When a mixture of NaCl,K_{2}Cr_{2}O_{7} and c | vedclass

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(C) $X$ is $CrO_{2}Cl_{2}$ and $Y$ is $Na_{2}CrO_{4}$.When a mixture of $NaCl$,$K_{2}Cr_{2}O_{7}$ and conc. $H_{2}SO_{4}$ is heated in a dry test tube

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$CrO_{2}Cl_{2}$ and $Na_{2}CrO_{4}$

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(C) $X$ is $CrO_{2}Cl_{2}$ and $Y$ is $Na_{2}CrO_{4}$.When a mixture of $NaCl$,$K_{2}Cr_{2}O_{7}$ and conc. $H_{2}SO_{4}$ is heated in a dry test tube,a red vapour $(X)$,$CrO_{2}Cl_{2}$ (chromyl chloride),is evolved.This vapour $CrO_{2}Cl_{2}$ reacts with an aqueous solution of $NaOH$ to form $Na_{2}CrO_{4}$ (sodium chromate),which is yellow in color.The chemical reactions are as follows:$4Cl^{-} + Cr_{2}O_{7}^{2-} + 6H^{+} \longrightarrow 2CrO_{2}Cl_{2} (X) + 3H_{2}O$$CrO_{2}Cl_{2} + 4OH^{-} \longrightarrow CrO_{4}^{2-} + 2Cl^{-} + 2H_{2}O$The resulting $CrO_{4}^{2-}$ ions in the presence of $Na^{+}$ ions form $Na_{2}CrO_{4} (Y)$.

List-$I$ (Aquated Ion)	List-$II$ (Colour)
$A. Ni^{2+}$	$I. \text{Violet}$
$B. Fe^{3+}$	$II. \text{Blue}$
$C. Mn^{3+}$	$III. \text{Yellow}$
$D. V^{4+}$	$IV. \text{Red}$
	$V. \text{Green}$

When a mixture of $NaCl$,$K_{2}Cr_{2}O_{7}$ and conc. $H_{2}SO_{4}$ is heated in a dry test tube,a red vapour $(X)$ is evolved. This vapour $(X)$ turns an aqueous solution of $NaOH$ yellow due to the formation of $Y$. $X$ and $Y$,respectively,are

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List-$I$ (Aquated Ion) List-$II$ (Colour)

$A. Ni^{2+}$ $I. \text{Violet}$

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$C. Mn^{3+}$ $III. \text{Yellow}$

$D. V^{4+}$ $IV. \text{Red}$

$V. \text{Green}$

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