Question

Thermal decomposition of a $Mn$ compound (X) at $513\, K$ results in compound $Y, MnO_2$ and a gaseous product. $MnO_2$ reacts with $NaCl$ and concentrated $H_2SO_4$ to give a pungent gas $Z. X, Y$ and $Z$, respectively.

• A. $K_2MnO_4, KMnO_4$ and $SO_2$
• B. $ K2MnO_4, KMnO_4$ and $ Cl_2$
• C. $K_3MnO_4, K_2MnO_4$ and $ Cl_2$
• D. $KMnO_4, K_2MnO_4$ and $ Cl_2$

Answer 1

Answer: (D)

$\underset{\text{ (X) }}{ 2KMnO_4 } \xrightarrow[\Delta]{513\, K} \underset{\text{ (Y)}}{ K_2MnO_4 }+ MnO_2 + O_{2(g)} $
$ MnO_2 + 4NaCl + 4H_2SO_4 \rightarrow MnCl_2 + 4NaHSO_4 + 2H_2O + \underset{\text{ 1000 (Z) pungent gas }}{ Cl_{2(g)}}$