Hello, everyone! I have a quick homework question that I assume has some relation to the reactivity series? It goes like this: "Would it be a good idea to store a solution of zinc nitrate in a container made of iron?  Why or why not?" I suspect it would be a fine idea to store the solution of zinc nitrate in a container made of iron because iron is less reactive than zinc and cannot displace it? I'm not entirely sure, as we skimmed over the reactivity series in class, so I would really appreciate a more in-depth and thorough answer. Thank you guys so much! 

33 minutes ago, Kagi98JP said:

Hello, everyone! I have a quick homework question that I assume has some relation to the reactivity series? It goes like this: "Would it be a good idea to store a solution of zinc nitrate in a container made of iron?  Why or why not?" I suspect it would be a fine idea to store the solution of zinc nitrate in a container made of iron because iron is less reactive than zinc and cannot displace it? I'm not entirely sure, as we skimmed over the reactivity series in class, so I would really appreciate a more in-depth and thorough answer. Thank you guys so much! 

Your logic looks OK to me. I see, consulting my Periodic Table, that the electronegativity of Fe is greater than that of Zn, so it doesn't look as if Fe will give up its electrons to Zn2+.  (Also, as I recall, the principle of galvanising relies on Zn being preferentially oxidised and thus protecting the Fe.)  

What about the zinc giving up electrons to the iron?

 

13 hours ago, Country Boy said:

What about the zinc giving up electrons to the iron?

 

To do that to Fe metal would involve make a "ferride" anion, Fe⁻ or something. That would not happen.  

But Zn metal could give electrons to Fe²⁺ or Fe³⁺ cations, reducing them to Fe, while the Zn was correspondingly oxidised to Zn²⁺.