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Question

Balance the following redox reactions by ion electron method.
$$Cr_2O^{2-}_7+SO_2(g)\rightarrow Cr^{3+}(aq)+SO^{2-}_4(aq)$$ (in acidic solution)


Solution

The oxidation half reaction is $$\displaystyle SO_2(g) + 2H_2O(l) \rightarrow SO_4^{2-} + 4H^+(aq) +2e^- $$.
The reduction half reaction is $$\displaystyle Cr_2O_7^{2-}(aq) + 14H^+(aq) +6e^- \rightarrow 2Cr^{3+}(aq)
+ 7H_2O(l) $$.
The oxidation half reaction is multiplied by 3 and added to the reduction half reaction to obtain the balanced redox reaction.
$$\displaystyle Cr_2O^{2-}_7+3SO_2(g)+2H^+(aq) \rightarrow 2Cr^{3+}(aq)+3SO^{2-}_4(aq)+H_2O(l) $$

Chemistry
NCERT
Standard XI

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