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(D) The decomposition reactions at $500 \ ^oC$ are as follows:$(I)$ $K_2CO_3(s) \xrightarrow{\Delta} 	ext{No reaction}$. Thus,$x_1 = 0$.$(II)$ $2NaHC

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$x_1 = x_2  x_4$

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(D) The decomposition reactions at $500 \ ^oC$ are as follows:$(I)$ $K_2CO_3(s) \xrightarrow{\Delta} 	ext{No reaction}$. Thus,$x_1 = 0$.$(II)$ $2NaHCO_3(s) \xrightarrow{\Delta} Na_2CO_3(s) + H_2O(g) + CO_2(g)$. For $n$ moles of $NaHCO_3$,we get $n$ moles of gaseous products.$(III)$ $MgCO_3(s) \xrightarrow{\Delta} MgO(s) + CO_2(g)$. For $n$ moles of $MgCO_3$,we get $n$ moles of gaseous products.$(IV)$ $2CsHCO_3(s) \xrightarrow{\Delta} Cs_2CO_3(s) + H_2O(g) + CO_2(g)$. For $n$ moles of $CsHCO_3$,we get $n$ moles of gaseous products.Comparing the pressure generated: $x_1 = 0$. Since $NaHCO_3$ and $CsHCO_3$ decompose to produce $2$ moles of gas per $2$ moles of reactant,and $MgCO_3$ produces $1$ mole of gas per $1$ mole of reactant,the pressure depends on the extent of decomposition. $MgCO_3$ decomposes more easily than alkali metal bicarbonates at this temperature. Thus,$x_1  x_4$ is not present. Re-evaluating: $x_1=0$. $NaHCO_3$ and $CsHCO_3$ produce $1$ mole of gas per mole of reactant. $MgCO_3$ produces $1$ mole of gas per mole of reactant. However,$MgCO_3$ is thermally less stable than alkali carbonates/bicarbonates. Therefore,$x_1  x_4$.

List-$I$	List-$II$
$A$. Chlorophyll	$I$. $Na_2CO_3$
$B$. Soda ash	$II$. $CaSO_4$
$C$. Dentistry,Ornamental work	$III$. $Mg^{2+}$
$D$. Used in white washing	$IV$. $Ca(OH)_2$

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Match List-$I$ with List-$II$.

List-$I$ List-$II$

$A$. Chlorophyll $I$. $Na_2CO_3$

$B$. Soda ash $II$. $CaSO_4$

$C$. Dentistry,Ornamental work $III$. $Mg^{2+}$

$D$. Used in white washing $IV$. $Ca(OH)_2$

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