How do you balance #Cr(s) + Fe(NO_3)_2(aq) -> Fe(s) + Cr(NO_3)_3(aq)#?

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Answer 1 · 2017-05-15T07:52:02

Write the individual redox equations........

Chromium metal is oxidized..........

#Cr(s) rarrCr^(3+) +3e^(-)# #(i)#

And #Fe^(2+)# is reduced...........

#Fe^(2+) +2e^(-) rarr Fe(s)# #(ii)#

And we cross multiply to multiply to remove the electrons: #2xx(i)+3xx(ii):#

#3Fe^(2+)+2Cr(s) rarr 3Fe(s)+2Cr^(3+)#

And if you like, you can add in some nitrate ions........

#3Fe(NO_3)_2+2Cr(s) rarr 3Fe(s)+2Cr(NO_3)_3(aq)#