$a)$ The ionic product of the solution obtained by mixing $10^{-4}\, M\, Ag ^{+}$ and $10^{-4} \,M\, Cl ^{-}$ is $10^{-8}\, M ^2$
$b)$ The ionic product of the solution obtained by mixing $10^{-5} \,M\, Ag ^{+}$ and $10^{-5} \,M \,Cl ^{-}$ is $10^{-10} \,M ^2$
$C)$ The ionic product of the solution obtained by mixing $10^{-6}\, M \,Ag ^{+}$ and $10^{-6}\, M\, Cl ^{-}$ is $10^{-12} \,M ^2$
$d)$ The ionic product of the solution obtained by mixing $10^{-10} \,M\, Ag ^{+}$ and $10^{-10}\, M \,Cl ^{-}$ is $10^{-20}\, M ^2$
Since $10^{-8} \,M ^2\,>\,1.8 \times 10^{-10}$, hence option $(a)$ is correct.
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${A_2}B(g) \to {A_2}(g) + B(g);\,\,\,\Delta {H^o} = 40\,kJ/mol$
${A_2}B(g) \to A(g) + AB(g);\,\,\,\Delta {H^o} = 50\,kJ/mol$
.....$ kJ/mol$
