisk: yes, I saw these too. OP's refusal to provide a reference speaks volumes. – Gert Dec 4 '17 at 16:26