Question

Write a balanced oxidation-reduction equation (in acidic solution) for the following:
\[\large{C_2O_4^{2-}+Cr_2O_7^{2-}\rightarrow CO_2+Cr^{3+}}\]

Answer 1

do you have any idea ? on the right side there is one carbon when on the left side there are 2 carbons - what you need to do ? or on the left side there are 2 croms and on the right side just 1 Cr. how you balance it ?

Answer 2

kitty how you ve learned this ? when there are in the left side 2 carbons like in the above your preblem and in the right side there is just one carbone so you need multiply it in the right side by 2 and in this way the carbons from every two parts will be balanced and will get this form

C_2O_4 +Cr_2O_7 -> 2CO_2+Cr

Answer 3

so now try getting the equilibru of oxigens - any idea for this way ?

Answer 4

I don't understand what you refer to. Sorry! I responded very late.

I'll close the question. I got it anyway. :)