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Consider the redox reaction 2S(2)O(3)^...

Consider the redox reaction
`2S_(2)O_(3)^(2-)+I_(2)rarrS_(4)O_(6)^(2-)+2I^(ө)`

A

`S_(2)O_(3)^(2-)` gets reduced to `S_(4)O_(6)^(2-)`

B

`S_(2)O_(3)^(2-0)` gets oxidised to `S_(4)O_(6)^(2-)`

C

`I_(2)` gets reduced to `I^(-)`

D

`I_(2)` gets oxidised to `I^(-)`

Text Solution

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The correct Answer is:
B, C
S undergoes increase in oxidation number from +2 to +2.5, while I undergoes decrease in oxidation number from 0 to -1.
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Consider the reaction: 2S_(2)O_(3)^(2-)(aq)+I_(2)(s) rarr S_(4)O_(6)^(2-)(aq) + 2I^(Θ)(aq) 2S_(2)O_(3)^(2-)(aq) + 2Br_(2)(l) + 5H_(2)O(l) rarr 2SO_(4)^(2-)(aq) + 4Br^(Θ)(aq)+10H^(o+)(aq) Why does the same reductant, thiosulphate, react differently with iodine and bromine?

In the reaction, 2S_(2)O_(3)^(2-)+I_(2)rarrS_(4)O_(6)^(2-)+2I^(-) . The eq. wt. of Na_(2)S_(2)O_(3) is equal to its:

I_(2)+S_(2)O_(3)^(2-) to I^(-)+S_(4)O_(6)^(2-)

I_(2)+S_(2)O_(3)^(2-) to I^(-)+S_(4)O_(6)^(2-)

Thiosulphate reacts differently with iodine and bromine in the reactions given below : S_(2)O_(3)^(2-)+I_(2) rarr S_(4)O_(6)^(2-) + 2I^(-) S_(2)O_(3)^(2-)+2Br_(2)+5H_(2)O rarr 2SO_(4)^(2-)+2Br^(-)+10H^(+) Which of the following statements justifies the above dual behaviour of thiosulphate ?

In the reaction, I_(2)+2S_(2)O_(3)^(2-) rarr 2I^(-)+S_(4)O_(6)^(2-) .

The reaction S_(2)O_(8)^(2-) + 3I^(ɵ) rarr 2SO_(4)^(2-) + I_(3)^(ɵ) is of first order both with respect to persulphate and iofide ions. Taking the initial concentration as a and b , respectively, and taking x as the concentration of the triofide at time t , a differential rate equation can be written. Two suggested mechanism for the reaction are: I. S_(2)O_(8)^(2-)+I^(ɵ) hArr SO_(4)I^(ɵ)+SO_(4)^(2-) ("fast") I^(ɵ)+SO_(4)I^(ɵ) overset(k_(1))rarrI_(2) + SO_(4)^(2-) (show) I^(ɵ) + I_(2) overset(k_(2))rarr I_(3)^(ɵ) ("fast") II. S_(2)O_(8)^(2-) + I^(ɵ) overset(k_(1))rarr S_(2)O_(8) I^(2-) (slow) S_(2)O_(8)I^(3-) overset(k_(2))rarr2SO_(4)^(2-)+I^(o+) ("fast") I^(o+) + I^(ɵ) overset(k_(3)) rarr I_(2) ("fast") I_(2) + I^(o+) overset(k_(4))rarr I_(3)^(ɵ) ("fast") For the reaction I_(2)+2S_(2)O_(3)^(2-) rarr S_(4)O_(6)^(2-) + 2I^(ɵ) I. (-d[I_(2)])/(dt) = -(1)/(2) (d[S_(2)O_(3)^(2-)])/(dt) II. (-d[I_(2)])/(dt) = -2 (d[S_(2)O_(3)^(2-)])/(dt) III. (-d[I_(2)])/(dt) = -2 (d[I^(ɵ)])/(dt) xx (d[S_(2)O_(3)^(2-)])/(dt) IV. (d[S_(4)O_(6)^(2-)])/(dt) = (1)/(2)(d[I^(ɵ)])/(dt) The correct option is

How many gram of I_(2) are present in a solution which requires 40 mL of 0.11N Na_(2)S_(2)O_(3) to react with it, S_(2)O_(3)^(2-)+I_(2)rarrS_(4)O_(6)^(2-)+2I

A constant current was flowen for 1 mi n through a solution of Kl . At the end of experiment, liberated I_(2) consumed 150mL of 0.01M solution of Na_(2)S_(2)O_(3) following the reaction : I_(2)+2S_(2)O_(3)^(2-) rarr 2I^(c-)+S_(4)O_(6)^(2-) What was the average rate of current flow in ampere ?

In the reaction, I_(2)+2S_(2)O_(3)^(2-) rarr 2I^(-)+S_(4)O_(6)^(2-) . Equivalent wieght of iodine will be equal to

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