The correct option is C Fe_2O_3 A light green crystalline solid is expected to be nbsp;ferrous sulphate. There is no reaction with dilute sulphuric acid ...

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Borax

Name the comp...

Question

Name the compound D.

F e (O H)_{2}

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F e O

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F e_{2} O_{3}

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F e_{3} O_{4}

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Solution

The correct option is C $F e_{2} O_{3}$
A light-green crystalline solid is expected to be ferrous sulphate. There is no reaction with dilute sulphuric acid. With potassium permanganate, ferrous sulphate is oxidized to ferric sulphate and the pink color disappears. On strong heating, it gives two gases which are two oxides of sulphur, along with a brown residue, ferric oxide. When gases are passed through acidified potassium dichromate, it is reduced by sulphur dioxide to give a green solution of chromium sulphate. On adding barium sulphate, the green solution of sulphate gives a white precipitate of barium sulphate. In charcoal cavity test, ferric oxide is reduced to iron which is magnetic.
$F e S O_{4} + d i l ⟶ N o r e a c t i o n$
$\begin{matrix} F e S O_{4} & + & K M n O_{4} & H_{2} S O_{4} - --- \to & F e_{2} (S O_{4})_{3} & + & M n^{2 +} (P i n k) & (C o l o r l e s s) \end{matrix}$
$F e S O_{4} Δ - \to F e_{2} O_{3} + S O_{2} ↑ + S O_{3} ↑$
$\begin{matrix} K_{2} C r_{2} O_{7} & + & S O_{2} & H_{2} S O_{4} - --- \to & C r_{2} (S O_{4})_{3} G r e e n \end{matrix}$
$H_{2} O + S O_{3} ⟶ H_{2} S O_{4}$
$\begin{matrix} H_{2} S O_{4} & + & B a (N O_{3})_{2} & ⟶ & 2 H N O_{3} & + & B a S O_{4} ↓ W h i t e \end{matrix}$

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Similar questions

In the production of iron, intermediate are $F e O$ , $F e_{2} O_{3}$ , and $F e_{3} O_{4}$ , which are oxide . If true enter 1 else 0.

Q. If

F e C l_{3}

is added to excess of hot water

Q. Consider the reaction:

F e_{2} O_{3} ⟶ F e_{3} O_{4}

n

-factor for

F e_{3} O_{4}

is :

Q. If

Δ G = - 177

Kcal for

2 F e (s) + \frac{3}{2} O_{2} (g) \to F e_{2} O_{3} (s)

and

Δ G = - 19 K c a l

for

4 F e_{2} O_{3} (s) + F e (s) \to 3 F e_{3} O_{4} (s)

. What is the Gibbs free energy of formation of

F e_{3} O_{4} (s)

Q. Balance the following equations by oxidation number method.

C O + F e_{3} O_{4} \to F e O + C O_{2}

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