Chemistry Forum

Hi all! I'm actually new here and was hoping someone could help me decipher what exactly this question is asking.

Write a balanced equation for the reaction of dichromate ion, Cr₂O₇ -2 with chromium metal in aqueous acidic solution, to give Cr₃+ and water.

I'm just a little confused with what exactly chromium metal in aqueous acidic solution means, if it was just Cr or if the aqueous acidic solution actually plays apart in the equation?

Any help would be much appreciated.

Thanks!

in my opinion, the action is as following
Cr₂O₇ 2- + Cr =>Cr₃+

and the Cr₃+ will Disperse to the solution. And this is usefull for the reaction.

but if the solution is Based(PH>7), there will be OH- in the solution, so the following reaction will Cr₃+ + 3OH- == Cr(OH)₃！ .

and this reaction will stop the first reaction.



my personal web: www.chem-zone.com

thanks for the repsonse, but i'm still a tad confused with what exactly the dichromate reacting with a chromium metal in aqueous acidic solution means exactly.

is that just Cr₂O₇₂- + Cr -> Cr+3 + H₂O ...?

So the aqeous acidic solution plays no real part before the balancing?