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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,$x_1  x_4$.

Compound	Percentage proportion
$1. CaO$	$d. 50-60\%$
$2. Al_2O_3$	$a. 5-10\%$
$3. SO_3$	$b. 1-3\%$

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