\"In the reaction Cl2(g) + S2O3 (2-)(aq) ? Cl?(aq) + SO4 (2-)(aq) of the thiosul

Question

"In the reaction Cl2(g) + S2O3 (2-)(aq) ? Cl?(aq) + SO4 (2-)(aq) of the thiosulfate ion with chlorine gas in an acidic solution:

Balance the equation using oxidation and reduction half-reactions. What is the smallest possible integer coefficient of Cl? in the combined balanced equation?"

I cannot figure out how to balance the thiosulfate half reaction for the life of me! It seems impossible. Is there something I'm missing? Please write explanations for any work so I can understand this problem. Thank you!!! :]

Explanation / Answer

A) __CL2 (g) + __S2O3^2- (aq) --> Cl- (aq) + __SO4^2- (aq)

Cl2 rule #1 @ zero take 2 electrons --> are reduced to 2(Cl)-1
[Cl2 , the oxidizer... took ... & went down in charge]

(S2O3)-2 has 3 O-2 's & needs 2 S+2 's to add up to -2 of (S2O3)-2
(SO4)-2 has 4 O-2 's & needs S+6 to add up to -2 of (SO4)-2
So: (S2O3)-2 @ 2 S+2 each--> 2 (SO4)-2 @ +6 each & 8 elec's lost

so we got:
Cl2 & 2 electrons taken --> 2 Cl-
(S2O3)-2 --> 2 (SO4)-2 & 8 electrons lost

we 4 times the Cl2 , to balance electrons:
4 Cl2 & 8 electrons taken --> 4 Cl-
(S2O3)-2 --> 2 (SO4)-2 & 8 electrons lost

combine:
A) 4CL2 + 1 (S2O3)2- --> 8 Cl- + 2 (SO4)2-

"if" more is asked of you, to balance charges & oxygen & hydrogens:

I will balance the total charge of both sides with H+ :
4CL2 + 1 (S2O3)2- --> 8 Cl- + 2 (SO4)2- & 10 H+

balance the Hydrogens using neutral water:
4CL2 + 1 (S2O3)2- 5 H2O--> 8 Cl- + 2 (SO4)2- & 10 H+

other answers:
Cl2 was theoxidizing agent(it took,...& its charge went down)
S2O3)-2 was the reducing agent (did the opposite)

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