Sulphide ion reacts with `[Fe(CN)_(5)NO]` to form a purple coloured compound (X). In this reaction oxidation state of iron .

Sulphide ion reacts with `[Fe(CN)_(5)NO]` to form a purple coloured compound (X). In this reaction oxidation state of iron .
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Sulphide ion reacts with `[Fe(CN)_(5)NO]` to form a purple coloured compound (X). In this reaction ... . changes from +2 to +4 D. does not change.
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A blue colour complex is obtained in the analysis of `Fe^(+3)` having formula `Fe_(4)[Fe(CN)_(6)]_(3)` Let a= oxidation number of Iron in the corrdina

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What will be the oxidation number of Fe in `K_(3)[Fe(CN)_(6)]` :-

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How many are redox reaction- `{:((i),K_(4)[Fe (CN)_(6)] + "conc."H_(2)SO_(4) overset(Delta)rarr,(ii),"conc." H_(2)SO_(4) + KCl rarr),((iii),"conc." H_

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How many are redox reaction- `{:((i),K_(4)[Fe (CN)_(6)] + "conc."H_(2)SO_(4) overset(Delta)rarr,(ii),"conc." H_(2)SO_(4) + KCl rarr),((iii),"conc." H_

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`Na_(2)S + Na_(2)[Fe(CN)_(5)NO]to " X"` (Violet colour) The total number of possible isomers for complex " X" is , provided the ambident behaviour of

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Sodium nitroprusside `Na_(2)[Fe(CN)_(5)NO]` is used as a reagent for the detection of

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In `K_(4)[Fe(CN)_(6)],Fe` is in the form of

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Calculate the EAN of central atom in the following complexes `(a) [Cr(CO)_(6)]" "(b) [Fe(CN)_(6)]^(4-)" " (c ) [Fe(CO)_(5)] " " (d) [Co(NH_(3))_(6)]^(

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Hydrogen peroxide oxidises `[Fe(CN)_(6)]^(4-)` to `[Fe(CN)_(6)]^(3-)` in acidic medium but reduces `[Fe(CN)_(6)]^(3-)` to `[Fe(CN)_(6)]^(4-)` in alkal

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Hydrogen peroxide oxidises `[Fe(CN)_(6)]^(4-)` to `[Fe(CN)_(6)]^(3-)` in acidic medium but reduces `[Fe(CN)_(6)]^(3-)` to `[Fe(CN)_(6)]^(4-)` in alkal

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IUPAC name of `K_(3)[Fe(CN)_(6)]` is

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A compound X of the formula `C_(2)H_(6)O` on reaction with Na metal gave Y, X also reacts with `PC1_(5)` to give Z the product obtained in the reactio

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