Cr2O7
2−+SO2(g)→Cr3+(aq)+SO4
2−(aq) (in acidic solution)
Answers
Explanation:
The reaction we are given here to Balance Cr_{2}{O_{7}}^{2-} + SO_{2}Cr
2
O
7
2−
+SO
2
gives cr_{3}+ + SO_{4}^{2-}SO
4
2−
is basically an example or a type of redox reaction.
In other words we can say there are two types of half reactions that has been taking place in the above given reaction one that has oxidation happening in it and other half has reduction happening in it.
So the two reactions to balance the equation would be
Cr_{2}{O_{7}}^{2-} + 14 H_{2}O + 6e^- \rightarrow 2Cr_{3}+ + 7H_{2}O + 14OH^-Cr
2
O
7
2−
+14H
2
O+6e
−
→2Cr
3
++7H
2
O+14OH
−
3{SO_{3}}^{2-} + 3H-{2}O + 6OH^- \rightarrow 3SO_{4}^{2-} + 6H_{2}O + 6e^-3SO
3
2−
+3H−2O+6OH
−
→3SO
4
2−
+6H
2
O+6e
−
Show the final balanced equation will be
3SO_{3}2^- + Cr_{2}{O_{7}}^{2-} + 4H_{2}O \rightarrow 2Cr_{3}+ + 3SO_{4}^{2-} + 8OH^-3SO
3
2
−
+Cr
2
O
7
2−
+4H
2
O→2Cr
3
++3SO
4
2−
+8OH
−