Read the following statements:
(i) A white amorphous powder (A) on strongly heating gives a colourless non-combustile gas (B) and solid (C).
(ii) The gas (B) turns lime water milky and turbidity disappear with the passage of excess of gas.
(iii) The solution (C) in dilute HCl gives a white precipitate with an aqueous solution of $K_4\left[Fe\right(CN{)}_6]$.
(iv) The solution of (A) gives a white precipitate (D) on pasiing $H_{2}S$ in presence of excess of $N{H}_{4}OH$.
Compound (A) to (D) are identified as:
(A) : $ZnC{O}_3$ (B) : $C{O}_2$, and (C) : $ZnO$, and (D) : $ZnS$
If true enter 1, else enter 0.

Q. A white amorphous powder (A) when heated gives a colourless gas (B), which turns lime water milky and the residue (C) which is yellow when hot but white when cold. The residue (C) dissolves in dilute HCl and the resulting solution gives a white precipitate on addition of potassium ferrocyanide solution. (A) dissolves in dilute HCl with the evolution of a gas which is identical in all respects with (B). The solution of (A) as obtained above gives a white precipitate (D) on addition of excess of $N{H}_{4}OH$ and on passing $H_{2}S$. Another portion of this solution gives initially a white precipitate (E) on addition of NaOH which dissolves in excess of it. Compounds (A) to (D) are identified as:
(A) : $ZnC{O}_3$, (B) : $C{O}_2$, (C) : $ZnO$, (D) : $ZnS$ and (E) : $Zn(OH{)}_2$
If true enter 1, else enter 0.

Q. A white amorphous powder $A$ on heating yields a colorless, noncombustible gas $B$ and a solid $C$. The latter compound assumes a yellow color on heating and changes to white on cooling. $C$ dissolves in dilute hydrochloric acid and the resulting solution gives a white precipitate with $K_{4}Fe(CN{)}_6$ solution. Dissolves in dilute $HCl$ with the evolution of gas, which is identical in all respect with $B$. The gas $B$ turns lime water milky, but the milkiness disappears with the continuous passage of gas. The solution of $A$ as obtained above gives a white precipitate $D$ on the addition of an excess of $N{H}_{4}OH$ and passing $H_{2}S$. Another portion of the solution gives initially a white precipitate $E$ on the addition of $NaOH$ solution, which dissolves on further addition of the base.

Q. An aqueous solution of salt (A) gives a white crystalline precipitate (B) with NaCl solution. The filtrate gives a black precipitate (C) when $H_{2}S$ is passed through it. Compound (B) dissolves in hot water and the solution gives yellow precipitate (D) on treatment with potassium iodine and on cooling. The compound (A) does not give any gas with dilute HCl but liberates a reddish brown gas on heating. Compounds (A) to (D) are identified as:

Q. (i) A black mineral (A) on heating in presence of air gives a gas (B).
(ii) The mineral (A) on reaction with dilute $H_{2}S{O}_4$ gives a gas (C) and solution of a compound (D).
(iii) On passing gas (C) into an aqueous solution (B), a white turbidity is obtained.
(iv) The aqueous solution of compound (D) on reaction with potassium ferricyanide gives a blue compound (E).

Q. A white powder $A$ on heating gave a non-combustible gas and a white residue. The residue on heating turns yellow. The residue dissolves in dilute $HCl$ and the solution gives a white precipitate with $K_4\left[Fe\right(CN{)}_6]$. Compound $A$ is: