Write a balanced redox equation for the following in acidic solution?
#C_2O_4^(2-)+Cr_2O_7^(2-)\toCO_2+Cr^(3+)#
I understand that #C_2O_4^(2-)\to2CO_2+2e^(-)#
but I don't know how the #Cr_2O_7^(2-)# part works out.
My attempt (where do the electrons go?)
#Cr_2O_7^(2-)+14H^(+)...\to2Cr^(3+)+7H_2O#
I understand that
but I don't know how the
My attempt (where do the electrons go?)
1 Answer
Well you gots a redox reaction here, which we address by the methods of half-equations that utilize electrons as stoichiometric particles...
Explanation:
Oxalate ion is oxidized to carbon dioxide...
We gots here the transition,
And meanwhile dichromate ion is REDUCED to
And for the balanced redox equation we simply add the half-equations in such a way as to eliminate the electrons....i.e.
....but we may cancel the electrons....
...to give after cancellation...
And so is this balanced with respect to MASS and charge...?
We could even further simplify this...by treating the