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In the reaction, I(2)+2S(2)O(3)^(2-) r...

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

A

n-factor of `Na_(2)S_(4)O_(6)` is 2

B

equivalent weight of `I_(2)` is 127

C

`I_(2)` is oxidizing agent

D

`Na_(2)S_(2)O_(3)` is oxidizing agent

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D
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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 ?

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-)

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

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:

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 ?

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?

(a). IF both (A) and (R) are correct and (R) is the correct explanation of (A). (b). If both (A) and (R) are correct but (R) is not the correct explanation of (A). (c). If (A) is correct, but (R) is incorrect. (d). If (A) is incorrect, but (R) is correct. ltbr. (e) if both (A) and (R) are incorrect. Q. Assertion (A): Estimation of reducing substance by the use of standard I_(2) is called iodometry. Reason (R): in the reaction I_(2)+S_(2)O_(3)^(2-)toS_(4)O_(6)^(2-)+2I^(ɵ) The n factor of S_(2)O_(3)^(2-) is one.

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") The general difference equation for the above reaction is

In this reaction 2Na_(2)S_(2)O_(3)+I_(2) to Na_(2)SO_(4)O_(6)+2NaI_(2) , NaI_(2) acts as:

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