Question

Calculate the oxidation number of Fe in Fe4[Fe(CN)6]

Answer 1

Answer:

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Answer 2

Answer:

Concept:

Iron oxides are iron and oxygen-based chemical compounds. Rust, a type of iron(III) oxide, is the most well-known of the sixteen recognized iron oxides and oxyhydroxides. Iron oxides and hydroxides are abundant in nature and are involved in a variety of biogeophysical processes. They are found in haemoglobin and are employed as iron ores, colors, catalysts, and thermite. Iron oxides are a low-cost, long-lasting pigment used in paints, varnishes, and coloured concretes. The golden spectrum's "earthy" end is frequently available. It bears the E number E172 if used as a food colour.

Given:

Determine the redox potential of Fe in the following equation. Fe4[Fe(CN)6]

Find:

find the oxidation number of given equation

Answer:

Determine the redox potential of Fe in the following equation $Fe_{4} [Fe(CN)_{6} ]_{3}$

1. Oxidation state of outer $Fe$

$Fe_{4} [Fe(CN)_{6} ]_{3}$ being a salt will dissociate as :

$Fe_{4} [Fe(CN)_{6} ]_{3} - > 4Fe_{3} +3[Fe(CN)_{6} ]4-$

As a result, the outer $Fe's$ oxidation state is $3+$.

2. Oxidation State of inner $Fe$

Let Fe's oxidation number be $X$

Here oxidation number on $CN=-1$

For $[Fe(CN)_{6} ]4-$

$X$ × $6(-1)$

$= -4$

∴ $X = +2$

Hence the oxidation state/ number of inner is $Fe +2$

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