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Oxides of Sulphur

Two solid lab...

Question

Two solid laboratory reagents (A) and (B) gives the following reactions:
Compound (A):
(i) on strongly heating gives two oxides of sulphur
(ii) on adding aqueous NaOH solution to its aqueous solution, a dirty green precipitate is obtained which starts turning brown on exposure to air
Compound (B) :
(iii) imparts green colour to the flame
(iv) Its solution does not give a precipitate on passing $H_{2} S$
(v) When it is heated with solid $K_{2} C r_{2} O_{7}$ and concentrated $H_{2} S O_{4}$ , a red gas is evolved. The gas when passed in an aq NaOH solution turns it yellow
Compound (A) and (B) are identified as $F e S O_{4}$ and $B a C l_{2}$ .
If true enter 1, else enter 0.

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Solution

The compound (A) is ferrous sulphate $F e S O_{4}$ and the compound (B) is barium chloride, $B a C l_{2}$ .
(i) On strongly heating, ferrous sulphate forms ferric oxide, sulphur dioxide and sulphur trioxide.
$2 F e S O_{4} ⟶ F e_{2} O_{3} + S O_{2} + S O_{3}$
(ii) Ferrous sulphate reacts with sodium hydroxide solution to form green ferrous hydroxide.
$F e S O_{4} + 2 N a O H ⟶ F e O H_{2} g r e e n ↓ + N a_{2} S O_{4}$
On exposure to air, ferrous ions are oxidized to ferric ions.
$2 F e (O H)_{2} + H_{2} O + O_{2} (a i r) ⟶ 2 F e (O H)_{3} ↓$
(iii) Green colour to flame is due to presence of Ba(II) ions.
Barium chloride does not form precipitate with hydrogen sulphide.
(V) barium chlorid gives chromyl chloride test.
$2 B a C l_{2} + {3 H}_{2} {S O}_{4} + K_{2} {C r}_{2} O_{7} Δ \to {2 C r O}_{2} {C l}_{2} y e l l o w c h r o m y l c h l o r i d e ↑ + 3 B a S O_{4} + 3 H_{2} O {C r O}_{2} {C l}_{2} + 4 N a O H {N a}_{2} {C r O}_{4} y e l l o w s o d i u m c h r o m a t e + 2 N a C l + 2 H_{2} O$

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